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.

Considering the solubility of Ca(IO₃)₂ and assuming that all activity coefficients are 1.0, the solubility product is 4.63 × 10⁻⁶.

Let's consider the equation for the solution of Ca(IO₃)₂.

Ca(IO₃)₂(s) ⇄ Ca²⁺(aq) + 2 IO₃⁻(aq)

We want to calculate the solubility product (Ksp).

The solubility product constant is a simplified equilibrium constant denoted as Ksp which is defined for equilibrium between a solid and its respective ions in a given solution.

The molar solubility (S) of Ca(IO₃)₂ is 0.0105 mol/L. To relate this value with the solubility product, we need to make an ICE chart.

It is a chart with 3 rows:

We complete each row with the concentration or change in the concentration for each step. Let's remember that we will neglect solids as they are not present in the equilibrium constant.

The ICE chart for the solution of Ca(IO₃)₂ is:

         Ca(IO₃)₂(s) ⇄ Ca²⁺(aq) + 2 IO₃⁻(aq)

I                                 0                   0

C                               +S               +2S

E                                 S                 2S

The solubility product for the solution of Ca(IO₃)₂ is:

Ksp = [Ca²⁺][IO₃⁻]² = S × (2S)² = 4 S³ = 4 (0.0105)³ = 4.63 × 10⁻⁶

Considering the solubility of Ca(IO₃)₂ and assuming that all activity coefficients are 1.0, the solubility product is 4.63 × 10⁻⁶.

Learn more about solubility product here: link

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

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