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

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FREE Expert Solution

We are asked if additional solid silver sulfate is added to the solution will dissolve if it already has  6.55 g in 1.5-L solution. 


Calculate molarity of solution: 

Molar mass Ag2SO4 = 311.79 g/mol

Molarity = moles soluteL solutionMolarity = 6.55 g×1 mol311.79 g1.5 L

Molarity = 0.014 M


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Problem Details

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

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Based on our data, we think this problem is relevant for Professor Houston's class at CSUS.