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Int Task 3

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3INT Task 3 1. Problem statement
How does salt have an effect on freezing point of water?

2. Relevance of your testable question
When salt is added to water it results in the reduction of its freezing point and the density of water increases. Freezing point depression which is a colligative property does not depend on its solute character rather it depends only on its solute concentration.

3. Literature review
Entropy is frequently defined as a quantitative measure of randomness. When a solute is dissolved in a solution similar to water, the entropy of the solution increases. Freezing becomes extemporaneous when the extent of heat energy lost by the water during freezing is equivalent to the temperature times the reduction in entropy linked with freezing (Brennan, n.d.). Water freezes and melts at 0°C (32°F). However, dissolving any substance in pure water lowers the freezing point. A water with very high salt level such as highly saline lake waters at Death Valley, California (nearly 300,000 units per million "salt") may freeze and melt at temperatures as low as -20 to -30°C. As salt lowers the freezing point depression, it is used on icy roads and highways in order to melt the ice (Benison, 1998). The reason why salt lowers the freezing temperature of water can be explained as follows: When liquid pure water reaches its freeze point and becomes ice, the water molecules form themselves into an ordered formation. Salt reduces this course. When salt is added, impurities also get added to the water. This breaks the water's ability to its freezing temperature. When salt gets dissolved in water, it breaks down into two ions chloride ion and sodium ion. These ions are foreign particles into pure liquid hydrogen and oxygen and this results in scattering of water molecules, separating them and making it difficult to

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