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Chapter 10: Problem 24

Choose the member of each set that you would expect to be more soluble in water. Explain your answer. (a) chloromethane, \(\mathrm{CH}_{3} \mathrm{Cl}\), or methanol, \(\mathrm{CH}_{3} \mathrm{OH}\) (b) nitrogen triiodide or potassium iodide (c) lithium chloride or ethyl chloride, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{Cl}\) (d) ammonia or methane

Short Answer

Expert verified
a) Chloromethane or Methanol b) Nitrogen Triiodide or Potassium Iodide c) Lithium Chloride or Ethyl Chloride d) Ammonia or Methane Answer: a) Methanol b) Potassium Iodide c) Lithium Chloride d) Ammonia

Step by step solution

01

Problem (a) - Chloromethane or Methanol

Chloromethane (\(\mathrm{CH}_{3} \mathrm{Cl}\)) is a slightly polar molecule due to the electronegativity difference between carbon and chlorine atoms. Methanol (\(\mathrm{CH}_{3} \mathrm{OH}\)), on the other hand, is polar and can form hydrogen bonds with water due to the presence of an -OH group. Hydrogen bonding increases the solubility of substances in water. Between the two, methanol (\(\mathrm{CH}_{3} \mathrm{OH}\)) is expected to be more soluble in water due to its ability to form hydrogen bonds with water molecules.
02

Problem (b) - Nitrogen Triiodide or Potassium Iodide

Nitrogen triiodide is a covalent compound, whereas potassium iodide is an ionic compound. In general, polar water molecules can more effectively solvate ions than nonpolar molecules. This means that potassium iodide, an ionic compound, will have higher solubility in water than the covalent nitrogen triiodide. Therefore, potassium iodide is expected to be more soluble in water than nitrogen triiodide.
03

Problem (c) - Lithium Chloride or Ethyl Chloride

Lithium chloride is an ionic compound composed of lithium and chloride ions. Ethyl chloride (\(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{Cl}\)) is a slightly polar molecule with lesser polarity than lithium chloride. As water is a polar solvent and can effectively solvate ions, lithium chloride is expected to be more soluble in water than ethyl chloride.
04

Problem (d) - Ammonia or Methane

Ammonia is a polar molecule and can form hydrogen bonds with water molecules due to the presence of nitrogen-containing polar bond. Methane is a nonpolar molecule with no hydrogen bonding ability. Based on the polarity and ability to form hydrogen bonds, ammonia is expected to be more soluble in water than methane.

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Most popular questions from this chapter

The freezing point of \(0.20 \mathrm{~m}\) HF is \(-0.38^{\circ} \mathrm{C}\). Is HF primarily nonionized in this solution (HF molecules), or is it dissociated to \(\mathrm{H}^{+}\) and \(\mathrm{F}^{-}\) ions?

Chloroform \(\left(\mathrm{CH} \mathrm{Cl}_{3}\right)\) boils at \(61.7^{\circ} \mathrm{C}\) and has a density of \(1.49 \mathrm{~g} / \mathrm{mL}\). (a) A solution prepared by dissolving \(0.146 \mathrm{~mol}\) of a nonelectrolyte in \(132 \mathrm{~mL}\) of chloroform boils at \(64.4^{\circ} \mathrm{C}\). What is the boiling point constant \(\left(k_{\mathrm{b}}\right)\) for chloroform? (b) Another solution is prepared by dissolving \(45.2 \mathrm{~g}\) of an unknown electrolyte (MM = \(154 \mathrm{~g} / \mathrm{mol}\) ) in \(427.5 \mathrm{~mL}\) of chloroform. The resulting solution boils at \(66.7^{\circ} \mathrm{C}\). What is \(i\) for the electrolyte?

What is the osmotic pressure of a \(0.250 \mathrm{M}\) solution of \(\mathrm{K}_{2} \mathrm{CO}_{3}\) at \(25^{\circ} \mathrm{C}\) ? (Assume complete dissociation.)

The Rast method uses camphor \(\left(\mathrm{C}_{10} \mathrm{H}_{16} \mathrm{O}\right)\) as a solvent for determining the molar mass of a compound. When \(2.50 \mathrm{~g}\) of cortisone acetate is dissolved in \(50.00 \mathrm{~g}\) of camphor \(\left(k_{\mathrm{f}}=40.0^{\circ} \mathrm{C} / \mathrm{m}\right)\), the freezing point of the mixture is determined to be \(173.44^{\circ} \mathrm{C}\); that of pure camphor is \(178.40^{\circ} \mathrm{C}\). What is the molar mass of cortisone acetate?

A solution is prepared by diluting \(225 \mathrm{~mL}\) of \(0.1885 \mathrm{M}\) aluminum sulfate solution with water to a final volume of \(1.450 \mathrm{~L}\). Calculate (a) the number of moles of aluminum sulfate before dilution. (b) the molarities of the aluminum sulfate, aluminum ions, and sulfate ions in the diluted solution.
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