Calculate the molar solubility of ca (io3) 2 in each solution below. the ksp of calcium iodate is7.1 * 10-7.

In order to find the answer, use an ICE chart:

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

some ... 0 ... 0

less ... + x ... + 2x

less ... x ... 2x

Ca (IO₃) ₂ ⇄ Ca⁺² + 2 IO⁻³

K sp = [Ca⁺²][IO₃⁻]²

K sp = (x) (2 x) ² = 4 x³

7.1 x 10⁻⁷ = 4 x³

x = molar solubility = 5.6 x 10 ⁻³ M

The answer is 5.6 x 10 ^ 3 M. (molar solubility)

Answer: 5.62 x 10⁻³ M

Explanation:

1) Equilibrium equation:

Ca (IO₃) ₂ ⇄ Ca⁺² + 2 IO⁻³

2) By stoichimetry ratio, the concentrtion of IO⁻³ ions is the double than the concentraion of Ca⁺², so call them x and 2x.

3) Solubility product constant, Ksp:

Ksp = [Ca⁺²] [IO⁻³]² = x (2x) ² = 4x³

=> 4x³ = 7.1 x 10⁻⁷

=> x^3 = 1.775 x 10⁻⁷

=> x = 5.62 x 10⁻³ M