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Chapter 13: Problem 29

Common laboratory solvents include acetone $\left(\mathrm{CH}_{3} \mathrm{COCH}_{3}\right)\(, methanol \)\left(\mathrm{CH}_{3} \mathrm{OH}\right)\(, toluene \)\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CH}_{3}\right),$ and water. Which of these is the best solvent for nonpolar solutes?

Short Answer

Expert verified
Toluene \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CH}_{3}\right)\) is the best solvent for nonpolar solutes among the given common laboratory solvents, as it is a nonpolar solvent itself, and "like dissolves like."

Step by step solution

01

Determine the polarity of acetone

Acetone (CH3COCH3) has a carbonyl group (C=O) in the middle of its structure, making the molecule polar. Oxygen is more electronegative than carbon, creating a dipole moment in the carbonyl group, which makes acetone a polar solvent.
02

Determine the polarity of methanol

Methanol (CH3OH) contains an oxygen-hydrogen (O-H) bond, which is polar due to the high electronegativity difference between oxygen and hydrogen. As a result, methanol is a polar solvent.
03

Determine the polarity of toluene

Toluene (C6H5CH3) has a benzene ring (C6H5) bonded to a methyl group (CH3). Both the benzene ring and the methyl group are composed of carbon and hydrogen atoms, with very little difference in electronegativity, making toluene a nonpolar solvent.
04

Determine the polarity of water

Water (H2O) is a well-known polar solvent due to its bent shape and the large difference in electronegativity between oxygen and hydrogen. This results in a dipole moment, making water a polar solvent.
05

Identify the best solvent for nonpolar solutes

Considering the polarity of each solvent, we can conclude that toluene, being a nonpolar solvent, will be the best choice for dissolving nonpolar solutes among the given common laboratory solvents.

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Most popular questions from this chapter

Calculate the molarity of the following aqueous solutions: (a) \(0.640 \mathrm{~g}\) of \(\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) in \(500.0 \mathrm{~mL}\) of solution, (b) \(50.0 \mathrm{~g}\) of \(\mathrm{LiClO}_{4} \cdot 3 \mathrm{H}_{2} \mathrm{O}\) in $250 \mathrm{~mL}$ of solution, (c) \(125 \mathrm{~mL}\) of \(3.00 \mathrm{M}\) \(\mathrm{HNO}_{3}\) diluted to \(1.00 \mathrm{~L}\)

(a) Do colloids made only of gases exist? Why or why not? (b) In the 1850s, Michael Faraday prepared ruby-red colloids of gold nanoparticles in water that are still stable today. These brightly colored colloids look like solutions. What experiment(s) could you do to determine whether a given colored preparation is a solution or colloid?

(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?

At \(35^{\circ} \mathrm{C}\) the vapor pressure of acetone, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{CO},\) is 47.9 \(\mathrm{kPa}\), and that of carbon disulfide, \(\mathrm{CS}_{2}\), is \(66.7 \mathrm{kPa}\). A solution composed of an equal number of moles of acetone and carbon disulfide has a vapor pressure of \(86.7 \mathrm{kPa}\) at $35^{\circ} \mathrm{C} .(\mathbf{a})$ What would be the vapor pressure of the solution if it exhibited ideal behavior? (b) Based on the behavior of the solution, predict whether the mixing of acetone and carbon disulfide is an exothermic \(\left(\Delta H_{\text {soln }}<0\right)\) or endothermic $\left(\Delta H_{\text {soln }}>0\right)$ process.

Indicate whether each statement is true or false: (a) If you compare the solubility of a gas in water at two different temperatures, you find the gas is more soluble at the lower temperature. (b) The solubility of most ionic solids in water decreases as the temperature of the solution increases. (c) The solubility of most gases in water decreases as the temperature increases because water is breaking its hydrogen bonding to the gas molecules as the temperature is raised. (d) Some ionic solids become less soluble in water as the temperature is raised.
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