Calcium oxalate (cac2o4) has a ksp value of 2.3 × 10–9 at 25°c. calculate the molar solubility of ca2+ and c2o42– in one liter of aqueous solution.
ksp = [x] × [x]
what is the molar solubility of ca2+?
2.3 x 10-9 m
4.8 x 10–5 m
4.60 x 10-9 m
5.29 x 10-18 m

Ksp is the equilibrium constant of solubility of a solid in a solution.

The solid is CaC2O4.

The dissolved ions are Ca2+ and C2O4 2-

The equation of the equilibrium is


Then Ksp = [Ca 2+][C2O4 2-]

Where the [ ] indicates molar concentration

The chemical equation for this equilibrium implies [Ca 2+] = [C2O4 2-]. Name X this quantity

Ksp = x^2 ==> x = square root of Ksp

x = sqrt(2.3 * 10^ -9) = 4.8 * 10^ -5

Which is the second option.

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