Question

Determine solubility of \(\mathrm{AgBr}\) in a \(0.1\mathrm{\ M\ KCN}\) solution. \([K_f \text{ of } [\mathrm{Ag(CN)_2}]^- = 5.6 \times 10^8; K_{sp} \text{ of } \mathrm{AgBr} = 7.7 \times 10^{-13}]\)

• A. \(2 \times 10^{-3}\mathrm{\ M}\)
• B. \(4 \times 10^{-6}\mathrm{\ M}\)
• C. \(2 \times 10^{-6}\mathrm{\ M}\)
• D. \(4 \times 10^{-3}\mathrm{\ M}\)

Hint:

Overall equilibrium constant \(K = K_{sp} \times K_f\).

Answer 1

The Correct Option is A