Question

What is the solubility in moles/liter for chromium(III) iodate at 25 oC given a Ksp value of 5.0 x 10-6. Write using scientific notation and use 1 or 2 decimal places (even though this is strictly incorrect!)

Answer 1

Answer: The solubility of chromium (III) iodate is $2.07\times 10^{-2}M$

Explanation:

Solubility product is defined as the product of concentration of ions present in a solution each raised to the power its stoichiometric ratio.

The chemical equation for the ionization of chromium (III) iodate follows:

$Cr(IO_3)_3(aq.)\rightleftharpoons Cr^{3+}(aq.)+3IO_3^-(aq.)$  

                                s                3s

The expression of $K_{sp}$ for above equation follows:

$K_{sp}=s\times (3s)^3$

We are given:  

$K_{sp}=5.0\times 10^{-6}$

Putting values in above expression, we get:

$5.0\times 10^{-6}=s\times (3s)^3\\\\s=2.07\times 10^{-2}M$

Hence, the solubility of chromium (III) iodate is $2.07\times 10^{-2}M$