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Chapter 10: Problem 21

Which of the following is more likely to be soluble in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) ? In each case, explain your answer. (a) \(\mathrm{CCl}_{4}\) or \(\mathrm{NaCl}\) (b) hexane \(\left(\mathrm{C}_{6} \mathrm{H}_{14}\right)\) or glycerol \(\left(\mathrm{CH}_{2} \mathrm{OHCHOHCH}_{2} \mathrm{OH}\right)\) (c) acetic acid \(\left(\mathrm{CH}_{3} \mathrm{COOH}\right)\) or heptanoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{13} \mathrm{COOH}\right)\) (d) \(\mathrm{HCl}\) or propylchloride \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{Cl}\right)\)

Short Answer

Expert verified
a) CCl4 or NaCl Answer: CCl4 b) hexane or glycerol Answer: hexane c) acetic acid or heptanoic acid Answer: heptanoic acid d) HCl or propylchloride Answer: propylchloride

Step by step solution

01

(a) CCl4 or NaCl

To determine which of these compounds is more likely to dissolve in benzene, we should consider their polarity. Benzene is a nonpolar compound, while CCl4 is also nonpolar, and NaCl is an ionic compound. Since nonpolar substances are likely to dissolve in nonpolar solvents, CCl4 is more likely to be soluble in benzene than NaCl.
02

(b) hexane or glycerol

Hexane (C6H14) is a nonpolar compound as it is an alkane, and glycerol (CH2OH-CHOH-CH2OH) is polar due to the presence of the hydroxyl (-OH) groups. Since benzene is nonpolar, it will have better solubility with hexane, which is also nonpolar, as like dissolves like.
03

(c) acetic acid or heptanoic acid

To determine which of these acids is more likely to dissolve in benzene, we should compare their polarities. Both acetic acid (CH3COOH) and heptanoic acid (C6H13COOH) are carboxylic acids and are polar compounds. However, heptanoic acid has a longer hydrocarbon chain, which makes it less polar than acetic acid. Since benzene is a nonpolar compound, heptanoic acid, which is less polar, is more likely to be soluble in benzene than acetic acid.
04

(d) HCl or propylchloride

In this case, we are comparing HCl, a polar molecule, to propylchloride (CH3CH2CH2Cl), a nonpolar organic compound. Since benzene is nonpolar, propylchloride, which is also nonpolar, will likely be more soluble in benzene as like dissolves like. HCl, being a polar molecule, will not be as soluble in benzene.

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Most popular questions from this chapter

It is found experimentally that the volume of a gas that dissolves in a given amount of water is independent of the pressure of the gas; that is, if \(5 \mathrm{~cm}^{3}\) of a gas dissolves in \(100 \mathrm{~g}\) of water at 1 atm pressure, \(5 \mathrm{~cm}^{3}\) will dissolve at a pressure of 2 atm, 5 atm, 10 atm, .... Show that this relationship follows logically from Henry's law and the ideal gas law.

For a solution of acetic acid (CH \(_{3} \mathrm{COOH}\) ) to be called "vinegar," it must contain \(5.00 \%\) acetic acid by mass. If a vinegar is made up only of acetic acid and water, what is the molarity of acetic acid in the vinegar? The density of vinegar is \(1.006 \mathrm{~g} / \mathrm{mL}\).

Show that the following relation is generally valid for all solutions: $$ \text { molality }=\frac{\text { molarity }}{d-\frac{\mathrm{MM}(\mathrm{molarity})}{1000}} $$ where \(d\) is solution density \(\left(\mathrm{g} / \mathrm{cm}^{3}\right)\) and \(\mathrm{MM}\) is the molar mass of the solute. Using this equation, explain why molality approaches molarity in dilute solution when water is the solvent, but not with other solvents.

A solution is prepared by diluting \(0.7850 \mathrm{~L}\) of \(1.262 \mathrm{M}\) potassium sulfide solution with water to a final volume of \(2.000 \mathrm{~L}\). (a) How many grams of potassium sulfide were dissolved to give the original solution? (b) What are the molarities of the potassium sulfide, potassium ions, and sulfide ions in the diluted solution?

An aqueous solution made up of \(32.47 \mathrm{~g}\) of iron(III) chloride in \(100.0 \mathrm{~mL}\) of solution has a density of \(1.249 \mathrm{~g} / \mathrm{mL}\) at \(25^{\circ} \mathrm{C}\). Calculate its (a) molarity. (b) molality. (c) osmotic pressure at \(25^{\circ} \mathrm{C}\) (assume \(\left.i=4\right)\). (d) freezing point.
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