Question

The solubility of MX2–type electrolytes is 0.5 × 10–4 Mole/lit. then find out the Ksp of electrolytes :

• A. 5 × 10–12
• B. 25 × 10–10
• C. 1 × 10–13
• D. 5 × 10–13

Answer 1

Answer: (D)

5 × 10–13

Answer 2

The correct option is (D) : 5 × 10–13

An electrolyte MX2 undergoes dissociation as follows :

MX2$\rightleftharpoons$M+2+2X− Concentration MX2 M+2 X− Initial concentration 1 0 0 Concentration at Equilibrium 1-s s 2s Thus from the above condition we can say that, Ksp=s×(2s)2=4×(s)3 Here, s (the solubility ) is 0.5×10−4mole/lit. ∴ Ksp =4×(0.5×10−4)3 ∴ Ksp=5×10−13