The 𝐾sp of copper(II) carbonate, CuCO3, is 1.4×10−10 . Calculate the molar solubility, 𝑆 , of this compound.

Question

How do I solve this question?

Answer 1

You solve this by setting up the expression for Ksp and then solving for s.

CuCO₃(s) <==> Cu²⁺(aq) + CO₃^2-(aq)

Ksp = [Cu²⁺][CO₃^2-]

Let s = solubility of Cu²⁺ = solubility of CO₃^2-

1.4x10^-10 = (s)(s) = s²

s = sqrt 1.4x10^-10

s = 1.18x10^-5 M