Question

In a sautrated solution of the sparingly soluble strong electrolyte $AgIO_3$ (Molecular mass $= 283$) the equilibrium which sets in is ${AgIO_{3(s)}<=>Ag^+_{(aq)} +IO^{-}_{3(aq)}}$ If the solubility product constant $K_{sp}$ of $AgIO_3$ at a given temperature is $1.0 ??10^{-8}$, what is the mass of $AgIO_3$ contained in $100\, ml$ of its saturated solution?

• A. $28.3 ??10^{-2}\, g$
• B. $28.3 ??10^{-3}\, g$
• C. $1.0 ??10^{-7}\, g$
• D. $1.0 ??10^{-4}\, g$

Answer 1

Answer: (B)

$28.3 ??10^{-3}\, g$

Answer 2

${AgIO_{3(s)}<=>Ag^+_{(aq)} +IO^{-}_{3(aq)}}$ Let the solubility of $AgIO_3$ be s $K_{sp}=\left[Ag^{+}\right]\left[IO^{-}_{3}\right]$ $1.0\times10^{-8}=S^{2}$ $S=10^{-4}\,mol/litre$ $=\frac{10^{-4}\times283}{1000}\times100$ $=283\times10^{-5}$ $=2.83\times10^{-3}\,g/ 100\, ml$ Hence, (2) is correct.