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 Ag_{2}SO_{4} = 311.79 g/mol

$\overline{){\mathbf{Molarity}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\frac{\mathbf{moles}\mathbf{}\mathbf{solute}}{\mathbf{L}\mathbf{}\mathbf{solution}}}\phantom{\rule{0ex}{0ex}}\mathbf{Molarity}\mathbf{}\mathbf{=}\mathbf{}\frac{\mathbf{6}\mathbf{.}\mathbf{55}\mathbf{}\overline{)\mathbf{g}}\mathbf{\times}{\displaystyle \frac{\mathbf{1}\mathbf{}\mathbf{mol}}{\mathbf{311}\mathbf{.}\mathbf{79}\mathbf{}\overline{)\mathbf{g}}}}}{\mathbf{1}\mathbf{.}\mathbf{5}\mathbf{}\mathbf{L}}$

**Molarity = 0.014 M**

Silver sulfate dissolves in water according to the following reaction: Ag_{2}SO_{4}(s) ⇌ 2 Ag^{+}(aq) + SO_{4}^{2–}(aq), K_{c} = 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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