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Chapter 15: Q39 E (page 873)
What [F-] is required to reduce [Ca2+] to 1.0脳10-4M by precipitation of CaF2?
The required [F-] = 6.2 脳10-4M
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Question: Using the dissociation constant, \({K_d} = 3.4 \times 1{0^{ - 15}}\), calculate the equilibrium concentrations of \(Z{n^{2 + }}\;and\;O{H^ - }in{\rm{\;}}\)\({\rm{\;}}a\;0.0465 - M\)solution of \(Zn(OH)_4^{2 - }\).
A \({\bf{0}}.{\bf{125}}{\rm{ }}{\bf{M}}\) solution of \({\bf{Mn}}{\left( {{\bf{N}}{{\bf{O}}_{\bf{3}}}} \right)_{\bf{2}}}\) is saturated with\({{\bf{H}}_{\bf{2}}}{\bf{S}}{\rm{ }}\left( {\left[ {{{\bf{H}}_{\bf{2}}}{\bf{S}}} \right]{\rm{ }} = {\rm{ }}{\bf{0}}.{\bf{10}}{\rm{ }}{\bf{M}}} \right)\). At what pH does MnS begin to precipitate?
\(MnS(s) \rightleftharpoons M{n^{2 + }}(aq) + {S^{2 - }}(aq)\quad {K_{sp}} = 4.3 \times 1{0^{ - 22}}\)
\({H_2}S(aq) + 2{H_2}O(l) \rightleftharpoons 2{H_3}{O^ + }(aq) + {S^{2 - }}(aq)\quad K = 1.0 \times 1{0^{ - 26}}\)
Question: What are the concentrations of Ag+, CN鈥�, and Ag (CN)2鈭� in a saturated solution of AgCN?
Question: Using the dissociation constant, \({K_d} = 1 \times 1{0^{ - 44}}\), calculate the equilibrium concentrations of \(F{e^{3 + }}\;and\;C{N^ - }\) in a \(0.333M\) solution of \(Fe(CN)_6^{3 - }\).
Iron concentrations greater than 5.4脳10-6M in water used for laundrypurposes can cause staining. What [OH-] is required to reduce [Fe2+] to this level by precipitation of Fe(OH)2?
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