Question

The concentration of $ A{{g}^{+}} $ ion in a given saturated solution of $ AgCl $ at $ 25{}^\circ C $ is $ 1.06\times {{10}^{-5}}g- $ ion per litre. Thus, the solubility product of $ AgCl $ is

• A. $ 0.353\times {{10}^{-10}} $
• B. $ 0.530\times {{10}^{-10}} $
• C. $ 1.12\times {{10}^{-10}} $
• D. $ 2.12\times {{10}^{-10}} $

Answer 1

The Correct Option is C

$[Ag^+] = 1.06 \times 10^{-5} \,g - ion/L$ $ = 1.06 \times 10^{-5} \,mol/L = [Cl^-]$ $AgCl(s) {<=>} Ag^+ + Cl^-$ $K_{sp} = [Ag^+][Cl^-]$ $= (1.06 \times 10^{-5})^2$ $ = 1.12 \times 10^{-10}$