chlorine and coke experiment

Coke and Chlorine Chemical Reaction By: evan f. and will

Overall, this is a very fun reaction to watch. First, you put the coke and chlorine together in the glass. The reactants will just start to fizz and turn light brown. Then after a little bit of waiting it will start to get interesting. The new liquid will then turn totally white and very fizzy. Then it will start uncontrollably flowing outside of the cup and steaming a lot. Be sure to avoid the gas because it is very poisonous. The reactants let off chlorine gas, and a whole lung-full of that won’t be very good for you. To us, this reaction was very entertaining.

Chemical Summary

This is what really happens when you mix Coca-cola and pool chlorine. There is just a small amount of phosphoric acid in coke. Sounds disgusting right? Well that is actually a reactant in this reaction. The phosphoric acid reacts with the pool chlorine, which also known as calcium hypochlorite. The product of this reaction is chlorine gas, which happens to be extremely dangerous. This is what happens when you mix coke and pool chlorine.

Relevant Chemistry Concept

When the coke and chlorine are mixed they create an exothermic reaction. This means when the reaction occurs heat is released. This is clearly demonstrated in the experiment because hot steam is a product of the reaction, (along with chlorine gas.)

Granulated pool chlorine

A glass cup/ beaker

• Obtain all the materials. (granulated pool chlorine, coke, and glass cup/beaker)
• Fill the glass about ¾ of the way with coke.
• Pour chlorine into the cup with the coke. (The more chlorine the larger the reaction.)
• Add chlorine until it makes up around 1/3 of the combination
• You next have to wait around 30 seconds for the chlorine to begin to break down and the reaction to begin.
• Avoid the poisonous chlorine gas.

Created with images by matt512 - "Fire / Cannon fun" • Cal Sr - "My chemicals" • GIANTsqurl - "Coke Bottle" • skycaptaintwo - "200ml"

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• Chemical Reactions
• Science Experiments

Coca Cola and Pool Chlorine

What Will Happen If You Mix Coke and Pool Chlorine? Watch this strange chemical reaction – Coca Cola and Pool Chlorine The small amount of phosphoric acid in the Coke sets off a chemical reaction with the calcium hypochlorite, producing poisonous chlorine gas and a spectacular little explosion.

Original link: http://www.youtube.com/watch?v=wPxjKRwHOiQ

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Safe­ty pre­cau­tions

Don’t drink the Coca-Cola used in any ex­per­i­ments! Ob­serve safe­ty pre­cau­tions when work­ing with heat­ing de­vices.

Reagents and equip­ment

• bleach (15% so­lu­tion sodi­um hypochlo­rite);
• a rusty tool;
• fry­ing pans;

Step-by-step in­struc­tions

Diet Coke and Men­tos erup­tion

Toss a Men­to into a bot­tle of Diet Coke. Ob­serve the re­lease of gas and for­ma­tion of a spout of foam .

Coca-Cola and milk

Pour 50 mL Coca-Cola into 30 mL milk . Ob­serve as the milk cur­dles and the so­lu­tion pales.

Coca-Cola and rust

Let a rusty tool sit in 150 mL Coca-Cola for 5 hours. Re­move it from the so­lu­tion, wipe it off with a pa­per tow­el, and pay at­ten­tion to the dis­ap­pear­ance of the rust.

Cola and bleach

Add 20 mL bleach (15% so­lu­tion sodi­um hypochlo­rite) to 50 mL Coca-Cola. Ob­serve as the mix­ture pales.

How much sug­ar does Cola con­tain?

Pour 200 mL of clas­sic Coca-Cola onto a fry­ing pan. Heat un­til all the liq­uid evap­o­rates. Re­peat the ex­per­i­ment in a sec­ond fry­ing pan us­ing Diet Coke. No­tice the large quan­ti­ty of black tar from the clas­sic Coca-Cola.

Process de­scrip­tion

• Men­tos have a rough sur­face, which aids the for­ma­tion of a large amount of car­bon diox­ide gas from the Coca-Cola on its sur­face. Food ad­di­tives in the Cola and Men­tos con­trib­ute to the for­ma­tion of a large quan­ti­ty of foam.
• Milk con­sists main­ly of pro­teins, fats, mi­croele­ments, and wa­ter. When Coca-Cola is added, the phos­phor­ic acid it con­tains forces the milk to cur­dle. Mean­while, the form­ing clots of pro­teins drag col­or­ing mol­e­cules with them, caus­ing the mix­ture to pale.
• Rust con­sists most­ly of iron(III) ox­ide, and de­vel­ops on iron ob­jects due to hu­mid air or house­hold chem­i­cals. But it’s no prob­lem for clas­sic Coca-Cola! A rusty tool left in Coca-Cola will be thor­ough­ly cleaned from the unattrac­tive tar­nish. This hap­pens thanks to the phos­phor­ic acid in Coca-Cola, which dis­solves the iron(III) ox­ide. 2H₃PO₄ + Fe₂O₃ = 2Fe­PO₄ + 3H₂O
• Bleach con­tains sodi­um hypochlo­rite, which is a strong ox­i­diz­ing agent and eas­i­ly ox­i­dizes the col­or­ing mol­e­cules in the Coca-Cola, caus­ing it to pale.
• The main in­gre­di­ents of clas­sic Cola are sug­ar and wa­ter. As the wa­ter evap­o­rates, the mix­ture thick­ens and forms a black mass re­sem­bling tar, which main­ly con­sists of caramelized sug­ar. Diet Coke con­tains sug­ar sub­sti­tutes in­stead of reg­u­lar sug­ar. These sub­sti­tutes are much sweet­er than sug­ar – even be­ing added in tiny amounts, they make the drink ev­ery bit as sweet as the clas­sic ver­sion. As a re­sult, we see a much small­er amount of residue than in clas­sic Cola.

Dozens of experiments you can do at home

One of the most exciting and ambitious home-chemistry educational projects The Royal Society of Chemistry

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Microscale reactions of chlorine with water or halide ions

In association with Nuffield Foundation

• No comments

Generate chlorine gas and investigate its reactions with water or halide ions in this class practical

In this experiment, students can use microscale apparatus to generate chlorine gas safely themselves in the open laboratory, investigating how it reacts with water and halide ions in solution.

The activity should take about 20 minutes.

• Eye protection (goggles)
• Student sheet with instructions and diagram of apparatus (available for download below)
• Clear plastic sheet – eg OHP film
• Plastic Petri dish and lid, 9 cm
• Plastic teat pipette (see note 10 below)
• Spatula (optional)
• Sodium chlorate(I) solution, 10–14% w/v chlorine (CORROSIVE) – also known as sodium hypochlorite (see note 11 below)
• Dilute hydrochloric acid, 1 M
• Sodium hydroxide solution, 1 M (CORROSIVE)
• Potassium (or sodium) chloride solution, 0.2 M
• Potassium (or sodium) bromide solution, 0.2 M
• Potassium (or sodium) iodide solution, 0.2 M
• Silver nitrate solution, 0.1 M, a few drops
• Zinc oxide powder (DANGEROUS FOR THE ENVIRONMENT), spatula tip
• Zinc sulfide powder, spatula tip
• Blue litmus or universal Indicator paper, about 1 cm

Health, safety and technical notes

• Read our standard health and safety guidance.
• Wear eye protection (goggles) throughout. Ensure laboratory is well ventilated.
• Sodium chlorate(I) solution, Also known as sodium hypochlorite NaOCl(aq), (CORROSIVE) – see CLEAPSS Hazcard HC089  and CLEAPSS Recipe Book RB081. 
• Chlorine, Cl 2 (g), (TOXIC, DANGEROUS FOR THE ENVIRONMENT) – see CLEAPSS Hazcard HC022a .  Chlorine gas is produced in small quantities in this experiment, however, care should be taken if large numbers of students are carrying out this experiment simultaneously. The lab should be well ventilated and students with asthma should be warned not to inhale the gas. Chlorine should be generated for no longer than is necessary to observe the results.
• Dilute hydrochloric acid, HCl(aq) – see CLEAPSS Hazcard HC047a  and CLEAPSS Recipe Book RB043.
• Sodium hydroxide solution, NaOH(aq), (CORROSIVE) – see CLEAPSS Hazcard HC091a  and CLEAPSS Recipe Book RB085. 
• Halide solutions: potassium chloride, KCl(aq), potassium bromide, KBr(aq), potassium iodide, KI(aq) – see CLEAPSS Hazcard HC047b .
• Silver nitrate solution, AgNO 3 (aq) – see CLEAPSS Hazcard HC087  and CLEAPSS Recipe Book RB077. 
• Zinc oxide, ZnO(s) (DANGEROUS FOR THE ENVIRONMENT) and zinc sulfide, ZnS(s) – see CLEAPSS Hazcard HC108b .  
• The ‘reaction vessel’ for the microscale apparatus is the hemispherical dome cut from the top of a plastic teat pipette. Students may cut this themselves with suitable scissors, or it can be provided.
• Commercial chlorine-based bleach solutions can be used instead of sodium chlorate(I) solution supplied by laboratory suppliers but they may not be sufficiently concentrated to generate enough chlorine. They are often less than 5% even when fresh. Some commercial bleaches now also contain detergents, which foam when chlorine is generated. They should not be used. Household ‘bleaches’ based on peroxide are becoming more widely available and do not contain chlorine, therefore they should not be used.
• Cover the worksheet containing the diagram of the microscale setup with the plastic sheet.
• Place the Petri dish directly over the circle on the worksheet.
• Use the microscale reaction vessel provided or make one by cutting the hemispherical top off the teat part of a plastic pipette. Place this in the centre of the Petri dish, as shown in the diagram.
• At the corners of the triangle on the worksheet place two to three drops of the test solutions indicated on the diagram. Moisten the small piece of indicator paper and place it in the space between any two of the test solutions, along the side of the triangle.
• Place two drops of bleach solution in the reaction vessel and add three drops of dilute hydrochloric acid. Quickly place the lid on the Petri dish to prevent any chlorine escaping.
• Record your observations over the next 10 minutes. The greenish-yellow colour of chlorine gas may be visible in the Petri dish, especially if viewed from the side. The indicator paper turns red and then becomes bleached. The sodium chloride solution is unaffected. The potassium bromide solution gradually turns pale yellow due to the formation of bromine. The potassium iodide solution turns yellow-brown due to the liberation of iodine by the chlorine.
• When the reactions have finished, add three drops of sodium hydroxide solution to the reaction vessel to stop the generation of chlorine and replace the lid.

Teaching notes

The effect of chlorine gas on the moist indicator paper shows that it dissolves to some extent in water and reacts to produce an acidic and strongly bleaching solution. The reaction is the reverse of the reaction used to generate the gas from bleach. Acidifying bleach solution produces chloric(I) acid, HOCl, which decomposes to produce chlorine:

HOCl(aq) + HCl(aq) → Cl 2 (g) + H 2 O(l)

When chlorine dissolves in water, it reacts to form the strong acid, HCl, and the weak but strongly oxidising acid, HOCl, which is responsible for the bleaching properties.

The displacement reactions involving chlorine and the solutions containing halide show that chlorine displaces bromine and iodine from solution:

Cl 2 (g) + 2KX(aq) → 2KCl(aq) + X 2 (aq), where X = Br or I.

or Cl 2 (g) + 2X – (aq) → 2Cl – (aq) + X 2 (aq)

This establishes the trend in reactivity of the halogens down Group 17, which could be extended by investigating the reaction of bromine water with halide ions in solution. The reactivity is related to the oxidising power of the halogens, which decreases down the group.

The tendency of halogen atoms to act as oxidising agents by accepting an electron can be related to their atomic radius. The smaller the halogen atom, the stronger the attraction of the nucleus on the electrons in the outer shell. Thus fluorine attracts an extra electron to complete its outer shell, most strongly, and is therefore the most powerful oxidising agent in the Group.

This microscale apparatus can be used in a similar way to investigate other chlorine reactions. The solutions at the three corners of the triangle can be replaced by silver nitrate solution, solid zinc sulfide and zinc oxide respectively. The silver nitrate solution becomes cloudy as the reaction of chlorine with water produces chloride ions in solution (see above), which then forms a silver chloride precipitate.

The zinc sulfide takes on a yellowish tinge due to the formation of elemental sulfur:

Cl 2 (g) + ZnS(s) → ZnCl 2 (s) + S(s)

Chlorine is reacting as an oxidising agent again. The zinc oxide shows no change although some oxygen gas is probably produced in a similar reaction.

Microscale reactions of chlorine - 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 .

© Nuffield Foundation and the Royal Society of Chemistry

• 14-16 years
• 16-18 years
• Practical experiments
• Properties of matter
• Reactions and synthesis

Specification

• Mandatory experiment 1.2 - Redox reactions of group VII elements - halogens as oxidising agents (reactions with bromides, iodides, Fe²⁺ and sulfites). Displacement reactions of metals (Zn with Cu²⁺, Mg with Cu²⁺). (Half equations only required e.g. 2Br⁻…
• Oxidation and reduction in terms of loss and gain of electrons.
• Oxidising and reducing agents.
• The trend in oxidising ability of the halogens down the group, including displacement reactions of halide ions in aqueous solution.
• The trend in reducing ability of the halide ions, including the reactions of solid sodium halides with concentrated sulfuric acid.
• The use of acidified silver nitrate solution to identify and distinguish between halide ions.
• The trend in solubility of the silver halides in ammonia.
• Students should be able to explain why: silver nitrate solution is used to identify halide ions.
• The silver nitrate solution is acidified.
• Ammonia solution is added.
• Halide ions in solution produce precipitates with silver nitrate solution in the presence of dilute nitric acid. Silver chloride is white, silver bromide is cream and silver iodide is yellow.
• A more reactive halogen can displace a less reactive halogen from an aqueous solution of its salt.
• 9.5Cc chloride ion, Cl⁻, bromide ion, Br⁻, iodide ion, I⁻, using dilute nitric acid and silver nitrate solution
• 6.10 Recall that the halogens, chlorine, bromine and iodine, form hydrogen halides which dissolve in water to form acidic solutions, and use this pattern to predict the reactions of other halogens
• 6.11 Describe the relative reactivity of the halogens chlorine, bromine and iodine, as shown by their displacement reactions with halide ions in aqueous solution, and use this pattern to predict the reactions of astatine
• C2.2.6 recall the simple properties of Group 7 elements including their states and colours at room temperature and pressure, their colours as gases, their reactions with Group 1 elements and their displacement reactions with other metal halides
• C5.2.4 describe tests to identify aqueous cations and aqueous anions and identify species from test results including: tests and expected results for metal ions in solution by precipitation reactions using dilute sodium hydroxide (calcium, copper, iron(I…
• C4.2b describe tests to identify aqueous cations and aqueous anions
• (r) the relative reactivities of chlorine, bromine and iodine as demonstrated by displacement reactions
• (s) the properties and uses of chlorine and iodine
• (q) the relative reactivities of chlorine, bromine and iodine as demonstrated by displacement reactions
• (r) the properties and uses of chlorine and iodine
• 1.6.18 describe how to test for chlorine gas (damp universal indicator paper changes to red and then bleaches white);
• 1.6.19 investigate the displacement reactions of Group 7 (VII) elements with solutions of other halides to establish the trend in reactivity within the group and make predictions based on this trend;
• 1.8.4 recall the reaction of chlorine with water to form chloride ions and chlorate(I) ions;
• 1.8.5 describe the trend in oxidising ability of the halogens down the Group applied to displacement reactions of the halogens with other halide ions in solution;

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Chlorine And Coke Creates An Impressive Reaction When Combined.

Experiment is the best way to know the result of a certain thing. We usually do this in science class. Experimenting is also used by scientists worldwide to make an observation for finding a solution and answers. When it comes to experiment videos on internet, Coca-Cola is always on the list. There are lots of experiments we already saw in any social networking sites like on YouTube and Facebook. Some mix this carbonated drink with milk or Mentos while others boil it, and all of these experiments have their own result. But what if a coke is mixed in a chlorine? Check out the video below and see what the reaction of Coca-Cola mixing with chlorine is.

Chlorine also has a multitude of industrial uses. Including making bulk materials like bleached paper products, plastics such as PVC and many more. But here on this video, Chlorine will be put it into a test wherein it will mixed to Coke. After a few seconds when the chlorine drops into a plastic up of Coca-Cola, it suddenly burst out like an active volcano. Watch the video below.

That was an amazing experiment. The reaction between Coca-Cola and chlorine is quite impressive. Two thumbs up for this experiment!

Thank you so much for dropping by and reading this blog post. For more science experiments, feel free to visit our website more often.

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When you mix Coca-Cola with bleach something deadly but amazing happens

This experiment proves how household cleaner can turn a fizzy drink into a lethal concoction - but it's not to be tried at home as it can kill!

• 10:10, 31 DEC 2015
• Updated 16:04, 31 DEC 2015

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If you've ever used a household bleach to clean your bathroom or kitchen then you'll be aware just how effective it is for removing stains.

But have you ever thought about pouring it into a glass of brown coloured fizzy soda to see what happens?

Well the maker of this video should probably have warned you that it's a very dangerous experiment indeed.

Coke the chemical phosphoric acid which reacts with hypochlorite in bleach and releases chlorine gas.

In the correct dosage it can easily become a chemical weapon and in fact accidental chlorine gas exposure has caused death.

This video should come with a public safety warning - but it shows exactly what happens when you mix bleach with Coca-Cola .

And the results while not exactly staggering are interesting.

This YouTube video posted by CrazyRussianHacker - has not only had four million hits - but it has turned this bonkers wannabe scientist into a viral sensation.

And while his unorthodox approach to traditional experiments is rudimentary it's most certainly amusing.

To begin with CrazyRussianHacker takes the powerful bleach and mixes it with a coke and as if by magic, or chemical process, seconds later the colour slowly disappears.

And it literally takes just two minutes for the bleach to dissolve the brown colour which is caused by the chemical 4-methylimidazole .

While this video which looks as if it was shot on the CrazyRussianHacker's porch is fun, it's certainly not advisable to play around with bleach - especially around kids.

Many thousands of children, adults and pets are injured due to the ferocious chemicals within household cleaning products each year by way of ingestion or through contact with skin.

While hundreds more are killed through deliberate actions involving the substance.

And while CrazyRussianHacker may be entertaining, safety isn't his first priority, doing the experiment entirely without rubber gloves.

So don't try this at home people!

• The Coca-Cola Company
• Most Recent

What Happen When Mix Coca Cola and Bleach?

Introduction: What Happen When Mix Coca Cola and Bleach?

What happen when you mix Coca Cola and Bleach? You can use Pepsi, Coke.

Bleach remove colors through oxidation. Breaking down the chemicals that create visible hues.

Step 1: Add Bleach to Cola

Pour Bleach into Cola..Watch it turn clear

Explanation: Bleach remove colors through oxidation. Breaking down the chemicals that create visible hues.

Please subscribe to my Youtube channel: http://www.youtube.com/channel/UCu-rEN_lWOYyyU2C5d...

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How to Create Carbonation

Do you know what happens when you mix salt and a carbonated beverage? A chemical reaction!

How does it work?

The unique reaction of salt and coke, called nucleation, is due to the rough surface of a grain of salt. When salt is added to the carbonized soda, the carbon dioxide suddenly has more points to react with water and form carbonic acid.

Click here to download a PDF of the instructions for this experiment to print and recreate at home!

Find us at Facebook.com/abc11scienceclub to share photos and videos of your experiment!

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News : What Happens When You Mix Coca Cola and Milk

Interesting reaction coke and milk The reaction of phosphoric acid (V) to proteins in the milk - they are cut and causes a precipitate

The reaction of phosphoric acid with calcium contained in milk gives rise to a precipitate 3Ca + 2H3PO4 ///\\\ Ca3(PO4)2 + 3H2

It is a reaction of the Phosphoric Acid contained in the coca cola to the milk. Phosphoric Acid molecules attach to the milk giving them more density and separate out while the remaining liquid that makes up the milk and cocoa cola now being lighter floats on top. The solid matter is basically milk that has been curdled by the addition of the more acidic soda.

Both items are acidic but coca-cola more so. In general, coca-cola has a pH of anywhere from 2.5-4.5 because of the Phosphoric Acid content where milk has a normal pH around 6.7 (almost neutral, milk that is in the base range is usually mastitic).

There are some studies to suggest that because of the high Phosphoric Acid content in most soft drinks that they can help to increase the likelihood that a person will develop Osteoporosis if they aren't getting enough Calcium in their diet. Coca-cola makes an excellent household cleaner - it can be used to take tarnish off of pennies and I've used it to degrease car engines. I will not drink any soft drinks.

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14 Comments

Oops, it looks a little bit gross.

may i use the investigatory project

hello, may i use this idea for my science fair project. im in 8th grade?

Its a good idea my fellow classmate didi this and im in 7th grade. just be sure to use the pop bttle and close the lid!

I'm going to be using this idea for my school experiment

please reply soon!

nice one....

I don't see why you wouldn't be able to use it. You can do the same thing with lemon juice. The precipitate when using lemon juice has another name: Ricotta cheese .

Why does this not work when using an open container?

We did this and it didi not work and i don't have a clue why and no one replied to my comment so yeah i don't know what i did wrong someone please tell me why this happened!!!

because it needs to be shaken often and depends on type of milk used ,, take an 500 ml coke bottle and the little space left inside the container you through in milk and close it ,, leave 5 min and shake ,, continue in intervals of +- 15 min

what type of reaction forms?? endothermic or exothermic ??

So, I found this lab, because my teacher wanted me to look for a lab that could answer these questions . Can an acid turn into a base? Can a base be turned into an acid? Can an acid be neutralized? I hope that this lab will help me with these questions!!!!

Hopefully the lab will help u

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