Question

Does any solid Ag2CrO4 form when 3.5 10-4 g of AgNO3 is dissolved in 15 mL...

Does any solid Ag2CrO4 form when 3.5 10-4 g of AgNO3 is dissolved in 15 mL of 6.8 10-5 M K2CrO4? Assume no volume change

a) Qsp

b) Ksp

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Answer #1

Molar Mass of AgNO3 is 169.87 g/mol.

Number of moles of AgNO3 present in 3.5 * 10-4 g of AgNO3 is {(3.5 * 10-4) / 169.87} mol = 2.06 * 10-6 mol.

Volume of the solution is 0.015 L.

So, molarity of AgNO3 as well as Ag+ in the solution is (2.06 * 10-6 mol / 0.015 L) = 1.37 *10-4 (M)

Molarity of the K2CrO4 solution is 6.8 * 10-5 (M).

So, molarity of CrO42- in the solution is 6.8 *10-5 (M)

The Ionic Product (Qsp) is [Ag+]2 * [CrO42-] = {(1.37 *10-4)2 * (6.8 * 10-5)} = 1.27 * 10-12

The Solubility Product (Ksp) of Ag2CrO4 is 1.1 * 10-12

As, the Qsp exceeds Ksp there will be precipitation of Ag2CrO4.

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