Question

The solubility of $S{b}_2{S}_3$ in water is $1.0\times {10}^{-5}$ mol/litre at $298K$. What will be its solubility product?

• A. $108\times {10}^{-25}$
• B. $1.0\times {10}^{-25}$
• C. $144\times {10}^{-25}$
• D. $126\times {10}^{-24}$

Answer 1

Answer: (A)

$108\times {10}^{-25}$

$S{b}_2{S}_3\to \underset{2x}{{2Sb}^{+3}}+\underset{3x}{{3S}^{--}};K_{sp}=(2x{)}^2.(3x{)}^3$

$K_{sp}=108x^5;K_{sp}=108\times (1\times {10}^{-5}{)}^5=108\times {10}^{-25}$