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Chapter 13: Problem 13

Indicate whether each statement is true or false: (a) A solute will dissolve in a solvent if solute-solute interactions are stronger than solute-solvent interactions. (b) In making a solution, the enthalpy of mixing is always a positive number. (c) An increase in entropy favors mixing.

Short Answer

Expert verified
(a) False - A solute will dissolve in a solvent if the solute-solute interactions are weaker than the solute-solvent interactions. (b) False - The enthalpy of mixing can be both positive or negative, depending on whether the mixing is endothermic or exothermic. (c) True - An increase in entropy favors mixing, as it increases the disorder of the solute and solvent molecules.

Step by step solution

01

(a) Solute-solute vs solute-solvent interactions

A solute will dissolve in a solvent if the solute-solute interactions are weaker than the solute-solvent interactions. This is because, for a solute to dissolve in a solvent, it needs to create new interactions with the solvent, which will be stronger and more favorable than the original solute-solute interactions. Therefore, this statement is false.
02

(b) Enthalpy of mixing

The enthalpy of mixing refers to the amount of energy (heat) that is either absorbed or generated due to the mixing of two substances. The enthalpy of mixing can be a positive or a negative number, depending on whether the mixing is endothermic (energy is absorbed, a positive number) or exothermic (energy is released, a negative number). Therefore, this statement is false.
03

(c) Increase in entropy and mixing

Entropy is a measure of the degree of disorder in a system. Higher entropy indicates more randomness, while lower entropy indicates a more ordered state. An increase in entropy generally favors mixing because mixing increases the disorder of the solute and the solvent molecules. Thus, this statement is true.

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Most popular questions from this chapter

(a) Does a 0.10 \(\mathrm{m}\) aqueous solution of NaCl have a higher bolling point, a lower boiling point, or the same boiling point as a 0.10 \(\mathrm{m}\) aqueous solution of \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6} ?(\mathbf{b})\) The experimental boiling point of the NaCl solution is lower than that calculated assuming that NaCl is completely dissociated in solution. Why is this the case?

An ionic compound has a very negative \(\Delta H_{\text { soln in water. }}\) (a) Would you expect it to be very soluble or nearly insoluble in water? (b) Which term would you expect to be the largest negative number: \(\Delta H_{\text { solvent }} \Delta H_{\text { solute }}\) or \(\Delta H_{\text { mix }}\) ?

Which of the following in each pair is likely to be more soluble in hexane, \(\mathrm{C}_{6} \mathrm{H}_{14} :(\mathbf{a}) \mathrm{CCl}_{4}\) or \(\mathrm{CaCl}_{2},(\mathbf{b})\) benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) or glycerol, \(\mathrm{CH}_{2}(\mathrm{OH}) \mathrm{CH}(\mathrm{OH}) \mathrm{CH}_{2} \mathrm{OH},(\mathbf{c})\) octanoic \(\mathrm{acid}, \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{COOH},\) or acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH} ?\) Explain your answer in each case.

\(\mathrm{KBr}\) is relatively soluble in water, yet its enthalpy of solution is \(+19.8 \mathrm{kJ} / \mathrm{mol} .\) 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-Brionic interactions. (d) KBr has a high molar mass compared to other salts like NaCl.

Calculate the freezing point of a 0.100 m aqueous solution of \(\mathrm{K}_{2} \mathrm{SO}_{4},\) (a) ignoring interionic attractions, and (b) taking interionic attractions into consideration by using the van't Hoff factor (Table 13.4 )
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