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