Using the solubility of Ca (IO3) 2 that you determined in pure water, calculate the value of Ksp using only concentrations, that is assuming that all activity coefficients are 1.0.

4.6305 * 10^-6 mol^3. L^-3

Explanation:

Firstly, we write the value for the solubility of Ca (IO3) 2 in pure water. This equals 0.0105mol/L.

We proceed to write the dissociation reaction equation for Ca (IO3) 2

Ca (IO3) 2 (s) Ca2 + (aq) + 2IO3 - (aq)

We set up an ICE table to calculate the Ksp. ICE stands for initial, change and equilibrium. Let the concentration of the Ca (IO3) 2 be x. We write the values for the ICE table as follows:

Ca2 + (aq). 2IO3 - (aq)

I. 0. 0.

C. + x. + 2x

E. x. 2x

The solubility product Ksp = [Ca2+][IO3-]^2

Ksp = x * (2x) ^2

Ksp = 4x^3

Recall, the solubility value for Ca (IO3) 2 in pure water is 0.0105mol/L

We substitute this value for x

Ksp = 4 (0.0105) ^2 = 4 * 0.000001157625 = 4.6305 * 10^-6