What is the solubility in moles/liter for chromium(III) iodate at 25 oC given a Ksp value of 5.0 x 10-6.

Question

What is the solubility in moles/liter for chromium(III) iodate at 25 ^oC given a K_sp value of 5.0 x 10^-6. 

the answer is:

2.07 x 10^-2

Please show your steps so I can follow along. Thank you!

Answer 1

Chromium(III) Iodate = Cr(IO₃)₃

Cr(IO₃)₃(s) ===> Cr³⁺(aq) + 3IO³(aq) ... this is the dissolution of the compound

Ksp = [Cr³⁺][IO₃^-]³ ... the is the Ksp epxression

If we let [Cr³⁺] = x, then the [IO₃^-] = 3x and since we are given the Ksp value, we can solve for x.

5.0x10^-6 = (x)(3x)³

5.0x10^-6 = 27x⁴

x⁴ = 1.85x10^-7

x = 2.07x10^-2 M = molar solubility