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Colligative Properties in Your Coke

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Colligative Properties in Your Coke

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Colligative properties in your Coke
Have you ever put salt on snow to get rid of it, or wondered how your car engine stays warm in cold weather? If you have, you’ve probably noticed that the salt quickly melts the snow, and you’ve wondered how the engine can stay warm, when the metal on the outside of the car is cold. These are just some of the many examples of how colligative properties work in our everyday lives. A colligative property is a property of a solvent that depends on the amount of solute particles dissolved in it. It does not focus on the identity or nature of those solute particles, meaning it depends more on how many particles of each solute or solvent is in the solution, and on which type of particle is the solvent or the solution. For example, if the solvent is water, and the solute is a metal, it would have different colligative properties from a solution in which the solvent is a metal, and the solute is water. If the solute is snow, and the solvent is salt, meaning there is more salt than snow, than the salt would be able to melt the snow, and then there would still be more salt left over. In that case if I were to add more snow (the solute) to the salt, then it would change the amount of salt left over, as it is in most colligative properties. If you add more of the solute, than it effects the solvent. Recent studies have shown, that Diet Coke is more likely to explode when frozen, then regular Coca Cola. This is because of the two sodas varying colligative properties. A can of Regular Coke contains about thirty-nine grams of sugar dissolved in it, while Diet Coke has about 0.1 gram of Aspartame sweetener in it. This causes the Diet Coke to have around the same freezing point as water, and because of the other properties in the soda, the freezing causes the pressure in the can to build up until it explodes. If the Diet Coke were have to have more sugar, (the solute) added to it, it would make the drink freeze slower,...