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Chapter 13: Problem 14

Indicate whether each statement is true or false: \((\) a) \(\mathrm{NaCl}\) dissolves in water but not in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) because benzene is denser than water. (b) NaCl dissolves in water but not in benzene because water has a large dipole moment and benzene has zero dipole moment. (c) NaCl dissolves in water but not in benzene because the water-ion interactions are stronger than benzene-ion interactions.

Short Answer

Expert verified
(a) False, (b) True, (c) True. The solubility of NaCl depends on the interactions between the solute and the solvent, not their densities. NaCl dissolves in polar solvents like water due to its large dipole moment, and strong water-ion interactions. It does not dissolve in nonpolar solvents like benzene with zero dipole moment and weak benzene-ion interactions.

Step by step solution

01

Statement A: NaCl dissolves in water but not in benzene because benzene is denser than water.

This statement is false because the solubility of NaCl in a solvent depends on the interactions between the solute (NaCl) and the solvent (water or benzene), not on the density of the solvent.
02

Statement B: NaCl dissolves in water but not in benzene because water has a large dipole moment and benzene has zero dipole moment.

This statement is true. NaCl is an ionic compound, so it dissolves in polar solvents like water, which have a large dipole moment. Benzene, being a nonpolar solvent with zero dipole moment, cannot dissolve NaCl due to lack of strong interactions between the ions of NaCl and benzene molecules.
03

Statement C: NaCl dissolves in water but not in benzene because the water-ion interactions are stronger than benzene-ion interactions.

This statement is also true. In order for NaCl to dissolve in a solvent, the solvent-solute interactions must be strong enough to overcome the ionic bonds in NaCl. In water, the strong water-ion interactions, due to hydrogen bonding, are capable of breaking the ionic bonds in NaCl and allowing it to dissolve. However, in benzene, the interactions between the benzene molecules and the ions in NaCl are weak, so NaCl does not dissolve.

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Most popular questions from this chapter

A solution contains \(0.50 \mathrm{~mol} \mathrm{H}_{2} \mathrm{O}\) and an unknown number of moles of sodium chloride. The vapor pressure of the solution at \(29^{\circ} \mathrm{C}\) is \(3.85 \mathrm{kPa}\). The vapor pressure of pure water at this temperature is \(4.05 \mathrm{kPa}\). Calculate the number of grams of sodium chloride in the solution. (Hint: Remember that sodium chloride is a strong electrolyte.)

Compounds like sodium stearate, called "surfactants" in general, can form structures known as micelles in water, once the solution concentration reaches the value known as the critical micelle concentration (cmc). Micelles contain dozens to hundreds of molecules. The cmc depends on the substance, the solvent, and the temperature. At and above the \(\mathrm{cmc}\), the properties of the solution vary drastically. (a) The turbidity (the amount of light scattering) of solutions increases dramatically at the \(\mathrm{cmc}\). Suggest an explanation. (b) The ionic conductivity of the solution dramatically changes at the \(\mathrm{cmc}\). Suggest an explanation. (c) Chemists have developed fluorescent dyes that glow brightly only when the dye molecules are in a hydrophobic environment. Predict how the intensity of such fluorescence would relate to the concentration of sodium stearate as the sodium stearate concentration approaches and then increases past the \(\mathrm{cmc}\).

A dilute aqueous solution of fructose in water is formed by dissolving $1.25 \mathrm{~g}\( of the compound in water to form \)0.150 \mathrm{~L}$ of solution. The resulting solution has an osmotic pressure of \(112.8 \mathrm{kPa}\) at \(20^{\circ} \mathrm{C}\). Assuming that the organic compound is a nonelectrolyte, what is its molar mass?

A "canned heat" product used to warm buffet dishes consists of a homogeneous mixture of ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) and paraffin, which has an average formula of $\mathrm{C}_{24} \mathrm{H}_{50}\(. What mass of \)\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ should be added to \(620 \mathrm{~kg}\) of the paraffin to produce $1.07 \mathrm{kPa}\( of ethanol vapor pressure at \)35^{\circ} \mathrm{C}$ ? The vapor pressure of pure ethanol at \(35^{\circ} \mathrm{C}\) is \(13.3 \mathrm{kPa}\).

Which two statements about gas mixtures are true? [Section 13.1] (a) Gases always mix with other gases because the gas particles are too far apart to feel significant intermolecular attractions or repulsions. (b) Just like water and oil don't mix in the liquid phase, two gases can be immiscible and not mix in the gas phase. (c) If you cool a gaseous mixture, you will liquefy all the gases at the same temperature. (d) Gases mix in all proportions in part because the entropy of the system increases upon doing so.
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