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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 carbon tetrachloride due to its predominantly non-polar nature. (b) Dioxane would be more soluble in water than cyclohexane due to its polar nature and ability to form hydrogen bonds with water molecules.

Step by step solution

01

(a) Determine the polarity and solubility of stearic acid in water and carbon tetrachloride

Stearic acid is chemically represented as \(\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{16} \mathrm{COOH}\). The long carbon chain makes the compound mostly non-polar, but the carboxylic acid group \(\mathrm{COOH}\) has a polar nature due to the presence of electronegative oxygen atoms. Even though the molecule has that polar moiety, the large non-polar part will dominate the solubility preference of the molecule. Therefore, since carbon tetrachloride (\(\mathrm{CCl}_4\)) is a non-polar solvent, stearic acid will be more soluble in carbon tetrachloride than in polar water.
02

(b) Determine the polarity and solubility of cyclohexane and dioxane in water

Cyclohexane is a non-polar hydrocarbon molecule that contains only C and H atoms. Hence, it tends to be more soluble in non-polar solvents. On the other hand, dioxane is a molecule with oxygen atoms making it moderately polar due to the oxygen atoms interacting with the hydrogen atoms of water via hydrogen bonding. Comparing the solubility of cyclohexane and dioxane in water, dioxane is expected to be more soluble in water than cyclohexane due to its polar nature, and ability to form hydrogen bonds with water molecules.

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Most popular questions from this chapter

Calculate the molality of each of the following solutions: (a) \(10.0 \mathrm{~g}\) of benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) dissolved in \(50.0 \mathrm{~g}\) of carbon tetrachloride \(\left(\mathrm{CCl}_{4}\right),(\mathbf{b}) 5.00 \mathrm{~g}\) of \(\mathrm{NaCl}\) dissolved in \(0.100 \mathrm{~L}\) of water.

Calculate the number of moles of solute present in each of the following solutions: (a) \(255 \mathrm{~mL}\) of \(1.50 \mathrm{M} \mathrm{HNO}_{3}(a q)\) (b) \(50.0 \mathrm{mg}\) of an aqueous solution that is $1.50 \mathrm{~m} \mathrm{NaCl}$, (c) \(75.0 \mathrm{~g}\) of an aqueous solution that is \(1.50 \%\) sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) by mass.

(a) What is the molality of a solution formed by dissolving 1.12 mol of KCl in 16.0 mol of water? (b) How many grams of sulfur \(\left(\mathrm{S}_{8}\right)\) must be dissolved in \(100.0 \mathrm{~g}\) of naphthalene $\left(\mathrm{C}_{10} \mathrm{H}_{8}\right)\( to make a \)0.12 \mathrm{~m}$ solution?

Soaps consist of compounds such as sodium stearate, $\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{16} \mathrm{COO}^{-} \mathrm{Na}^{+},$ that have both hydrophobic and hydrophilic parts. Consider the hydrocarbon part of sodium stearate to be the "tail" and the charged part to be the "head." (a) Which part of sodium stearate, head or tail, is more likely to be solvated by water? (b) Grease is a complex mixture of (mostly) hydrophobic compounds. Which part of sodium stearate, head or tail, is most likely to bind to grease? (c) If you have large deposits of grease that you want to wash away with water, you can see that adding sodium stearate will help you produce an emulsion. What intermolecular interactions are responsible for this?

Indicate whether each statement is true or false: (a) The higher the temperature, the more soluble most gases are in water. (b) The higher the temperature, the more soluble most ionic solids are in water. (c) As you cool a saturated solution from high temperature to low temperature, solids start to crystallize out of solution if you achieve a supersaturated solution. (d) If you take a saturated solution and raise its temperature, you can (usually) add more solute and make the solution even more concentrated.
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