Silver sulfate dissolves in water according to the reaction: Ag2SO4 (s) ∆ 2 Ag + (aq) + SO42 - (aq) Kc = 1.1 * 10-5 at 298 K A 1.5-L solution contains 6.55 g of dissolved silver sulfate. If addi - tional solid silver sulfate is added to the solution, will it dissolve?

additional solute will not dissolve.

Explanation:

First we must obtain the number of moles of Ag + and SO4^2 - ions present.

Number of moles of the compound = mass / molar mass

Molar mass of compound = (2*108) + 32 + 4 (16) = 216 + 32 + 64 = 312gmol-1

Number of moles of compound = 6.55g/312gmol-1 = 0.021moles

Concentration of Ag + = (2*0.021) / 1.5 = 0.028M

Concentration of SO4^2 - = 0.021/1.5 = 0.014M

Qsp = [Ag+]^2[SO42-] = (0.028) ^2 (0.014) = 1.1 x 10^-5 = Ksp

Since Qsp=Ksp, additional solute will not dissolve.