The solubility of zinc oxalate is 7.9 x 10 ^-3 M at 18 degrees C. Calculate its Ksp.
To calculate the solubility product constant (Ksp) for zinc oxalate (ZnC2O4), we need to use the formula:
Ksp = [Zn2+][C2O4 2-]
Given that the solubility of zinc oxalate is 7.9 x 10 ^-3 M, we can assume that the concentration of both the zinc ion (Zn2+) and oxalate ion (C2O4 2-) is equal to this value.
So, [Zn2+] = [C2O4 2-] = 7.9 x 10 ^-3 M
Now, substitute these values into the Ksp formula:
Ksp = (7.9 x 10 ^-3)^2
Ksp = 6.24 x 10 ^-5
Therefore, the solubility product constant (Ksp) for zinc oxalate is 6.24 x 10 ^-5.
To calculate the solubility product constant (Ksp) of zinc oxalate, we need the equation that represents the dissociation of the compound in water.
The formula for zinc oxalate is ZnC2O4, and when it dissolves in water, it dissociates into its constituent ions:
ZnC2O4 (s) ⇌ Zn2+ (aq) + 2C2O4^2- (aq)
The solubility of zinc oxalate, given as 7.9 x 10^-3 M, corresponds to the concentration of Zn2+ ions in the solution since there are two oxalate ions for every zinc ion.
Now, we can set up the expression for the solubility product constant (Ksp):
Ksp = [Zn2+] * [C2O4^2-]^2
Since the coefficient of Zn2+ is 1, the concentration of Zn2+ is also 7.9 x 10^-3 M.
Substituting this value into the equation, we get:
Ksp = (7.9 x 10^-3) * (2 * 7.9 x 10^-3)^2
= (7.9 x 10^-3) * (1.6 x 10^-2)^2
= 2.53 x 10^-6
Therefore, the solubility product constant (Ksp) of zinc oxalate is 2.53 x 10^-6.
ZnC2O4 ==> Zn^+ + SO4^-2
Ksp + (Zn^+2)(SO4^-2)
Substitute the molar solubility into the Ksp expression and solve.