This figure shows the interaction of a cation with surrounding water molecules. (b) Which of the following explanations accounts for the fact that the ion–solvent interaction is greater for Li⁺ than for K⁺? a. Li⁺ is of lower mass than K⁺. b. The ionization energy of Li is higher than that for K. c. Li⁺ has a smaller ionic radius than K⁺. d. Li has a lower density than K. e. Li reacts with water more slowly than K. [Section 13.1]

Consider two ionic solids, both composed of singly charged ions, that have different lattice energies. (b) If not, which solid will be more soluble in water, the one with the larger lattice energy or the one with the smaller lattice energy? Assume that solute–solvent interactions are the same for both solids. [Section 13.1]

The structures of vitamins E and B6 are shown below. Predict which is more water soluble and which is more fat soluble. [Section 13.3]

The figure shows two identical volumetric flasks containing the same solution at two temperatures. (b) Does the molality of the solution change with the change in temperature? [Section 13.4]

This portion of a phase diagram shows the vapor–pressure curves of a volatile solvent and of a solution of that solvent containing a nonvolatile solute. (b) What are the normal boiling points of the solvent and the solution? [Section 13.5]

Suppose you had a balloon made of some highly flexible semipermeable membrane. The balloon is filled completely with a 0.2 M solution of some solute and is submerged in a 0.1 M solution of the same solute:

Initially, the volume of solution in the balloon is 0.25 L. Assuming the volume outside the semipermeable membrane is large, as the illustration shows, what would you expect for the solution volume inside the balloon once the system has come to equilibrium through osmosis? [Section 13.5]

The diagrams shown represent an emulsion, a true solution, and a liquid crystal. The colored balls represent different liquid molecules. Which diagram corresponds to which type of mixture? [Section 13.6]

Indicate the type of solute–solvent interaction that should be most important in each of the following solutions: a. CCl4 in benzene (C₆H₆),

Indicate the type of solute–solvent interaction that should be most important in each of the following solutions: b. methanol (CH3OH) in water,

 Indicate the type of solute–solvent interaction that should be most important in each of the following solutions: c. KBr in water,

Indicate the type of solute–solvent interaction that should be most important in each of the following solutions: d. HCl in acetonitrile (CH₃CN).

Indicate the principal type of solute–solvent interaction in each of the following solutions and rank the solutions from weakest to strongest solute–solvent interaction: (a) KCl in water

Indicate the principal type of solute–solvent interaction in each of the following solutions and rank the solutions from weakest to strongest solute–solvent interaction: (b) CH₂Cl₂ in benzene (C₆H₆)

Indicate the principal type of solute–solvent interaction in each of the following solutions and rank the solutions from weakest to strongest solute–solvent interaction: (c) methanol (CH₃OH) in water

An ionic compound has a very negative ∆H_soln in water (b) Which term would you expect to be the largest negative number: ∆H_solvent, ∆H_solute, or ∆H_mix?

When ammonium chloride dissolves in water, the solution becomes colder. (a) Is the solution process exothermic or endothermic?

When ammonium chloride dissolves in water, the solution becomes colder. (b) Why does the solution form?

Two nonpolar organic liquids, hexane (C₆H₁₄) and heptane (C₇H₁₆), are mixed. (a) Do you expect ∆H_soln to be a large positive number, a large negative number, or close to zero? Explain.

Two nonpolar organic liquids, hexane (C₆H₁₄) and heptane (C₇H₁₆), are mixed. (b) Hexane and heptane are miscible with each other in all proportions. In making a solution of them, is the entropy of the system increased, decreased, or close to zero, compared to the separate pure liquids?

KBr is relatively soluble in water, yet its enthalpy of solution is + 19.8 kJ/mol. Which of the following statements provides the best explanation for this behavior? (a) Potassium salts are always soluble in water. (b) The entropy of mixing must be unfavorable. (c) The enthalpy of mixing must be small compared to the enthalpies for breaking up water–water interactions and K–Br ionic interactions. (d) KBr has a high molar mass compared to other salts like NaCl.

By referring to Figure 13.15, determine whether the addition of 40.0 g of each of the following ionic solids to 100 g of water at 40 °C will lead to a saturated solution:(c) K₂Cr₂O₇

By referring to Figure 13.15, determine whether the addition of 40.0 g of each of the following ionic solids to 100 g of water at 40 °C will lead to a saturated solution: (d) Pb(NO₃)₂.

By referring to Figure 13.15, determine the mass of each of the following salts required to form a saturated solution in 250 g of water at 30 °C: (b) Pb(NO₃)₂,

By referring to Figure 13.15, determine the mass of each of the following salts required to form a saturated solution in 250 g of water at 30 °C: (c) Ce₂(SO₄)₃.

Oil and water are immiscible. Which is the most likely reason? (a) Oil molecules are denser than water. (b) Oil molecules are composed mostly of carbon and hydrogen. (c) Oil molecules have higher molar masses than water. (d) Oil molecules have higher vapor pressures than water. (e) Oil molecules have higher boiling points than water.

Which of the following in each pair is likely to be more soluble in hexane, C₆H₁₄: b. benzene (C₆H₆) or glycerol, CH₂(OH)CH(OH)CH₂OH,

Which of the following in each pair is likely to be more soluble in water: (a) cyclohexane (C₆H₁₂) or glucose (C₆H₁₂O₆),

Which of the following in each pair is likely to be more soluble in water: (c) HCl or ethyl chloride (CH₃CH₂Cl)? Explain in each case.

Indicate whether each statement is true or false: (d) If you take a saturated solution and raise its temperature, you can (usually) add more solute and make the solution even more concentrated.

(a) Calculate the mass percentage of Na₂SO₄ in a solution containing 10.6 g of Na₂SO₄ in 483 g of water.