Fun Science Projects & Experiments - Limewater Test
In these lessons, we shall learn the limewater test for carbon dioxide - how it works and how to use it.
Related Pages Alkane And Alkene Tests Science projects, videos and experiments for various grades and topics.
Science Projects or Science Experiments: Grades 5 & 6
The following diagrams show the test for Carbon Dioxide. Carbon Dioxide will turn limewater (calcium hydroxide) cloudy. Scroll down the for examples and explanations.
Limewater Test - To check for carbon dioxide in your breath
Lime Water Breath Experiment Using lime water is a fun and easy way to test for the presence of carbon dioxide. The exhaled carbon dioxide is used to produce a precipitate of calcium carbonate with the lime water.
Bubble room air through one beaker for one minute using a pipette and pipette pump. Observe and record the results.
With the other beaker, bubble exhaled air through the solution for 1 minute. Try to bubble the air through the same rate that you did with the first beaker. After 1 minute record your results.
Limewater & CO 2 Carbon dioxide dissolves in water to form carbonic acid (H 2 CO 3 ).
Lime water is a solution of calcium hydroxide (Ca(OH) 2 ).
They react to form calcium carbonate (CaCO 3 ) and water. Calcium carbonate is insoluble and forms a white precipitate.
If CO 2 continues to be passed, more carbonic acid forms, which then reacts with the calcium carbonate to form calcium hydrogencarbonate, which is soluble, so the precipitate is seen to dissolve.
To Investigate the Carbon Dioxide Levels of Inhaled and Exhaled Air In this experiment we will investigate the carbon dioxide levels of inhaled and exhaled air. We use limewater to test for the presence of carbon dioxide.
Carbon dioxide dissolves in water Here is some pure water, which has a pH of 7, shown by using this testing paper and matching the color to the chart on the side of the box.
If I take a straw and blow into the water, what gases are going into the water?
The one I am interested in is carbon dioxide, which can dissolve in water and react to form an acid. CO 2 (g) + H 2 O(l) → H 2 CO 3 (aq) → H + (aq) + HCO 3 − (aq)
So after I blow into the water several times, I should have a solution which is more acid than it was before. Let’s check by retesting the pH of the solution. It is now down to 5, rather than the 7 it was as pure water. pH 5 is an acid, so the carbon dioxide has dissolved in the water and reacted.
Thus my chemical reaction really has made hydrogen ions in the water, meaning that the carbon dioxide gas dissolved and reacted.
CO 2 (g) + H 2 O(l) → H + (aq) + HCO 3 − (aq)
What does this mean about rain which passes through air with CO 2 in it?
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Science project, the limewater carbon dioxide test.
Carbon dioxide , also commonly known by its chemical formula CO 2 , is one of the major building blocks of life. It is usually found in its gaseous form, and is a major part of the plant and animal life cycle. CO 2 is consumed by plants in photosynthesis and is produced by animals (like us!) during respiration. It is also expelled from the earth’s core during volcanic eruptions and exits a vehicle’s engine from its tailpipe when the motor is running. It’s considered a greenhouse gas, one of several compounds which contributes to global climate change. Carbon dioxide is all around us, and this simple experiment will help you see CO 2 production by conducting a carbon dioxide test with two chemical reactions.
How can we test for the presence of carbon dioxide?
Container with lid (a plastic food container would work fine)
Distilled water
Calcium oxide (lime)
¼ cup measuring cup
White vinegar
Small shallow dish (a baby food jar or a salad dressing cup work great)
2 clear water bottles
Modeling clay
2 bendy straws
Toilet paper
Baking soda
Take the container with a lid and add 1L of distilled water and 1 teaspoon of calcium oxide. Stir with the spoon.
Let the solution sit overnight. This will be your limewater. Why do we refer to it as limewater?
Fill the small, shallow dish with limewater.
Take modeling clay and mold it into a ring just below the bendable part of your straw.
Add ¼ cup of water and ¼ cup of white vinegar into the water bottle.
Take 1 square of toilet paper and spread some baking soda in the middle of the paper. Roll it up and twist the ends of the toilet paper so the baking soda does not spill out.
Drop of the baking soda in the toilet paper into the water bottle.
Immediately insert the end of the straw into the water bottle, making sure that it is submerged in the liquid. Use the modeling clay to seal the straw into the neck of water bottle.
Bend the end of the straw and submerge it in your container of limewater.
Observe what happens. Record your observations.
Add ¼-cup of limewater to another clear water bottle.
Make a second modeling clay plug around your second bendy straw and insert the straw and plug into the water bottle.
Take a deep breath and exhale into the straw so your breath goes into the limewater. Be careful not to suck any lime water up!
Record your observations.
When carbon dioxide, CO 2 , enters the limewater, the limewater becomes cloudy. When you exhale into the bottle, the limewater will turn cloudy.
Chemists refer to baking soda as sodium bicarbonate , a compound with the chemical formula NaHCO 3 . Vinegar is a mixture of acetic acid (CH 3 COOH) and water (H 2 0). When the two are combined, the following reaction takes place:
NaHCO 3 + HC 2 H 3 O 2 → NaC 2 H 3 O 2 + H 2 O + CO 2
But this is known to happen in two steps:
NaHCO 3 + HC 2 H 3 O 2 → NaC 2 H 3 O 2 + H 2 CO 3,
...where carbonic acid is formed, and finally
H 2 CO 3 → H 2 O + CO 2,
...where carbonic acid breaks down into water and CO 2 . The CO 2 then bubbles up through the straw and into the limewater.
Limewater is created with calcium hydroxide , or Ca(OH) 2 . Named for the mineral, not the fruit, lime reacts with CO 2 in water to form calcium carbonate , which is white and does not dissolve in water, causing the water to turn cloudy.
Similarly, when we exhale we are removing CO 2 from our bodies, so breathing CO 2 into the lime water will produce the same reaction, though probably not as quickly due to the smaller amount of CO 2 in your breath.
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How Do a CO₂ Test: Detect & Analyze Carbon Dioxide Gas
Last Updated: August 2, 2024 Fact Checked
Preparing a Sample for CO₂ Testing
Testing for Carbon Dioxide with Limewater
Testing for Carbon Dioxide with a Lit Splint
Expert Q&A
Things you'll need.
This article was co-authored by Meredith Juncker, PhD . Meredith Juncker is a PhD candidate in Biochemistry and Molecular Biology at Louisiana State University Health Sciences Center. Her studies are focused on proteins and neurodegenerative diseases. There are 7 references cited in this article, which can be found at the bottom of the page. This article has been fact-checked, ensuring the accuracy of any cited facts and confirming the authority of its sources. This article has been viewed 381,701 times.
Carbon dioxide (CO 2 ) is colorless and odorless, so you can't detect it through direct observation. You'll need to collect an air sample (or a CO 2 sample), then run one of several simple tests to identify the presence of the gas. You can bubble the gas through limewater, or you can hold a lit splint into the sample to see if it is extinguished by the presence of CO 2 .
Testing for Carbon Dioxide
Collect a sample of CO 2 in a sealed test tube. Then, bubble the gas through a limewater (1 teaspoon (4.9 mL) calcium hydroxide diluted in distilled water). If the liquid turns milky white, CO 2 is present. Or, hold a lit splint to the sample and see if the flame goes out, indicating CO 2 .
Preparing a Sample
You can continue to collect the gas for as long as the reaction occurs.
For classroom demonstrations, you only need a small amount of hydrochloric acid, which is diluted to 1 M; a 2 M concentration works best, but should be used with extra care because it's a strong acid. The equation is: CaCO 3 (s) + 2HCl(aq) ==> CaCl 2 (aq) + H 2 O(l) + CO 2 (g).
Be very careful when working with hydrochloric acid – wear gloves, a lab coat, and protective goggles, and do not let the acid touch your skin! It's best to only perform this reaction if you have access to a lab environment. [2] X Research source
Bubbling Through Limewater
Limewater is also called "white wash" or "milk of lime." If you see these terms, you'll know they mean limewater. [5] X Research source
Put 1 teaspoon (4.9 mL) of calcium hydroxide into a clean 1 gallon (3.8 L) or smaller glass jar. Limewater is a saturated solution, which means there will be some extra chemical that doesn't dissolve. A teaspoon will result in a fully saturated solution, whether you use a gallon jar or a smaller container.
Fill the jar with distilled water. It's best to use distilled water for this experiment, as it will give you a purer solution.
Put a lid on the jar. Shake the solution vigorously for 1-2 minutes, then let it stand for 24 hours.
Pour the clearer solution off the top of the jar through a clean coffee filter or filter paper. Be very careful not to stir up the sediment. If necessary, repeat this filtering step until you obtain a clear limewater solution. Store in a clean jar or bottle.
If you don't want to boil anything, you can use a gas syringe to discharge the CO 2 gas directly into the half-filled limewater test tube. Stopper the test tube, then shake vigorously for 1-2 minutes. If there is carbon dioxide in the sample, then the solution should grow cloudy. [6] X Research source
CO 2 + H 2 O ==> H 2 CO 3 (carbon dioxide + water = carbonic acid)
Calcium hydrogen carbonate is soluble in water, making your solution clear!
Testing with a Lit Splint
Bear in mind that any oxygen-free gas will also extinguish a flame in this manner. Thus, this is an unreliable test for carbon dioxide, and it may lead you to misidentify the gas. [8] X Research source
To test for carbon dioxide, start by diluting some calcium hydroxide with water to make a limewater solution. Then, fill up a test tube halfway with the limewater and bring it to a boil. Next, use a delivery tube to pipe the contents of your sample into the boiling limewater. If the limewater turns cloudy and milky white, your sample has carbon dioxide in it. If no change occurs, there's no carbon dioxide in the sample. To learn how to collect a carbon dioxide sample, keep reading! Did this summary help you? Yes No
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Date
10 November 2009 by Quest 2, to link in with of our book.
Aim
To use lime water to detect CO .
Method
Add a small amount of calcium hydroxide to a test tube and add water. Add bung and shake. Allow to settle. Decant the clear solution into a beaker: lime water.
Add about 2 cm lime water to a test tube. Blow through a drinking straw to bubble CO through the lime water solution until it goes cloudy (20-30 seconds).
Continue to bubble CO through the solution until the precipitate just disappears.
Materials & Equipment . for drinking through). Results/Observations
The lime water turned cloudy quite easily but didn't want to turn completely clear again, even after much blowing.
Conclusion . Discussion
Basically, the carbon dioxide in our breath reacts with the lime water to make a white solid, calcium carbonate (which is what limestone is made of). Blowing more carbon dioxide into the lime water turns the water acidic, which dissolves the calcium carbonate again.
When carbon dioxide dissolves in water, it forms carbonic acid.
CO (g) + H O(l) → H CO (aq)
Lime water neutralizes the carbonic acid and carbonate ion is formed.
H CO (aq) + 2 OH (aq) → CO (aq) + 4 H O(l)
Calcium carbonate is insoluble and precipitates.
Ca (aq) + CO → CaCO (s)
As still more CO is bubbled into solution, all the OH is used up, and the solution becomes acidic.
CO (g) + H O(l) → H CO (aq)
Carbonate ion is converted into bicarbonate, which has a very soluble calcium salt.
(s) + H CO (aq) → Ca (aq) + 2 HCO (aq)
In nature, calcium is a very common ion in igneous rocks. As these rocks weather and the calcium goes into solution, CO 2 in the atmosphere precipitates some of it as CaCO 3 . Found in massive sedimentary deposits, this material is called limestone. Cracks in limestone deposits allow water (containing more CO 2 ) to percolate through, dissolving part of the material and forming limestone caves. Re-precipitation of the CaCO 3 results in the formation of stalactites and stalagmites.
Tap water that is "hard" because it comes from wells and has been in contact with limestone for a long time contains relatively large amounts of calcium and bicarbonate ions. When this water is heated in coffee pots or water heaters and allowed to cool, limy deposits called "boiler scale" build up.
Experiment Refinements
If repeating the experiment, we would make the following refinements.
Prepare a more carefully controlled sample of limewater that definitely didn't have any extra solid calcium hydroxide floating around in suspension.
Leave the solution longer to settle.
Use the pipette to remove the clear solution instead of pouring it out.
After decanting, make a slightly less than saturated solution by adding a little fresh water to dissolve the last remnants of calcium hydroxide.
This will mean all the cloudiness in the lime water is caused by CO 2 .
Use a control (set aside a sample) at each stage that we can compare with so we can definitely see the change in cloudiness.
If bubbling CO 2 through the lime water doesn't completely turn it clear again, simply leave a sample exposed to the air for a few days. It may absorb enough CO 2 from the air to dissolve the suspended limestone. Shake occasionally to ensure it's not just settling.
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AQA GCSE Chemistry
Test for carbon dioxide.
To identify the presence of carbon dioxide gas in a sample, you can perform a simple experiment using limewater. Here’s what you’ll need to do:
1. Prepare two test tubes, one containing the sample gas and the other containing limewater.
Limewater is an aqueous solution of calcium hydroxide, which is calcium oxide dissolved in water.
2. Bubble the gas sample into the limewater solution.
3. Observe the limewater solution. If the limewater turns cloudy, this indicates that the sample gas contains carbon dioxide.
The limewater turns cloudy because the carbon dioxide and calcium hydroxide react to form calcium carbonate. C alcium carbonate is an insoluble white precipitate, so all the little particles make the solution appear cloudy.
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The solution will turn milky due to the fact that calcium carbonate is a white precipitate. This reaction is actually used to test for the presence of carbon dioxide.
An unknown gas is bubbled through a solution of calcium hydroxide - if the solution turns cloudy, then the unknown gas is carbon dioxide.
If you continue to bubble the carbon dioxide through the limewater another acid - base reaction occurs which results in the precipitate dissolving to give soluble calcium hydrogen carbonate:
What is the thermochemical equation for the combustion of benzene?
Why are chemical reactions reversible?
Why are chemical reactions important?
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How Does Carbon Dioxide React with Lime water?
What happens when Lime Water reacts to Carbon Dioxide?
Written as an Equation
In its equation form that makes:
How to test for carbon dioxide?
Now, we will answer how to test for carbon-dioxide. One of the most effective ways to test for carbon dioxide gas is the limewater test. When carbon dioxide reacts with lime water (calcium hydroxide solution), a white precipitate of calcium carbonate is produced. The solution of calcium hydroxide is limewater and if carbon dioxide bubbles through the limewater, it turns cloudy white or milky.
How does carbon dioxide turns lime water milky?
Now, the question arises why the solution turns milky. Well, the answer is simple, The reason for the milky solution is that calcium carbonate which is produced as a result of this reaction is a white precipitate. This nature of calcium carbonate also helps us to test for the presence of carbon dioxide gas. All you have to do is to bubble the gas through a solution of calcium hydroxide. If the gas is carbon dioxide, then the solution will turn milky. If not then the gas which is subjected to the test is not carbon dioxide. If you continue to bubble the carbon dioxide gas through limewater, you will witness another acid-base reaction that will dissolve the precipitate to generate soluble calcium hydrogen carbonate. The equation of this reaction is given below:
What is the reaction between carbon dioxide and water?
Since it is a weak acid, therefore some of it dissociates to generate H+ ions. This depicts it is a slightly acidic solution that forms hydro carbonate ion.
All of these reactions are reversible.
Does lime water absorb carbon dioxide?
Yes, limewater absorbs carbon dioxide. When lime water and carbon dioxide reacts, calcium carbonate is generated along with the water. Calcium carbonate is an insoluble salt. The equation of this reaction is given below:
Why is lime water used in experiments?
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A photon interacts with a ground state electron in a hydrogen atom and is absorbed.
I have all of the answers except this one........... A photon interacts with a ground state electron in a hydrogen atom and is absorbed. The electron is ejected from the atom and exhibits a de Broglie wavelength of 5.908×10−10 m. Determine the frequency (in hz) of the interacting photon.
anyone want to help?
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Chemistry help
Sulfur vapor is analyzed by photoelectron spectroscopy (PES). Measurements determine that photoelectrons associated with the 1st ionization energy of sulfur move with de Broglie wavelength λ=5.091 A˚. What is the maximum wavelength (in meters) of radiation capable of ionizing sulfur and producing this effect?
Gas phase reaction help
The gas-phase reaction between trichloromethane, CHCl3, and chlorine, Cl2, has time-independent stoichiometry and can be represented as follows:
Equation 1 CHCl3(g) + Cl2(g) = CCl4(g) + HCl(g)
Under certain experimental conditions, the experimental rate equation was found to be:
Equation 2 J = kR[CHCl3][Cl2]^1/2
A three-step mechanism has been proposed for Reaction 1:
Equation 3 k1 Cl2 ↔ 2Cl• k-1
Equation 4 k2 CHCl3 + Cl• → HCl + CCl3•
Equation 5 k3 CCl3 + Cl• → CCl4
(i) Explain why the form of the experimental rate equation indicates that Reaction 1 cannot be an elementary reaction.
(ii) With reference to the three-step mechanism (Equations 3–5 ), and assuming that the second step (Equation 4) is rate-limiting, derive the chemical rate equation for this mechanism and then compare it with the experimental rate equation given in Equation 2.
(iii)The activation energy for the forward reaction, Ef , of step 1 (Equation 3) is 243.4 kJ mol^-1. Given this information, determine the activation energy for the reverse reaction, Er, and comment on the significance of the value (one sentence only).
Help Help Help
You wish to increase the carbon content of a slab of steel by exposing it to a carburizing atmosphere at elevated temperature. The carbon concentration in the steel before carburization is 359.5 ppm and is initially uniform through the thickness of the steel. The atmosphere of the carburizing furnace maintains a carbon concentration of 6695.0 ppm at the surface of the steel. Calculate the time required to carburize steel so that the concentration of carbon at a depth of 38.0 x 10-2 cm is one half the value of the carbon concentration at the surface. The diffusion coefficient of carbon in steel is 3.091 x 10-7 cm2/s at the carburizing temperature. Express your answer in hours.
DATA: Error Function Values erf(ξ
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How does copper oxide and sulphuric acid react to eachother?
Reacting Copper Oxide with Sulphuric Acid
Writing the Equation form of Copper oxide + Sulphuric Acid
This chemical reaction can be written as the following:
Copper oxide(solid) + Sulphuric Acid (aqueous)-> Copper Sulphate (aqueous)+ Water(liquid) To find out how you can make Copper Sulphate at home check out this article.
What happens when the copper reacts with concentrated Sulphuric acid?
The reduction potential of diluted sulphuric acid is higher than that of hydrogen. Copper is unable to displace hydrogen from non-oxidizing acids, for instance, hydrochloric acid or diluted sulphuric acid. In other words, we can say that the copper does not react with the diluted sulphuric acid. However, it does react with the concentrated sulphuric acid because sulphuric acid in concentrated form is an oxidizing agent. When copper gets heated with concentrated sulphuric acid, there is a redox reaction and the acid turns into sulfur dioxide. The equation of this chemical reaction is given below:
What is the balanced equation for copper oxide and Sulphuric acid?
The copper oxide and sulphuric acid balanced equation is given below:
Why do copper oxide and Sulphuric acid turn blue?
We all know that the copper oxide + sulfuric acid reaction results in a blue-colored chemical. But have you ever wondered why copper oxide sulphuric acid reaction results in a blue-colored chemical? Well, we will answer this question in detail here. Copper oxide is a black-colored solid. When it reacts with sulphuric acid, it produces a cyan-blue colored chemical which is known as copper sulphate. The blue color is due to the formation of soluble salt. The copper and sulphate ions dissociate as the copper sulphate gets dissolved in water. Although there is no change in the effect, however, the nature of the split between t2g and eg orbitals in this new complex is such that it absorbs reddish-orange light. Due to this absorption, you will see a bluish-colored solution.
Does sulfuric acid dissolve copper?
No, sulphuric acid cannot dissolve the copper. However, if dissolution is observed, it can be due to one of the following two reasons:
The formation of a vortex during the agitation. A tiny amount of air (oxygen) that was introduced to a leach solution acted like an oxidant.
What salt is produced when copper oxide reacts with hydrochloric acid?
The reaction of copper and hydrochloric acid is not possible. However, copper oxide can react with this acid. When a metal reacts with an acid, a redox reaction occurs. Because of the higher reduction potential of copper as compared to hydrogen, it is unable to react with non-oxidizing acids like sulphuric acid and hydrochloric acid.
But copper oxide is not a metal, rather it is a metal oxide. Metal oxides are basic substances that can react with acids to form salt and water. These acid-base reactions are also known as neutralization and are non-redox in nature.
Being a weak base, copper oxide reacts with HCL easily to generate a soluble copper chloride and water. The equation of this chemical reaction is given below:
Main Group Elements- Reaction Between Carbon Dioxide and Limewater
Reaction Between Carbon Dioxide and Limewater
Description: Carbon dioxide gas bubbling through limewater produces a precipitate. Sources of carbon dioxide include exhaled breath, Alkaseltzer® tablets, or dry ice. The precipitate will redissolve if the concentration of carbon dioxide is high enough.
Source: Shakhashiri, B.Z. Chemical Demonstrations: A Handbook for Teachers of Chemistry
Procedures with some intermediate steps to results
Safety Precautions:
Eye protection required
Gloves required
Avoid inhalation or ingestion
Absorbent materials on hand
Perform in a well-ventilated area
Class: Aqueous Equilibrium and Precipitation Reactions, Main Group Elements
Division: General
Home| General Chemistry Demos
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Identifying the products of combustion
In association with Nuffield Foundation
No comments
Illustrate the presence of water and carbon dioxide in the products of hydrocarbon combustion in this demonstration
In this experiment, students observe as the teacher burns a solid hydrocarbon (in the form of a tea light or candle), using a pump to divert the gaseous combustion products. These substances are then drawn by the pump over a piece of cobalt chloride paper and through limewater, with changes indicating the presence of water and carbon dioxide respectively.
With this demonstration, the apparatus can be left running for some time and students can file past in small groups to see it more closely. Alternatively a flexicamera can be used, linked to a projector.
If students are not familiar with the cobalt chloride paper and limewater tests, either demonstrate these separately or allow students to try the tests themselves.
Assuming everything is already set up this demonstration takes only a few minutes.
Looking for a class practical?
Check out a simplified version of the experiment below, using a gas jar to collect the products of combustion , which is suitable for students to carry out themselves.
Eye protection
Glass funnel, about 6 cm in diameter
Boiling tubes, x2
Two-holed rubber bungs, x2, to fit the boiling tubes, and fitted with one long and one short piece of glass tubing (see diagram)
Glass or plastic tubing for connections (see note 5 below)
Filtering pump (see note 6)
Tea light, night light or candle
Piece of blue cobalt chloride paper (TOXIC)
Limewater (treat as IRRITANT), about 20 cm 3
Health, safety and technical notes
Read our standard health and safety guidance.
Wear eye protection throughout.
Cobalt chloride/cobalt chloride paper (TOXIC, DANGEROUS TO THE ENVIRONMENT) – see CLEAPSS Hazcard HC025 and CLEAPSS Recipe Book RB030. Cobalt chloride paper can be stored in a desiccator. Minimise handling of cobalt chloride paper (SENSITISER) and wash hands after use (cobalt chloride is a category 2 carcinogen). See the standard procedure for preparing and using cobalt chloride papers for more information.
Calcium hydroxide solution, ‘limewater’, Ca(OH) 2 (aq), (treat as IRRITANT) – see CLEAPSS Hazcard HC018 and CLEAPSS Recipe Book RB020. Ideally, the limewater should be made fresh on the day.
Source: Royal Society of Chemistry
Connect the funnel to two test tubes, one containing cobalt chloride paper and the other containing limewater
Care should be taken with the right-angle bend connected to the funnel. If this is made of flexible tubing, it can get hot and melt. Ideally, the glass stem of the funnel should be bent into a right-angle. Alternatively, join a standard funnel onto a right angled piece of glass tubing using epoxy resin. A more temporary arrangement is to slide one arm of a right-angled piece of glass tubing inside the stem of the funnel and seal the join on the outside with a piece of flexible tubing (see diagram).
How to set up and seal a right-angled bend connected to the funnel
Information about the type and use of various grades of filter papers can be found in section 9.11.4 of the CLEAPSS Laboratory Handbook. The use of traditional water-operated filter pumps for vacuum filtration and for drawing air through solutions is covered in section 10.6.4 of the CLEAPSS Laboratory Handbook. It is strongly recommended that this is referred to before purchasing or using such pumps – it may not be possible or appropriate to use this type of equipment in your school or college. Alternative means of carrying out vacuum filtration and drawing air through solutions are suggested in this section of the Laboratory Handbook .
Before the demonstration, assemble the apparatus as shown in first diagram above. Ensure that the connections to the boiling tubes are the correct way round.
Place a piece of blue cobalt chloride paper into the first boiling tube and half-fill the second boiling tube with limewater.
At the start of the demonstration, turn on the pump so that a gentle stream of air is drawn through the apparatus.
Light the tea light and leave for a few minutes until the cobalt chloride paper turns pink (from blue) and the limewater goes milky (produces a white precipitate). This indicates the presence of water and carbon dioxide respectively.
Teaching notes
Some students will know that air contains both water vapour and carbon dioxide. To show that the changes observed are not due to these alone, repeat the experiment without the tea light and note how much longer it takes for any changes to be observed.
Understanding the process of burning is important at all levels of chemistry. Emphasis that burning in air is a reaction with oxygen. The elements hydrogen and carbon are present in hydrocarbons, such as candle wax. Students will quite readily appreciate that carbon reacts with oxygen to form carbon dioxide, but often need help to grasp that hydrogen combines with oxygen to form water.
The production of carbon dioxide could lead to discussion of the role of this gas in the greenhouse effect.
The experiment could be extended to burning alcohols with a spirit burner.
Try this simplified class practical
In this alternative version of the experiment above, students burn a candle inside a gas jar, before testing for the presence of carbon dioxide and water.
Student sheet
Download the accompanying student sheet as a PDF or editable Word document .
Gas jar and lid
Candle on a tray
Heat resistant mat
Limewater (treat as IRRITANT), 0.02 mol dm –3
See notes 1–4 in the health and safety guidance above.
Set up the apparatus as shown in the diagram. The gas jar should be placed over the lit candle on a heatproof mat.
When the candle goes out, put a lid on the gas jar.
Test to see if the candle made water by adding a piece of blue cobalt chloride paper, test the sides of the jar. If it turns pink, water is present. Record what you observe.
Now test to see if carbon dioxide was produced. Pour a little limewater into the gas jar. Swill it around a little. If carbon dioxide is present, the limewater turns cloudy. Record what you observe.
Questions for students
What is the gas that reacts with the hydrocarbon when it burns?
What gases does the candle produce when it burns?
Name another fuel that produces the same gases when it burns.
Carbon dioxide and water.
Methane or similar hydrocarbon or fuel.
Teaching tips
As an extension, the students could suggest other experiments to do to find out if other fuels form carbon dioxide and water when they burn.
Data logging sensors and software can be used to demonstrate what may be happening in the jar as the candle burns. Use a bell jar and place sensors inside to monitor humidity, temperature, light or oxygen levels as the candle burns. The software will show the changes as a graph against time. When the candle extinguishes, readmit air to the jar and continue to record for a few moments.
Identifying the products of combustion - student sheet
Additional information.
This is a resource from the Practical Chemistry project , developed by the Nuffield Foundation and the Royal Society of Chemistry.
Practical Chemistry activities accompany Practical Physics and Practical Biology .
The experiment is also part of the Royal Society of Chemistry’s Continuing Professional Development course: Chemistry for non-specialists .
The simplified version of this resource also previously appeared as part of our Classic chemistry experiments collection.
The combustion of hydrocarbon fuels releases energy. During combustion, the carbon and hydrogen in the fuels are oxidised. The complete combustion of a hydrocarbon produces carbon dioxide and water.
8.7 Describe the complete combustion of hydrocarbon fuels as a reaction in which: carbon dioxide and water are produced; energy is given out
C3.4.18 predict the formulae and structures of products of reactions (combustion, addition across a double bond and oxidation of alcohols to carboxylic acids) of the first four and other given members of these homologous series
Hydrocarbons and alcohols burn in a plentiful supply of oxygen to produce carbon dioxide and water.
(f) the combustion reactions of hydrocarbons and other fuels
2.3.4 describe the complete and incomplete combustion of alkanes in air and link the appearance of the flame to the amount of carbon present;
2.5.9 describe the complete combustion of alkanes to produce carbon dioxide and water, including observations and tests to identify the products.
1.8.15 describe how to test for carbon dioxide: limewater (calcium hydroxide solution) will change from colourless to milky if the test is positive; and
1.8.14 describe how to test for carbon dioxide: limewater (calcium hydroxide solution) will change from colourless to milky if the test is positive; and
Combustion of alkanes and other hydrocarbons.
7. Investigate the effect of a number of variables on the rate of chemical reactions including the production of common gases and biochemical reactions.
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Signs of Chemical Changes: Testing for CO2, O2, and H2
When chemistry or physical science students initially learn about chemical changes and chemical reactions, they are taught to look for evidence of the change or reaction. Chemical changes, or reactions, are the result of breaking bonds in the starting substances, called reactants , and the rearrangement of those substances and bonds to make new substances, called products .
The rearrangement of reactants into products is usually accompanied by some type of observable or measurable indicator. Students often look for:
Color changes
Temperature changes
Formation of a solid product or precipitate
Production of heat
Production of light
Bubbles indicating gas formation
Presenting students a variety of reactions, with easily observable indicators, encourages them to develop and use a predictive model of reaction types. Carolina ChemKits®: Types of Chemical Reactions provides students with reliable, safe examples of chemical reactions and guides them through the process of predicting the reaction products. With practice, students become adept at analyzing observable indicators to identify the different types of chemical reactions.
Carbon Dioxide
Reactions that produce carbon dioxide gas.
As students move through the reaction identification process, they should associate the production of bubbles with the production of a gaseous product. Refinement of reaction type models can help students identify the actual gaseous product. Since the production of carbon dioxide in biological processes like respiration and the chemical weathering reactions of minerals like calcite may already be familiar to students, we will look at reactions that produce carbon dioxide first.
Examples of reactions that produce CO 2
Decomposition of metallic carbonates M = reactive metal MCO 3 → MO + CO 2 (g)
Decomposition of metallic hydrogen carbonates or metallic bicarbonates MHCO 3 → MCO 3 + H 2 O + CO 2 (g)
Combustion of a hydrocarbon C x H y + O 2 → H 2 O + CO 2 (g)
Students should recognize the relationship between the carbonate ion (CO 3 2- ), its chemical stability, and the production of carbon dioxide gas. If you need additional cross-curricular activities, you may want students to:
Investigate how the production of carbon dioxide by algae during photosynthesis affects the pH of water using Carolina BioKits ®: Algae Bead Photosynthesis
Examine chemical weathering of limestone with Carolina Investigations® for AP® Environmental Science: Soil Formation and Properties
Reactions that produce oxygen gas
Oxygen, as a gaseous product, is formed from several different types of reactions including decomposition and photosynthesis. Again, the photosynthesis equation is a useful cross-curricular example of a reaction that produces oxygen. Earth science or geology students may be familiar with decomposition of metal oxides if they learned about mining and ore refinement. The decomposition of water through electrolysis is a tried-and-true demonstration, both for the technique and identification of the products. Students are probably familiar with hydrogen peroxide as a cleaning solution for cuts and scrapes. They may realize hydrogen peroxide decomposes in sunlight so it must be stored in a brown bottle. With a catalyst, the decomposition of the compound is rapid and makes a showstopping demonstration known as elephant toothpaste .
Examples of reactions that produce O 2
Decomposition of metallic chlorates MClO 3 → MCl + O 2 (g)
Electrolysis of H 2 O 2H 2 O → 2H 2 + O 2 (g)
Decomposition of metal oxides MO → M + O 2 (g)
Photosynthesis CO 2 + H 2 O → C 6 H 12 O 6 + O 2 (g)
Decomposition of hydrogen peroxide
2H 2 O 2 → 2H 2 O + O 2
Reactions that produce hydrogen gas
If students have chemistry experience with acids and pH, they are probably familiar with the aqueous hydrogen ion and the indicator color changes produced as the hydrogen ion concentration increases or decreases. Familiarity with the periodic table may help students recall that hydrogen is a very reactive, diatomic, lightweight gas. The explosion of the German airship Hindenburg, on May 6, 1937 in Lakehurst, New Jersey, is a great visual representation of the power and force of the combustion of hydrogen gas. Two different forms of single replacement reactions generate hydrogen gas and require that students understand the activity series of metals . In both instances, a metal reacting with water and a metal reacting with acid, the metal must be more reactive, or higher on the activity series, than diatomic hydrogen. Metals falling below hydrogen on the activity series will not react with water or acids.
Model reactions that produce H 2
Electrolysis of water 2H 2 O → O 2 + 2 H 2 (g)
Single replacement of an active metal reacting with water: M + H 2 O → MOH + H 2 (g)
Single replacement of an active metal reacting with acid: M + HX → MX + H 2 (g)
Tests to identify gases
The generation and/or collection of carbon dioxide, oxygen, and hydrogen produces bubbles. How can students tell which gas is in the bubble? The glowing splint test is widely accepted and easy to perform. Students light a small splint, like a wooden coffee stirrer, blow out the flame but leave the embers, and then place the glowing splint into the unknown gas. In carbon dioxide, the splint goes out completely. In oxygen, the splint reignites. In hydrogen, a reaction with oxygen occurs that sounds like a bark.
Hydrogen bubbled into water will increase the hydrogen ion concentration, which decreases the pH and causes acid/base indicators to change colors. Bubbling carbon dioxide through water also results in the formation of an acid (carbonic acid), and that too will decrease pH, resulting in an indicator color change. Carbon dioxide bubbled through lime water will make a milky precipitate, calcium carbonate, that is easily seen.
As students master the techniques for testing and identifying hydrogen, oxygen, and carbon dioxide gas, they can use experimental results to confirm or reject a specific reaction model. With repeated experiments and practice using equation models to predict products, students will become proficient at identifying and explaining chemical changes. They will easily isolate the key evidence to support their claim of a specific reaction model and continue to develop and refine their model of chemical changes.
For labs and materials to enhance student learning and help with model development, explore our chemistry kits.
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Crusty, Open-Crumb Baguettes
This post may contain affiliate links. Please read my disclosure policy .
Made with a no-knead, four-ingredient dough, these baguettes have an open crumb and a shatteringly crisp crust. The overall process is simple, but the key to an excellent baguette is twofold: time, which develops flavor, encourages browning, and promotes a light and airy crumb; and baking in a steamy environment, which you can create easily in your home oven. You’ll find step-by-step instructions below.
Nearly every week someone writes me asking if I have a baguette recipe. They’ll say: “I checked your bread archives and couldn’t find one, but wanted to make sure I didn’t miss anything.”
They hadn’t!
I’ve hesitated to add a baguette recipe here for a number of reasons, namely because before recently, I hadn’t had much success with them. Over the years I’ve dabbled, but I’ve found the process discouraging from the shaping (requiring very practiced hands) to the equipment (couches, lames, lava rocks) to the baking (demanding steam). Baguettes, I resigned, were best left to the professionals.
But at some point a few months ago, I rolled an extra round of pizza dough into a log, threw it in my Challenger Bread Pan , and baked it. And when it emerged golden and crusty, I felt hopeful. And when I halved it to reveal a wild amorphous crumb, I nearly cried.
Kidding. However, there is something very satisfying about producing a deeply burnished, light and airy baguette, in your own kitchen.
Since this first successful bake, I have experimented with a number of different baking methods, and in this post, I have outlined the two (actually three… see below) I’ve had the most success with: one calling for the Challenger Bread Pan or other oval-shaped Dutch oven and the other for a Baking Steel or baking stone plus a turned-over disposable aluminum pan.
What do the two methods have in common? They both use a lid for the first ten minutes of the baking process. Why? To create steam. And why is steam good? Let’s jump right in.
Warning: This post gets a little nerdy. I consulted two books, Chad Robertson’s Tartine Bread and Jeffrey Hamelman’s Bread , while writing this post. Know this: if I can get it, so can you!
Why is steam good for baguettes?
Steam is good for baguettes (and many breads, such as this simple sourdough bread recipe and Jim Lahey’s no-knead bread ) for two reasons: oven spring and crust development (both color and texture).
Let’s start with oven spring. First of all: what is oven spring? In short, oven spring is exactly as it sounds: dough springing in the oven upon entry.
Dough springs in the oven for a few reasons: 1. Increased fermentation activity, meaning as the yeasts rapidly multiply in the hot oven, the dough produces carbon dioxide gas. 2. Steam : As water in the dough evaporates it transforms into steam. Both the carbon dioxide gas and the steam push against the gluten structure, causing the dough to spring.
A moist, steamy environment allows for maximum oven spring because it allows the dough to expand to its fullest potential before a crust forms. In other words: when dough stays soft during the early phases of baking, its oven spring will be greater because it isn’t being restricted by a dry, hard crust.
And the reason we want dough to spring to its potential is because a greater spring promotes a crumb that is light and airy.
Make sense?
Now onto crust color and texture. In the early stages of baking, the rapid increase in enzymatic activity on the surface of the loaf breaks down the starches in the dough into simple sugars. These sugars ultimately contribute to crust color. In a steamy environment, the enzymes remain active for longer, leading to an even richer color.
A steamy environment will also help produce a crust with a subtle sheen. This is because, during the early stages of baking, the starches on the surface of the loaf gelatinize — meaning they swell with water, and as they break down, they form a gel. During the last 10 minutes of baking, when the lid is removed and the baguettes are baking in dry heat, that gel layer dries out, transforming into a shiny crackly crust as opposed to one that is dull and hard.
Compare the two photos below. This first one shows a baguette baked with steam:
In the below photo, the baguettes were baked on the Baking Steel without steam. In the above photo, observe the caramelization of the crust, the score differentiation, and the slight sheen. Compare it to the dry, lusterless crusts below:
Note: In my experiments, I tried using other methods to create the steamy environment: ice (adding ice cubes to a skillet placed next to the loaf during the first 10 minutes of baking) and water (pouring water into a hot skillet set next to the loaf). While both methods indeed created steam, I found them mostly ineffective in terms of creating a nice crust.
So, to recap: baking in a sealed environment is important to create steam, which is optimal for good oven spring and crust formation. But steam is not the only factor responsible for producing a baguette with a beautifully burnished crust and light and airy crumb.
Time is essential, too.
Why is time good for baguettes?
When dough rises slowly, good things happen: during a long, slow fermentation, enzymes in both the flour and the yeast break down the starches in the flour into simple sugars, which contributes both to flavor and to browning.
If you make your dough at least a day before you plan on baking it, you will see improved flavor and browning. It’s for these reasons, I always make my pizza dough two to three days before I plan on cooking it.
This dough calls for a long slow initial rise, roughly 6 to 10 hours depending on the time of year and the temperature of your kitchen. Following this first rise, you’ll ball up your four portions of dough and, ideally, store them in the fridge for a day or two for the above-mentioned reasons: time = goodness.
The beauty of this method is that you can store the dough balls in the fridge for as long as a week, and you can bake off the baguettes one at a time as needed. Unless you are baking for a lot of people, you don’t want to have lots of extra baguettes on hand — while they reheat fine on subsequent days, baguettes are best eaten the day of.
On baking day you’ll want to remove your dough three hours before you plan on baking.
All of this said, you can skip the fridge time all together — find a photo just before the recipe card at the bottom of the post that shows a baguette that experienced no fridge time: the dough was mixed Friday evening; the baguettes were baked Saturday afternoon.
Example Timeline #1: Fridge Time
Wednesday Evening: Mix Dough
Thursday Morning : Ball Up Dough, Transfer to Fridge
Friday Afternoon (or any subsequent afternoon for as long as a week): Remove Dough Ball From Fridge 3 Hours Prior to Baking
Friday Evening: Bake Baguette
Example Timeline #2: No Fridge Time
Thursday Evening: Mix Dough
Friday Morning : Ball Up Dough, Transfer to a Lidded Vessel (such as a DoughMate), Leave at Room Temperature for Two Hours.
Friday Midday: Shape the Dough Balls into Baguette Shape and Return to Lidded Vessel, Leave at Room Temperature for Roughly Two Hours More.
Friday Afternoon : Bake the Baguettes
Ready? You got this 🥖🥖🥖🥖🥖
How to Make Baguettes, Step by Step
I’ve broken down this step-by-step guide into three sections:
Part I: Mixing and Portioning the Dough
Part ii: shaping and proofing, part iii: baking.
Gather your ingredients: flour, salt, yeast, and water. I conducted most of my experiments with King Arthur Bread flour, since it is widely available and such a reliable flour. SAF instant yeast is my favorite. See notes in the recipe box regarding salt.
I also had excellent results using this Petra 0102 flour , which is made from partially sprouted wheat flour and which I love for the flavor and texture it lends to a bread or pizza.
Measure everything out, ideally with a scale :
Combine the dry ingredients together first:
Whisk them together:
Then add the water:
Mix until you have a shaggy dough ball:
Let it rest for 30 minutes or so, then stretch and fold it (see video for guidance):
Cover the bowl with an airtight lid, then let it rise at room temperature until it doubles in volume and its surface is covered in bubbles.
Using lightly floured hand, deflate the dough:
Then turn it out onto a work surface and divide it into four equal portions. I do like to use a scale to ensure each portion is identical, roughly 237 grams each.
Ball up each portion:
Transfer to storage vessels :
Then transfer to the fridge ideally for at least a day. The dough balls can stay in the fridge for as long as a week.
Shaping baguettes takes a little bit of practice, but I find using cold, refrigerated dough makes the process easy. Below you will find video and photo guidance of the process.
On baking day, turn the dough out onto a work surface. I do not use any flour here, but if you find the dough to be sticky, use flour lightly as needed.
Pat the dough into roughly a 6×7-inch rectangle:
Fold the dough from the top down:
Rotate the dough 180 degrees, and fold from the top down (also known as an “envelope” fold).
Then fold again from the top down, essentially folding the envelope in half.
Then, repeat (see video for guidance):
Pinch the seam closed.
Turn over so that the seam is down and gently roll.
Transfer to a floured, lidded storage vessel. I love these DoughMates , but you could use a large Tupperware or a 9×13-inch dish tucked inside a 2-gallon ziptop bag.
Often I’ll proof two at one time, though I try to stagger the entry of each by 30 minutes so as to avoid overproofing the dough.
Cover the container and let the dough proof for 2.5 to 3 hours or…
… until it feels very light and airy to the touch. One assessment tool you can use is the “poke” test: using a lightly floured finger, poke the dough making an indentation roughly 1/2-inch deep; if it springs back immediately, the dough needs more time; if it springs back slowly initially, but then holds a partial indentation — in other words, if it doesn’t completely refill — the dough is ready to be baked. (And if it doesn’t spring back at all, the dough is overproofed, but push on anyway, because it may bake up just fine.) I don’t love this method because I find it to be misleading: my dough behaves nearly the same way at the 2-hour mark as it does at the 3-hour mark, and yet my baguettes consistently have a lighter, airier crumb if I wait 3 hours before baking them. Nonetheless, it is a tool you can use.
When the dough is ready for baking, remove it from the DoughMate and place it on a sheet of parchment paper — I take full sheets, fold them in half lengthwise, then cut them in half.
Use a razor blade to score it.
Then bake it…
Method 1: Preheated Challenger Bread Pan . Place the Challenger or other oblong-shaped Dutch oven into an oven and preheat to 450ºF. This takes roughly 30 minutes in my oven. Lower the scored log, parchment paper and all into the preheated pan.
Cover it and return it to the oven for 10 minutes.
Uncover it, and return it to the oven for another 10 minutes…
… or until the baguette is beautifully golden brown:
Transfer to a cooling rack. Let cool for 15 minutes or so before…
… serving.
As noted above, I’ve been experimenting with Petra 0102 flour . The baguette on the left is made with Petra flour; the one on the right is King Arthur bread flour.
Left: Petra flour ; right: King Arthur bread flour.
Method 2: Baking Steel or stone. Note: This method is inspired by this post on Serious Eats . Place a Baking Steel ( the original or the pro ) or a baking stone in the middle of your oven and preheat it to 450ºF. This may take 30 or so minutes.
Score your dough:
Then shimmy it onto the hot Baking Steel or pizza stone using a peel (this is my favorite peel ).
Cover the baguette with a disposable aluminum pan (lasagna-sized) and weigh it down with something heavy enough to seal it down without collapsing it:
Bake for 10 minutes. Then remove the weight and pan.
Continue baking the baguette for another 10 minutes…
… or until it’s golden and bronzy to your liking:
Let cool for 20-ish minutes or so before halving:
A few other bakes with this method: left Petra ; right KAF bread flour.
The below pictured loaf is made with KAF bread flour, and this dough experienced no refrigeration: I mixed the dough on Friday night, portioned it and balled it up Saturday morning, let the balls rest in a DoughMate for 2 hours or so, shaped into baguettes and let rest again for another 2 hours; then baked:
Bonus Method: Covered Emile Henry Baker
I bought this Emile Henry baguette baker on a whim several years ago but it has mostly sat unused in my basement. I pulled it out to experiment because when I mentioned I had been baking baguettes in my newsletter, someone emailed me telling me she had just purchased an Emile Henry baguette baker and was looking forward to using it.
I was incredibly pleased by the results, which consistently produced a beautiful crust if slightly less crusty than the two methods outlined above. The crumb, while light, similarly isn’t as open or airy as the other two methods. That said, it’s still delicious. Moreover, a slightly smaller amount of dough might produce a lighter, airier baguette because it wouldn’t fill the baguette well so tightly.
This method is perhaps the easiest of the three in that you don’t have to preheat a vessel. For this sort of baker, simply place the baguette into the buttered well, score it, then bake covered at 450ºF for 10 minutes and then uncovered for 10 more minutes.
For its ease, this is a great option:
The crumb is the least open of the three methods, but the flavor is still great:
5 from 3 reviews
Author: Alexandra Stafford
Total Time: 48 hours 20 minutes
Yield: 4 baguettes
Diet: Vegan
Description
Adapted from the outdoor variation of the Neapolitanish pizza dough recipe from my cookbook, Pizza Night .
For best results, use a scale to measure everything.
Flour: In most of my experiments I used King Arthur Bread flour but I also got excellent results and often an even more open crumb when I used Petra 0102 Flour , which is made from partially sprouted wheat.
Salt : I use Diamond Crystal kosher salt, but you could use fine sea salt in its place. Again, for best results use a scale to measure. 16 grams of salt may seem like a lot, but the rule for bread and pizza dough is that the amount of salt should be 2 to 3% the weight of the flour. 16.5 grams is 3%; 11 grams is 2%. If you are using Diamond Crystal kosher salt, you’ll use roughly 5 teaspoons. If you are using Morton kosher salt or fine sea salt, you’ll use 2.5 teaspoons.
Yeast: SAF instant yeast is my favorite.
Plan Ahead: This recipe calls for a long slow initial rise of roughly 6-10 hours followed, ideally, by some fridge time.
Three baking tools for baguettes:
Challenger Bread Baker
Baking Steel ( the original or the pro ) + a disposable aluminum lasagna pan
Emile Henry Lidded Baguette Baker or other
Other Equipment:
Dough Storage Containers: This set of four has become a favorite.
DoughMate storage vessel
parchment paper
razor blades
Ingredients
550 grams (about 4¼ cups ) bread flour or all-purpose flour, plus more for dusting, see notes above
15 to 16 grams salt, see notes above
2 grams (about ½ teaspoon ) instant yeast, see notes above
Mix the dough : In a large bowl, whisk together the flour, salt, and yeast. Add the water and use a spatula to mix until the dough comes together into a shaggy dough ball. If the dough is dry, use your hands to gently knead it in the bowl until it comes together. Cover the bowl with a towel and let rest for at least 15 minutes and up to 30 minutes.
Stretch and fold : Fill a small bowl with water. Dip one hand into the bowl of water, then use the dry hand to stabilize the bowl while you grab an edge of the dough with your wet hand, pull up, and fold it toward the center. Repeat this stretching and folding motion 8 to 10 times, turning the bowl 90 degrees after each set. By the end, the dough should transform from shaggy in texture to smooth and cohesive.
Pour about 1 teaspoon of olive oil over the dough and use your hands to rub it all over. Cover the bowl tightly and let the dough rise at room temperature until it has nearly doubled in volume, 6 to 10 hours. The time will vary depending on the time of year and the temperature of your kitchen.
Portion the dough : Turn the dough out onto a lightly floured work surface and use a bench scraper to divide the dough into 4 equal portions, roughly 237 grams each. Using flour as needed, form each portion into a ball by grabbing the edges of the dough and pulling them toward the center to create a rough ball. Then flip the ball over, cup both your hands around the dough, and drag it toward you, creating tension as you pull. Repeat this cupping and dragging until you have a tight ball.
Store the dough: Place the dough balls in individual airtight containers (see notes above) and transfer to the fridge for 1 to 3 days.
Shape and proof the dough: On baking day, remove however many rounds of dough you wish to make into baguettes. Place on a clean work surface. I prefer to use no flour here, but if you are finding the dough to be too sticky, lightly flour your work surface. ( Note: I suggest watching the video before you attempt shaping. ) Pat the dough into roughly a 6 inch square or 6×7-inch rectangle. Fold the top down toward the center and pinch it gently. Turn the dough 180º and fold the top down again toward the center and pinch it gently (creating an “envelope”). Fold the top down again toward the center, pinching gently. Repeat one last time folding the top down all the way to end, pinching to seal the two halves together. (Again: Best to watch the video here!) Use both hand to gently roll the dough, then flip the log over and pinch the seam together. Flip the log over one last time, roll gently, then transfer to a lightly floured DoughMate container. (Alternatively you could use a 9×13-inch baking pan, which you will tuck inside a 2-gallon ziptop bag to create an airtight environment.) Roll the log in the flour, letting it rest seam-side down. Cover the vessel and let rest for 2.5 – 3 hours or until the dough passes the poke test: when it’s pressed gently, it springs back slowly.
Challenger Bread Baker: After the dough has proofed for roughly 2 hours, place your Challenger bread pan in the oven on a middle rack and preheat it to 450ºF. This will take roughly 30 minutes. Fold a standard sheet of parchment paper in half vertically, and tear or cut along the seam.
Baking Steel: After the dough has proofed for roughly 2 hours, place your Baking Steel in the oven on a middle rack, and preheat it to 450ºF. This will take roughly 30 minutes. Fold a standard sheet of parchment paper in half vertically, and tear or cut along the seam. Have the disposable aluminum pan at the ready as well as a small oven-safe skillet or vessel, strong enough to weigh down the pan without collapsing it.
Emile Henry Baguette Baker: Butter your baguette baker and set aside. Preheat your oven to 450ºF (you do not preheat this vessel).
Score your Dough: Open the lid of the DoughMate and gently roll the log back and forth a few times to release it from the bottom of the vessel. Use your hand to brush away the excess flour. If you are using the Challenger Bread Baker or Baking Steel, lift up the dough and transfer it to one of the parchment paper strips. Using a sharp blade, make three diagonal slashes evenly spaced along the top of the log. If you using something similar to the Emile Henry lidded baguette baker, simply transfer it to the buttered baker, then using a sharp blade, make three diagonal slashes evenly spaced along the top of the log.
Challenger Bread Baker: Using reliable oven mitts, remove the lid from the baker and lower the parchment sheet into the bottom of the pan, orienting it on the diagonal to allow for the most space. Cover the vessel. Close the oven. Bake for 10 minutes. Uncover and bake for 10 minutes more or until the baguette is evenly golden brown or to your liking.
Baking Steel: Place the parchment sheet on a peel, and shimmy it parchment paper and all onto the steel. Cover with the aluminum pan. Place a small oven-safe skillet or something heavy enough to weigh the pan down without collapsing it. Bake for 10 minutes. Uncover and bake for 10 minutes more or until the baguette is evenly golden brown or to your liking.
Emile Henry Baguette Baker: Your scored dough is in the baker (per step 8). Cover the vessel and transfer to your preheated oven (450ºF). Bake for 10 minutes. Uncover and bake for 10 minutes more or until the baguette is evenly golden brown or to your liking.
Let Cool: Remove the baguette from the oven and let cool for 20-ish minutes before serving.
Storing: Baguettes are best eaten the day they are made, but if you must store them, transfer them to a ziplock bag and store at room temperature for up to 3 days or in the freezer for up to 3 months. Always reheat before serving: 350ºF for 15 minutes or so.
Prep Time: 2 days
Cook Time: 20 minutes
Category: Bread
Method: Oven
Cuisine: American, French
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9 Comments on “Crusty, Open-Crumb Baguettes”
Never mind!!! Yes! Then shimmy it onto the hot Baking Steel or pizza stone
Did you experiment with Gluten Free flours?
What do you think about using an oval shaped granite ware lid instead of a disposable foil pan as a topper if baking on a stone? I’m going to try it.
Alex thank you for this precise post. Would the pizza steel/alum pan option or the oval le creuset pot be the better choice? I ask as the creuset is significantly deeper than your oval lidded pot so not sure which direction would give the better results. Thank you. Can’t wait.
Qoestion: Have you tried a perforated baguette pan and poring boiling water in a pan at the bottom of oven.. Thank you
Super instructions. I’ve been wanting to make dinner rolls with roughly the same crumb and crust. Do you have any sense of how to do this (weight of dough ball per roll, differences in rising time, if any; differences in baking time)? I’m assuming baking methods 1 and 2 would remain the same. Would it be possible to use 3 and just spread the rolls out in the wells?
I took your pizza classes this summer at Baking Steel and Milk Street. You’re a very good teacher. Thank you!
Hi, I’m curious to know the process/results of using a baguette pan (perforated metal). I have/love your “Pizza Night!” Thank you for all of your free resources, recipes, etc.!
Great recipe! Can’t wait to try it. Do you think I could use sourdough instead of yeast?
Your baguettes look delicious! Fresh bread with Camembert cheese 😋
Unfortunately, I cannot find Petra flour. I checked on Amazon but this one does not come up. Besides KA flour, can you recommend another kind of Italian flour?
I have an Émile Henry Baguette Baker but on your video, I saw the difference between the Challenger and the Émile Henry bread Baker. The Challenger has more holes like the true French baguette. Which Challenger bread baker would you recommend?
As always, thank you for your recipes and helpful videos!!
baking soda+ venigar= carbon dioxide. experiment by shloka
One Minute Science
Carbon Dioxide Experiment 🧪 by Mind Museum #mindmuseum #cardondioxide #scienceexperiment
10 CBSE Carbon dioxide in lime water
COMMENTS
Limewater Carbon Dioxide Test
Procedure. **Day before preparations. Add 1 teaspoon of calcium hydroxide (slaked lime) to the large jar or bottle. Fill the bottle with distilled water and stir or shake (if your jar has a lid) vigorously for 1-2 minutes. Let stand undisturbed for 24 hours. **Day of procedures. After 24 hours, using the filter and filter paper, strain the lime ...
Limewater Test
Lime Water Breath Experiment. Using lime water is a fun and easy way to test for the presence of carbon dioxide. The exhaled carbon dioxide is used to produce a precipitate of calcium carbonate with the lime water. carbon dioxide + calcium hydroxide (limewater) → calcium carbonate + water. Procedure: Add 50 ml of lime water to two 100 ml beakers.
The Limewater Carbon Dioxide Test
The Limewater Carbon Dioxide Test. Carbon dioxide, also commonly known by its chemical formula CO2, is one of the major building blocks of life. It is usually found in its gaseous form, and is a major part of the plant and animal life cycle. CO 2 is consumed by plants in photosynthesis and is produced by animals (like us!) during respiration.
Testing for CO2 (Carbon dioxide) with Limewater
To test of the presence of Carbon dioxide (CO2 in a gas) we can bubble it through a solution of limewater. If there is CO2 present it will react with the li...
To Investigate the Carbon Dioxide Levels of Inhaled and ...
In this experiment we will investigate the carbon dioxide levels of inhaled and exhaled air. We use limewater to test for the presence of carbon dioxide.Teac...
How to Test for Carbon Dioxide (CO₂): Easy Scientific Steps
Testing for Carbon Dioxide. Collect a sample of CO 2 in a sealed test tube. Then, bubble the gas through a limewater (1 teaspoon (4.9 mL) calcium hydroxide diluted in distilled water). If the liquid turns milky white, CO 2 is present. Or, hold a lit splint to the sample and see if the flame goes out, indicating CO 2.
Science Experiment : Carbon Dioxide and Limewater (Breath Test)
This experiment proves the presence of carbon dioxide in our breath. Great Science Fair Project.All animals require oxygen to breathe and most plants require...
The reaction of carbon dioxide with water
Place about 125 cm 3 of water in a 250 cm 3 conical flask. Add one or two drops of phenol red to the water. Add two drops of sodium hydroxide solution to produce a red solution. Talk or blow gently into the flask - ie add carbon dioxide. Continue adding the carbon dioxide until a colour change is observed.
Experiment 4: Lime Water Test For CO2
Method. Make lime water. Add a small amount of calcium hydroxide to a test tube and add water. Add bung and shake. Allow to settle. Decant the clear solution into a beaker: lime water. Turn the lime water cloudy. Add about 2 cm lime water to a test tube. Blow through a drinking straw to bubble CO 2 through the lime water solution until it goes ...
Test the gas
The test for carbon dioxide uses an aqueous solution of calcium hydroxide (lime water). When carbon dioxide is shaken with or bubbled through limewater the limewater turns milky (cloudy). 4.8.3 Identification of ions by chemical and spectroscopic means. 4.8.3.3 Carbonates. Carbonates react with dilute acids to form carbon dioxide gas.
Test for Carbon Dioxide
To identify the presence of carbon dioxide gas in a sample, you can perform a simple experiment using limewater. Here's what you'll need to do: 1. Prepare two test tubes, one containing the sample gas and the other containing limewater. Limewater is an aqueous solution of calcium hydroxide, which is calcium oxide dissolved in water. 2 ...
How does carbon dioxide react with limewater
Carbon dioxide reacts with limewater to form calcium carbonate, which precipitates out of the solution. The reaction between limewater, which is a solution of calcium hydroxide, "Ca(OH)"_2, and carbon dioxide will result in the formation of an insoluble solid called calcium carbonate, "CaCO"""_3. Ca(OH)_(2(aq)) + CO_text(2(aq]) -> CaCO_(3(s)) darr + H_2O_((l)) The solution will turn milky due ...
Reacting Carbon Dioxide with Lime water
27 July 2016. Carbon dioxide reacts with limewater to form calcium carbonate, which precipitates out of the solution. The carbon dioxide and limewater react to produce calcium carbonate and water. Calcium carbonate is chalk, and when it is produced, it precipitates and solid particles of chalk appear.
PDF Carbon Dioxide
Carbon Dioxide Data Table Make a diagram of this experiment. Label both test tubes, rubber stopper, 90° glass tubing, limewater, sodium hydrogen sulfate, sodium carbonate, and carbon dioxide. Exercises Answer the questions below: 1. How was limewater used in this experiment? 2. How do you know if carbon dioxide was actually produced? 3.
Main Group Elements- Reaction Between Carbon Dioxide and Limewater
Reaction Between Carbon Dioxide and Limewater Description: Carbon dioxide gas bubbling through limewater produces a precipitate. Sources of carbon dioxide include exhaled breath, Alkaseltzer® tablets, or dry ice. The precipitate will redissolve if the concentration of carbon dioxide is high enough. Source: Shakhashiri, B.Z. Chemical Demonstrations: A Handbook for Teachers of Chemistry Year ...
Lime Water Breath Experiment
Using lime water is a fun and easy way to test for the presence of carbon dioxide. The exhaled carbon dioxide is used to produce a precipitate of calcium ca...
Identifying the products of combustion
In this experiment, students observe as the teacher burns a solid hydrocarbon (in the form of a tea light or candle), using a pump to divert the gaseous combustion products. ... 1.8.14 describe how to test for carbon dioxide: limewater (calcium hydroxide solution) will change from colourless to milky if the test is positive; and; Unit C2 ...
Carbon dioxide (CO2) and Limewater (Ca(OH)2)
A chemical demonstration to show the action of CO2 on Lime water. This experiment also proves that exhaled air contains carbon dioxide (CO2)
Signs of Chemical Changes: Testing for CO2, O2, and H2
Bubbling carbon dioxide through water also results in the formation of an acid (carbonic acid), and that too will decrease pH, resulting in an indicator color change. Carbon dioxide bubbled through lime water will make a milky precipitate, calcium carbonate, that is easily seen. ... With repeated experiments and practice using equation models ...
Enhanced Rock Weathering for Carbon Removal-Monitoring and Mitigating
Terrestrial enhanced rock weathering (ERW) is the application of pulverized silicate rock to soils for the purposes of carbon removal and improved soil health. Although a geochemical modeling framework for ERW in soils is emerging, there is a scarcity of experimental and field trial data exploring potential environmental impacts, risks, and monitoring strategies associated with this practice ...
Crusty, Open-Crumb Baguettes
Increased fermentation activity, meaning as the yeasts rapidly multiply in the hot oven, the dough produces carbon dioxide gas. 2. Steam: As water in the dough evaporates it transforms into steam. Both the carbon dioxide gas and the steam push against the gluten structure, causing the dough to spring.
Lime water and carbon dioxide Experiment
Reewaz is blowing the lime water for the carbon dioxide test
IMAGES
VIDEO
COMMENTS
Procedure. **Day before preparations. Add 1 teaspoon of calcium hydroxide (slaked lime) to the large jar or bottle. Fill the bottle with distilled water and stir or shake (if your jar has a lid) vigorously for 1-2 minutes. Let stand undisturbed for 24 hours. **Day of procedures. After 24 hours, using the filter and filter paper, strain the lime ...
Lime Water Breath Experiment. Using lime water is a fun and easy way to test for the presence of carbon dioxide. The exhaled carbon dioxide is used to produce a precipitate of calcium carbonate with the lime water. carbon dioxide + calcium hydroxide (limewater) → calcium carbonate + water. Procedure: Add 50 ml of lime water to two 100 ml beakers.
The Limewater Carbon Dioxide Test. Carbon dioxide, also commonly known by its chemical formula CO2, is one of the major building blocks of life. It is usually found in its gaseous form, and is a major part of the plant and animal life cycle. CO 2 is consumed by plants in photosynthesis and is produced by animals (like us!) during respiration.
To test of the presence of Carbon dioxide (CO2 in a gas) we can bubble it through a solution of limewater. If there is CO2 present it will react with the li...
In this experiment we will investigate the carbon dioxide levels of inhaled and exhaled air. We use limewater to test for the presence of carbon dioxide.Teac...
Testing for Carbon Dioxide. Collect a sample of CO 2 in a sealed test tube. Then, bubble the gas through a limewater (1 teaspoon (4.9 mL) calcium hydroxide diluted in distilled water). If the liquid turns milky white, CO 2 is present. Or, hold a lit splint to the sample and see if the flame goes out, indicating CO 2.
This experiment proves the presence of carbon dioxide in our breath. Great Science Fair Project.All animals require oxygen to breathe and most plants require...
Place about 125 cm 3 of water in a 250 cm 3 conical flask. Add one or two drops of phenol red to the water. Add two drops of sodium hydroxide solution to produce a red solution. Talk or blow gently into the flask - ie add carbon dioxide. Continue adding the carbon dioxide until a colour change is observed.
Method. Make lime water. Add a small amount of calcium hydroxide to a test tube and add water. Add bung and shake. Allow to settle. Decant the clear solution into a beaker: lime water. Turn the lime water cloudy. Add about 2 cm lime water to a test tube. Blow through a drinking straw to bubble CO 2 through the lime water solution until it goes ...
The test for carbon dioxide uses an aqueous solution of calcium hydroxide (lime water). When carbon dioxide is shaken with or bubbled through limewater the limewater turns milky (cloudy). 4.8.3 Identification of ions by chemical and spectroscopic means. 4.8.3.3 Carbonates. Carbonates react with dilute acids to form carbon dioxide gas.
To identify the presence of carbon dioxide gas in a sample, you can perform a simple experiment using limewater. Here's what you'll need to do: 1. Prepare two test tubes, one containing the sample gas and the other containing limewater. Limewater is an aqueous solution of calcium hydroxide, which is calcium oxide dissolved in water. 2 ...
Carbon dioxide reacts with limewater to form calcium carbonate, which precipitates out of the solution. The reaction between limewater, which is a solution of calcium hydroxide, "Ca(OH)"_2, and carbon dioxide will result in the formation of an insoluble solid called calcium carbonate, "CaCO"""_3. Ca(OH)_(2(aq)) + CO_text(2(aq]) -> CaCO_(3(s)) darr + H_2O_((l)) The solution will turn milky due ...
27 July 2016. Carbon dioxide reacts with limewater to form calcium carbonate, which precipitates out of the solution. The carbon dioxide and limewater react to produce calcium carbonate and water. Calcium carbonate is chalk, and when it is produced, it precipitates and solid particles of chalk appear.
Carbon Dioxide Data Table Make a diagram of this experiment. Label both test tubes, rubber stopper, 90° glass tubing, limewater, sodium hydrogen sulfate, sodium carbonate, and carbon dioxide. Exercises Answer the questions below: 1. How was limewater used in this experiment? 2. How do you know if carbon dioxide was actually produced? 3.
Reaction Between Carbon Dioxide and Limewater Description: Carbon dioxide gas bubbling through limewater produces a precipitate. Sources of carbon dioxide include exhaled breath, Alkaseltzer® tablets, or dry ice. The precipitate will redissolve if the concentration of carbon dioxide is high enough. Source: Shakhashiri, B.Z. Chemical Demonstrations: A Handbook for Teachers of Chemistry Year ...
Using lime water is a fun and easy way to test for the presence of carbon dioxide. The exhaled carbon dioxide is used to produce a precipitate of calcium ca...
In this experiment, students observe as the teacher burns a solid hydrocarbon (in the form of a tea light or candle), using a pump to divert the gaseous combustion products. ... 1.8.14 describe how to test for carbon dioxide: limewater (calcium hydroxide solution) will change from colourless to milky if the test is positive; and; Unit C2 ...
A chemical demonstration to show the action of CO2 on Lime water. This experiment also proves that exhaled air contains carbon dioxide (CO2)
Bubbling carbon dioxide through water also results in the formation of an acid (carbonic acid), and that too will decrease pH, resulting in an indicator color change. Carbon dioxide bubbled through lime water will make a milky precipitate, calcium carbonate, that is easily seen. ... With repeated experiments and practice using equation models ...
Terrestrial enhanced rock weathering (ERW) is the application of pulverized silicate rock to soils for the purposes of carbon removal and improved soil health. Although a geochemical modeling framework for ERW in soils is emerging, there is a scarcity of experimental and field trial data exploring potential environmental impacts, risks, and monitoring strategies associated with this practice ...
Increased fermentation activity, meaning as the yeasts rapidly multiply in the hot oven, the dough produces carbon dioxide gas. 2. Steam: As water in the dough evaporates it transforms into steam. Both the carbon dioxide gas and the steam push against the gluten structure, causing the dough to spring.
Reewaz is blowing the lime water for the carbon dioxide test