Chemistry, 03.08.2020 14:01 zacharoo10
For the following equilibrium, Ag3PO4(s)↽−−⇀3Ag+(aq)+PO3−4(aq) If Ksp=2.4×10−28, what is the molar solubility of Ag3PO4? Report your answer in scientific notation with the correct number of significant figures.
Answers: 1
![K_{sp} =\text{[Ag$^{+}$]$^{3}$[PO$_{4}^{3-}$]} = (3x)^{3}x = 2.4 \times 10^{-28}\\27x^{4} = 2.4 \times 10^{-28}\\x^{4} = 8.89 \times 10^{-30}\\x = \sqrt[4]{8.89 \times 10^{-30}}\\= \mathbf{5.5\times 10^{-8}} \textbf{ mol/L}\\\text{The molar solubility of silver phosphate is $\large \boxed{\mathbf{5.5\times 10^{-8}}\textbf{ mol/L }}$}](/tpl/images/0716/8807/790d1.png)
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For the following equilibrium, Ag3PO4(s)↽−−⇀3Ag+(aq)+PO3−4(aq) If Ksp=2.4×10−28, what is the molar s...
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