What are [Ba2+] and [CrO42-] in a saturated BaCrO4 solution if the Ksp of BaCrO4 is 1*10-10?

[Ba2+] =

[CrO42-] =

1) Chemical equation of the equilibrium

BaCrO4⇄ Ba (2+) + CrO4 (2-)

2) Ksp equation

Ksp = [Ba (2+) ] [CrO4 (2-) ]

where Ksp = 1.0 * 10^ - 10 and [Ba (2+) ] = [CrO4 (2-) ] = x

3) Calculations

1.0 * 10^ - 10 = x * x

=> x^2 = 1.10 * 10^-10

=> x = √[1.0 * 10^ - 10] = 0.000010

Answer: [Ba (2+) ] = [CrO4 (2-) ] = 0.00001 M