Solubility Equilibria

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Calculate the concentrations of Ag $^+$ , Ag(S $_2$ O $_3$ ) $^-$ , and Ag(S $_2$ O $_3$ ) $_2^{3-}$ in a solution prepared by mixing 150.0 mL of 1.00 x 10 $^{-3}$ M AgNO $_3$ with 200.0 mL of 5.00 M Na $_2$ S $_2$ O $_3$ . The stepwise formation equilibria are:

Ag $^+$ + S $_2$ O $_3^{2-}$ $\leftrightharpoons$ Ag(S $_2$ O $_3$ ) $^-$ K $_{f1}$ = 7.4 x 10 $^{8}$

Ag(S $_2$ O $_3$ ) $^-$ + S $_2$ O $_3^{2-}$ $\leftrightharpoons$ Ag(S $_2$ O $_3$ ) $_2^{3-}$ K $_{f2}$ = 3.9 x 10 $^{4}$

Posted by Dalton Wylde a year ago

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