Question
The solubility product of CU(IO3)2 is 1.08×10^-3 assuming that neither ions react appreciably with water to form H+ and OH- . What is the solubility of this salt?
Answers
GPT 3.5
To find the solubility of CU(IO3)2, we need to first write out the equilibrium expression for the dissolution of the salt:
CU(IO3)2 (s) ⇌ Cu^2+ (aq) + 2IO3- (aq)
The solubility product constant (Ksp) for this equilibrium is given as 1.08×10^-3.
Let x be the solubility of CU(IO3)2 in mol/L. Then the equilibrium concentrations are [Cu^2+] = x and [IO3-] = 2x.
Substitute these values into the Ksp expression:
Ksp = [Cu^2+][IO3-]^2
1.08×10^-3 = x(2x)^2
1.08×10^-3 = 4x^3
Solve for x:
x = (1.08×10^-3 / 4)^(1/3)
x ≈ 0.158 mol/L
Therefore, the solubility of CU(IO3)2 is approximately 0.158 mol/L.
CU(IO3)2 (s) ⇌ Cu^2+ (aq) + 2IO3- (aq)
The solubility product constant (Ksp) for this equilibrium is given as 1.08×10^-3.
Let x be the solubility of CU(IO3)2 in mol/L. Then the equilibrium concentrations are [Cu^2+] = x and [IO3-] = 2x.
Substitute these values into the Ksp expression:
Ksp = [Cu^2+][IO3-]^2
1.08×10^-3 = x(2x)^2
1.08×10^-3 = 4x^3
Solve for x:
x = (1.08×10^-3 / 4)^(1/3)
x ≈ 0.158 mol/L
Therefore, the solubility of CU(IO3)2 is approximately 0.158 mol/L.