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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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Hello everyone. Today, we have the following problem. The temperature of the system decreases when potassium chlorate is dissolved in water. Which of the following statements explains why the solution is formed. So when potassium chloride dissolves Mrs, potassium chlorine as a solid, it is going to dissolve, dissolve to form potassium ions and chlorate ions. And so when this occurs, the number of particles in the solution are going to increase the number of particles increase. And this process is going to lead to an increase in the disorder or chaos of the system. This is going to result in an increase in the entropy of the system, which is, which is defined as the measure of disorder in a system. And so we can say that when we increase the entropy, this increase is going to drive the solution formation. And so the answer choice d best applies to that the increase in entropy makes up for the increase in entropy of the system. And this drives the solution formation. And with that, we've answered the question overall, I hope this helped. And until next time
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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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