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Chapter 13: Problem 31

(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? (b) Which would you expect to be more soluble in water, cyclohexane or dioxane?

Short Answer

Expert verified
(a) Stearic acid would be more soluble in nonpolar carbon tetrachloride (CCl鈧�) than in polar water due to its long nonpolar hydrocarbon chain dominating the interactions. (b) Dioxane, being a polar compound with hydrogen bonding capacity, is more soluble in water than nonpolar cyclohexane.

Step by step solution

01

(a) Stearic acid solubility in water and carbon tetrachloride

Stearic acid has a polar carboxyl group (\(\mathrm{COOH}\)) and a long nonpolar hydrocarbon chain (\(\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{16}\)). - Water is a polar solvent, thus it can interact with the polar part of stearic acid. - Carbon tetrachloride is a nonpolar solvent, thus it will interact with the nonpolar hydrocarbon chain of stearic acid. Since the nonpolar hydrocarbon chain in stearic acid is much larger than the polar carboxyl group, the interactions between the nonpolar chain and carbon tetrachloride will dominate. Therefore, stearic acid would be more soluble in carbon tetrachloride (CCl鈧�) than in water.
02

(b) Solubility comparison of cyclohexane and dioxane in water

Cyclohexane is a nonpolar compound with no hydrogen bonding capacity, while dioxane has polar bonds and can form hydrogen bonds. - Water is a polar solvent, and it forms hydrogen bonds easily. As a result, dioxane, being a polar compound with hydrogen bonding capacity, is more likely to dissolve in water than the nonpolar compound cyclohexane, which is not capable of forming hydrogen bonds with water molecules. Thus, dioxane is more soluble in water than cyclohexane.

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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, \((\mathbf{d}) \mathrm{HCl}\) in acetonitrile \(\left(\mathrm{CH}_{3} \mathrm{CN}\right)\)

A dilute aqueous solution of an organic compound soluble in water is formed by dissolving 2.35 g of the compound in water to form 0.250 L of solution. The resulting solution has an osmotic pressure of 0.605 atm at \(25^{\circ} \mathrm{C}\) . Assuming that the organic compound is a nonelectrolyte, what is its molar mass?

Carbon disulfide \(\left(\mathrm{CS}_{2}\right)\) boils at \(46.30^{\circ} \mathrm{C}\) and has a density of 1.261 \(\mathrm{g} / \mathrm{mL}\) . (a) When 0.250 \(\mathrm{mol}\) of a nondissociating solute is dissolved in 400.0 \(\mathrm{mL}\) of \(\mathrm{CS}_{2},\) the solution boils at \(47.46^{\circ} \mathrm{C} .\) What is the molal boiling-point-elevation constant for \(\mathrm{CS}_{2}\) ? (b) When 5.39 \(\mathrm{g}\) of a nondissociating unknown is dissolved in 50.0 \(\mathrm{mL}\) of \(\mathrm{CS}_{2},\) the solution boils at \(47.08^{\circ} \mathrm{C} .\) What is the molar mass of the unknown?

Seawater contains 34 g of salts for every liter of solution. Assuming that the solute consists entirely of \(\mathrm{NaCl}\) (in fact, over 90\(\%\) of the salt is indeed NaCl), calculate the osmotic pressure of seawater at \(20^{\circ} \mathrm{C}\) .

A lithium salt used in lubricating grease has the formula \(\mathrm{LiC}_{n} \mathrm{H}_{2 n+1} \mathrm{O}_{2} .\) The salt is soluble in water to the extent of 0.036 \(\mathrm{g}\) per 100 \(\mathrm{g}\) of water at \(25^{\circ} \mathrm{C}\) . The osmotic pressure of this solution is found to be 57.1 torr. Assuming that molality and molarity in such a dilute solution are the same and that the lithium salt is completely dissociated in the solution, determine an appropriate value of \(n\) in the formula for the salt.
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