Silver carbonate dissolves according to At

CHEMISTRY · Multi-part · AP · Chemistry · Equilibrium · Equilibrium

Problem

Silver carbonate dissolves according to

Ag_2CO_3(s) \rightleftharpoons 2\,Ag^+(aq) + CO_{3}^{2-}(aq)

25\,^\circ\text{C}

, the solubility–product constant is

K_{sp}=8.1\times10^{-12}

. A chemist adds

0.500\,\text{g}

of finely powdered

Ag_2CO_3

(molar mass =

275.8\,\text{g mol}^{-1}

) to

1.00\,\text{L}

of pure water at

25\,^\circ\text{C}

, seals the vessel, and allows the system to reach equilibrium. (a) Calculate the maximum mass of

Ag_2CO_3

that can dissolve in

1.00\,\text{L}

of water under these conditions. Show all steps clearly. (b) Determine the mass of solid

Ag_2CO_3

that will remain undissolved at equilibrium. (c) Using both the value of

K_{sp}

and the results from parts (a) and (b), classify

Ag_2CO_3

as soluble, sparingly soluble, or effectively insoluble in water at

25\,^\circ\text{C}

. Explain how your numerical findings support the classification.