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

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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