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Chapter 15: Q54E (page 839)
Question: Calculate the molar solubility of \(AgBr\;in\; 0.035MNaBr\left( {{K_{sp}} = 5 \times 1{0^{ - 13}}} \right)\).
The molar solubility is \(1.43 \cdot {10^{ - 11}}{\rm{M}}\) .
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Magnesium hydroxide and magnesium citrate function as mild laxatives when they reach the small intestine. Why do magnesium hydroxide and magnesium citrate, two very different substances, have the same effect in your small intestine. (Hint: The contents of the small intestine are basic.)
Question: Using Lewis structures, write balanced equations for the following reactions:
\({\rm{\;}}(a)\;HCl(g) + P{H_3}(g) \to \)
\({\rm{\;}}(b)\;{H_3}{O^ + } + CH_3^ - \to \)
\({\rm{\;}}(c)\;CaO + S{O_3} \to \)
\(\;(d)\;NH_4^ + + {C_2}{H_5}{O^ - } \to \)
Question: The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, 鈥揘H2, and a carboxylic acid group, 鈥揅O2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid, CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3.
(a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH.
(b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the 鈥揘H2 and 鈭扖O2鈭� groups.)
Question: 29. The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate \({K_{sp}}\) for each of the slightly soluble solids indicated:
(a) TlCl:\(\left( {T{l^ + }} \right) = 1.21 \times 1{0^{ - 2}}M,\left( {C{l^ - }} \right) = 1.2 \times 1{0^{ - 2}}M\)
(b)\(Ce{\left( {I{O_3}} \right)_4}:\left( {C{e^{4 + }}} \right) = 1.8 \times 1{0^{ - 4}}M,\left( {I{O_3}^ - } \right) = 2.6 \times 1{0^{ - 13}}M\)
(c)\(G{d_2}{\left( {S{O_4}} \right)_3}:\left( {G{d^{3 + }}} \right) = 0.132M,\left( {SO_4^{2 - }} \right) = 0.198M\)
(d)\(A{g_2}S{O_4}:\left( {A{g^ + }} \right) = 2.40 \times 1{0^{ - 2}}M,\left( {SO_4^{2 - }} \right) = 2.05 \times 1{0^{ - 2}}M\)
(e) \(BaS{O_4}:\left( {B{a^{2 + }}} \right) = 0.500M,\left( {SO_4^{2 - }} \right) = 2.16 \times 1{0^{ - 10}}M\)
Question: 30. Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for \({K_{sp}}\) values.)
(a) \(KCl{O_4}:\left( {{K^ + }} \right) = 0.01{M^ - }\left( {ClO_4^ - } \right) = 0.01M\)
(b) \({K_2}PtC{l_6}:\left( {{K^ + }} \right) = 0.01M,\left( {PtC{l_6}^{2 - }} \right) = 0.01M\) \(\)
(c) \(Pb{I_2}:\left( {P{b^{2 + }}} \right) = 0.003M,\left( {{I^ - }} \right) = 1.3 \times 1{0^{ - 3}}M\)
(d) \(A{g_2}\;S:\left( {A{g^ + }} \right) = 1 \times 1{0^{ - 10}}M,\left( {{S^{2 - }}} \right) = 1 \times 1{0^{ - 13}}M\)
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