Question

Solubility product $(K_{sp})$ of saturated PbCl$_2$ in water is $1.8 \times 10^{-4}\ \text{mol}^3\text{dm}^{-9}$. What is the concentration of Pb$^{2+}$ in the solution?}

• A. $(0.45 \times 10^{-4})^{1/3}$ mol dm$^{-3}$
• B. $(1.8 \times 10^{-4})^{1/3}$ mol dm$^{-3}$
• C. $(0.9 \times 10^{-4})^{1/3}$ mol dm$^{-3}$
• D. $(2.0 \times 10^{-4})^{1/3}$ mol dm$^{-3}$
• E. $(2.45 \times 10^{-4})^{1/3}$ mol dm$^{-3}$

Hint:

For salt MX$_2$: always remember $K_{sp} = 4s^3$.

Answer 1

The Correct Option is A