chemistry - Equilibrium

Question

CaCO3 calcium carbonate only partially dissolves in an aqueous medium according to the reaction:

(= is supposed to be arrows that go both ways since I can not type that on my laptop)

CaCO3(solid) = Ca^2(aq)+CO3^2-(aq)

Assuming that the initial amount of CaCO3 was 1.0 mole in a 1.0-liter solution and that at equilibrium x moles of CaCO3 have dissolved, which of the following statements is correct?

A. The equilibrium constant of this reaction is X^2/(1-x).

B. The efficiency of this reaction is equal to X^2.

C. The degree of dissociation of this reaction is equal to X/2.

D. The equilibrium constant of this reaction is X^2.

Please help me solve this step by step with an explanation in detail.

Thank you so much

Answer 1

CaCO3(s) <==> Ca2+(aq) + CO32-(aq)

Write the Ksp expression (equilibrium expression/equilibrium constant):

Ksp = [Ca²⁺][CO₃^2-]

Ksp = (x)(x)

Ksp = x²