Question

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?

Answer 1

Answer:

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.