Problem 50
From the solubility data given, calculate the solubility products for the following compounds: (a) \(\mathrm{SrF}_{2}\), \(7.3 \times 10^{-2} \mathrm{~g} / \mathrm{L},\) (b) \(\mathrm{Ag}_{2} \mathrm{PO}_{4}, 6.7 \times 10^{-3} \mathrm{~g} / \mathrm{L}\)
Problem 51
The molar solubility of \(\mathrm{MnCO}_{3}\) is \(4.2 \times 10^{-6} \mathrm{M}\). What is \(K_{\mathrm{sp}}\) for this compound?
Problem 52
The solubility of an ionic compound MX (molar mass = \(346 \mathrm{~g}\) ) is \(4.63 \times 10^{-3} \mathrm{~g} / \mathrm{L}\). What is \(K_{\mathrm{sp}}\) for this compound?
Problem 53
The solubility of an ionic compound \(\mathrm{M}_{2} \mathrm{X}_{3}\) (molar mass \(=288 \mathrm{~g}\) ) is \(3.6 \times 10^{-17} \mathrm{~g} / \mathrm{L}\). What is \(K_{\mathrm{sp}}\) for this compound?
Problem 56
The \(\mathrm{pH}\) of a saturated solution of a metal hydroxide MOH is 9.68 . Calculate the \(K_{s p}\) for this compound.
Problem 58
A volume of \(75 \mathrm{~mL}\) of \(0.060 \mathrm{M} \mathrm{NaF}\) is mixed with 25 \(\mathrm{mL}\) of \(0.15 \mathrm{M} \mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2} .\) Calculate the concentrations in the final solution of \(\mathrm{NO}_{3}^{-}, \mathrm{Na}^{+}, \mathrm{Sr}^{2+}\), and \(\mathrm{F}^{-}\). \(\left(K_{\mathrm{sp}}\right.\) for \(\left.\mathrm{SrF}_{2}=2.0 \times 10^{-10} .\right)\)
Problem 59
How does the common ion effect influence solubility equilibria? Use Le Châtelier's principle to explain the decrease in solubility of \(\mathrm{CaCO}_{3}\) in an \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) solution.
Problem 60
The molar solubility of \(\mathrm{AgCl}\) in \(6.5 \times 10^{-3} \mathrm{M} \mathrm{AgNO}_{3}\) is \(2.5 \times 10^{-8} M\). In deriving \(K_{\mathrm{sp}}\) from these data, which of the following assumptions are reasonable? (a) \(K_{\mathrm{sp}}\) is the same as solubility. (b) \(K_{\mathrm{sp}}\) of \(\mathrm{AgCl}\) is the same in \(6.5 \times 10^{-3} \mathrm{M} \mathrm{AgNO}_{3}\) as in pure water. (c) Solubility of \(\mathrm{AgCl}\) is independent of the concentration of \(\mathrm{AgNO}_{3}\). (d) \(\left[\mathrm{Ag}^{+}\right]\) in solution does not change significantly upon the addition of \(\mathrm{AgCl}\) to \(6.5 \times 10^{-3} \mathrm{M} \mathrm{AgNO}_{3}\). (e) \(\left[\mathrm{Ag}^{+}\right]\) in solution after the addition of \(\mathrm{AgCl}\) to \(6.5 \times 10^{-3} \mathrm{M}\) \(\mathrm{AgNO}_{3}\) is the same as it would be in pure water.
Problem 61
Give an example to illustrate the general effect of complex ion formation on solubility.
Problem 63
The solubility product of \(\mathrm{PbBr}_{2}\) is \(8.9 \times 10^{-6} .\) Determine the molar solubility in (a) pure water, (b) \(0.20 M \mathrm{KBr}\) solution, and (c) \(0.20 \mathrm{M} \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) solution.
