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Ch.13 - Properties of Solutions
Chapter 13, Problem 18b

When ammonium chloride dissolves in water, the solution becomes colder. (b) Why does the solution form?

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Dissolution Process

The dissolution process involves the breaking apart of solute particles and their interaction with solvent molecules. In the case of ammonium chloride (NH4Cl), when it dissolves in water, the ionic bonds between the ammonium and chloride ions are broken, allowing them to disperse throughout the water. This process requires energy, which is absorbed from the surroundings, leading to a decrease in temperature.
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Endothermic Reactions

An endothermic reaction is a chemical process that absorbs heat from its surroundings. The dissolution of ammonium chloride in water is an example of this type of reaction, as it requires energy to break the ionic bonds and separate the ions. As a result, the surrounding water loses heat, causing the temperature of the solution to drop.
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Thermodynamics of Solutions

Thermodynamics in the context of solutions refers to the energy changes that occur during the mixing of solutes and solvents. The overall energy change during dissolution is determined by the balance between the energy required to break solute-solute and solvent-solvent interactions and the energy released from solute-solvent interactions. In the case of ammonium chloride, the energy absorbed during dissolution exceeds the energy released, resulting in a colder solution.
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Related Practice
Textbook Question

Indicate the principal type of solute–solvent interaction in each of the following solutions and rank the solutions from weakest to strongest solute–solvent interaction: (c) methanol (CH3OH) in water

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Textbook Question

An ionic compound has a very negative ∆Hsoln in water (b) Which term would you expect to be the largest negative number: ∆Hsolvent, ∆Hsolute, or ∆Hmix?

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Textbook Question

When ammonium chloride dissolves in water, the solution becomes colder. (a) Is the solution process exothermic or endothermic?

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Textbook Question

Two nonpolar organic liquids, hexane (C6H14) and heptane (C7H16), are mixed. (a) Do you expect ∆Hsoln to be a large positive number, a large negative number, or close to zero? Explain.

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Textbook Question

Two nonpolar organic liquids, hexane (C6H14) and heptane (C7H16), are mixed. (b) Hexane and heptane are miscible with each other in all proportions. In making a solution of them, is the entropy of the system increased, decreased, or close to zero, compared to the separate pure liquids?

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Textbook Question

KBr is relatively soluble in water, yet its enthalpy of solution is + 19.8 kJ/mol. Which of the following statements provides the best explanation for this behavior? (a) Potassium salts are always soluble in water. (b) The entropy of mixing must be unfavorable. (c) The enthalpy of mixing must be small compared to the enthalpies for breaking up water–water interactions and K–Br ionic interactions. (d) KBr has a high molar mass compared to other salts like NaCl.

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