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Chapter 15: Q61E (page 875)
Question: Under what circumstances, if any, does a sample of solid AgCl completely dissolve in pure water?
A saturated solution is not produced because of the small amount of solid.
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Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that it is not appropriate to neglect the changes in the initial concentrations of the common ions.
(a) \(TlCl(s)\) in \(0.025MTlN{O_3}\)
(b) \(Ba{F_2}(\;s)\) in \(0.0313M\;KF\)
(c) \(Mg{C_2}{O_4}\) in \(2.250\;L\)of a solution containing \(8.156\;g\) of \(Mg{\left( {N{O_3}} \right)_2}\)
(d) \(Ca{(OH)_2}(\;s)\) in an unbuffered solution initially with a pH of \(12.700\)
Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product:
\(\begin{array}{l}(a)KH{C_4}{H_4}{O_6}\\(b)Pb{I_2}\\(c)A{g_4}\left[ {Fe{{(CN)}_6}} \right],a salt containing the Fe{(CN)_4}^ - ion\\(d)H{g_2}{I_2}\end{array}\)
Question: What are the concentrations of Ag+, CN–, and Ag (CN)2− in a saturated solution of AgCN?
Question: Calculate the cadmium ion concentration, \(\left( {C{d^{2 + }}} \right)\)in a solution prepared by mixing 0.100 L of 0.0100 M \(Cd{\left( {N{O_3}} \right)_2}\)with 1.150 L of 0.100 \(N{H_3}(aq)\).
To a \({\bf{0}}.{\bf{10M}}\) solution of \({\bf{Pb}}{\left( {{\bf{N}}{{\bf{O}}_{\bf{3}}}} \right)_{\bf{2}}}\) is added enough \({\bf{HF}}\left( {\bf{g}} \right)\) to make\(\left[ {{\bf{HF}}} \right]{\rm{ }} = {\rm{ }}{\bf{0}}.{\bf{10}}{\rm{ }}{\bf{M}}\).
(a) Does \({\bf{Pb}}{{\bf{F}}_{\bf{2}}}\) precipitate from this solution? Show the calculations that support your conclusion.
(b) What is the minimum pH at which \({\bf{Pb}}{{\bf{F}}_{\bf{2}}}\) precipitates?
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