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# What is the molar solubility of barium phosphate. The Ksp of Ba3(PO4)2 is: 3.40*10^-23.?

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- busterwasmycatLv 73 weeks ago
Take X as the molarity that you seek ("molar solubility" is presumably in units of molarity). When ionized, you would have 3X of Ba(2+) and 2X of PO4(-3) in solution, so Ksp=(3X)^3*(2X)^2=27*4*X^5. Solve for X. fifth root of 10^-25, or something on the order of 10^-5 M, I would think.

- Anonymous3 weeks ago
Write the equation

Develop the ICE table

Substitute and solve.

I think it's 7.1 * 10^-6

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