Question

Calculate the molar solubility of zinc carbonate in

ZnCO3(s) Zn2+(aq) + CO32-(aq) Kps=3.10-8
Water: solubility = [ ] mol.L-1
• Zn (NO3) 2 solution 0.0500 mol.L-1: solubility = [ ] mol.L-1
• K2CO3 solution 0.0500 mol.L-1; solubility = [ ] mol.L-1

Answer 1

The molar solubility of zinc carbonate in water is 5.6 × 10-5 mol.L-1.

Step-by-step explanation:

The molar solubility of zinc carbonate in water can be calculated using the solubility product constant (Ksp) and the stoichiometry of the reaction. The balanced equation for the dissociation of zinc carbonate is:

ZnCO3(s) → Zn2+(aq) + CO32-(aq)

Since the Ksp value is given as 3.10-8, we can set up the equation:

[Zn2+][CO32-] = 3.10-8

Since the concentration of Zn2+ and CO32- are equal at equilibrium, we can substitute x for both concentrations:

x² = 3.10-8

Solving for x gives the molar solubility of zinc carbonate as:

x = √(3.10-8) = 5.6 × 10-5 mol.L-1

Therefore, the molar solubility of zinc carbonate in water is 5.6 × 10-5 mol.L-1.