Solubility Product Problems

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0.25 moles of AgNO $_3$ are dissolved in 1 L of 0.60 M NaCN and 1 mole of NaCl is added. Will AgCl precipitate?

AgCl K $_{sp}$ = 1.8 x 10 $^{-10}$

Ag(CN) $_2^-$ K $_{f}$ = 5.6 x 10 $^{18}$

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Calculate the solubility (in grams per liter) of PbI $_2$ in water from the solubility product constant 1.4 x 10 $^{-8}$ .

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What are the concentrations of the ionic species in a saturated solution of Ag $_2$ CrO $_4$

K $_{sp}$ = 1.1 x 10 $^{-12}$

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Calculate the equilibrium concentration of Pb $^{2+}$ , I $^-$ , Na(\^+ $, and NO$ _3^- $when 100.0 mL of 0.0500 M Pb(NO$ _3 $)$ _2## and 200.0 mL of 0.100 M NaI are mixed.

PbI $_2$ K $_{sp}$ = 1.4 x 10 $^{-8}$

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How many moles of Mg(OH) $_2$ can be dissolved in a 1 L solution that already contains 0.52 moles Mg $^{2+}$ .

Mg(OH) $_2$ K $_{sp}$ = 8.9 x 10 $^{-12}$

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