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Chapter 13: Problem 68

List the following aqueous solutions in order of decreasing freezing point: \(0.040 \mathrm{~m}\) glycerin \(\left(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}_{3}\right), 0.020 \mathrm{~m}\) \(\mathrm{KBr}, 0.030 \mathrm{~m}\) phenol \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\right)\).

Short Answer

Expert verified
The order of decreasing freezing points for the given aqueous solutions is Phenol > Glycerin = KBr.

Step by step solution

01

1. Recall the formula for freezing point depression.

The formula for freezing point depression (\(\Delta T_{f}\)) is given by: \[\Delta T_{f} = K_f \cdot i \cdot m \] Where \(K_f\) is a constant called the cryoscopic constant (which is the same for all solutes in a given solvent), \(i\) is the van't Hoff factor, and \(m\) is the molality of the solute in the solution.
02

2. Determine the van't Hoff factor for each solute.

The van't Hoff factor (\(i\)) is the number of dissolved particles produced from a single molecule of solute. For non-electrolytes like glycerin and phenol, the van't Hoff factor is 1. For electrolytes like potassium bromide, \(i\) has to be calculated based on the number of ions produced during the dissociation. In this case, for KBr: \[ \mathrm{KBr} \rightarrow \mathrm{K}^{+} + \mathrm{Br}^{-} \] Thus, the van't Hoff factor for KBr is 2.
03

3. Calculate the freezing point depression for each solution.

Use the calculated van't Hoff factors and the given molalities to find the freezing point depressions: \[\Delta T_{f \, glycerin} = K_f \cdot 1 \cdot 0.040 \] \[\Delta T_{f \, KBr} = K_f \cdot 2 \cdot 0.020 \] \[\Delta T_{f \, phenol} = K_f \cdot 1 \cdot 0.030 \] As \(K_f\) is common for all solutes in the same solvent, we directly compare the numerical values: \[\Delta T_{f \, glycerin} : \Delta T_{f \, KBr} : \Delta T_{f \, phenol} = (1 \cdot 0.040) : (2 \cdot 0.020) : (1 \cdot 0.030) = 0.040 : 0.040 : 0.030\]
04

4. List the solutions in order of decreasing freezing point.

Since the freezing point is inversely proportional to freezing point depression, the solution with the lowest freezing point depression will have the highest freezing point. From step 3, we find the following order of freezing points; Phenol > Glycerin = KBr So, the order of decreasing freezing points for these aqueous solutions is Phenol > Glycerin = KBr.

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Most popular questions from this chapter

Indicate the type of solute-solvent interaction (Section 11.2) that should be most important in each of the following solutions: (a) \(\mathrm{CCl}_{4}\) in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\), (b) methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) in water, (c) \(\mathrm{KBr}\) in water, (d) \(\mathrm{HCl}\) in acetonitrile \(\left(\mathrm{CH}_{3} \mathrm{CN}\right)\).

The density of acetonitrile \(\left(\mathrm{CH}_{3} \mathrm{CN}\right)\) is \(0.786 \mathrm{~g} / \mathrm{mL}\) and the density of methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) is \(0.791 \mathrm{~g} / \mathrm{mL}\). A solution is made by dissolving \(22.5 \mathrm{~mL} \mathrm{CH}_{3} \mathrm{OH}\) in \(98.7 \mathrm{~mL}\) \(\mathrm{CH}_{3} \mathrm{CN}\). (a) What is the mole fraction of methanol in the solution? (b) What is the molality of the solution?

A solution is made containing \(25.5 \mathrm{~g}\) phenol \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\right)\) in \(425 \mathrm{~g}\) ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\). Calculate (a) the mole fraction of phenol, (b) the mass percent of phenol, (c) the molality of phenol.

When \(10.0 \mathrm{~g}\) of mercuric nitrate, \(\mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2}\), is dissolved in \(1.00 \mathrm{~kg}\) of water, the freezing point of the solution is \(-0.162^{\circ} \mathrm{C}\). When \(10.0 \mathrm{~g}\) of mercuric chloride \(\left(\mathrm{HgCl}_{2}\right)\) is dissolved in \(1.00 \mathrm{~kg}\) of water, the solution freezes at \(-0.0685^{\circ} \mathrm{C}\). Use these data to determine which is the stronger electrolyte, \(\mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2}\) or \(\mathrm{HgCl}_{2}\).

(a) Would you expect stearic acid, \(\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{16} \mathrm{COOH}\), to be more soluble in water or in carbon tetrachloride? Explain. (b) Which would you expect to be more soluble in water, cyclohexane or dioxane? Explain.
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