First slide

Solubility product(KSP)

Question

Calculate the solubility of silver phosphate (Ag₃PO₄) in 0.1M AgNO₃ (k_SP Ag₃PO₄= 1.1 X 10^-16)

Easy

A

1 x 10^-8M
B

1 x 10^-15M
C

1.1 x 10^-15M
D

1.1 x 10^-13M

Solution

$\begin{aligned} {Ag}_{3} {PO}_{4} ⇌ \underset{(3 s + 0.1)}{{Ag}^{+}} + {PO}_{4}^{- 3} \end{aligned}$
$\begin{array}{r} Ksp = (3 s + 0.1)^{3} (s) = 1.1 \times 10^{- 16} \end{array}$
$\begin{array}{l} 10^{- 3} \times s = 1.1 \times 10^{- 16} \\ s = 1.1 \times 10^{- 13} \end{array}$

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