# Jack mixes 82 mL of 4.0x10^-4 M silver acetate with 18 mL of 1.0x10^-4 M Sodium Chloride. Write the overall reaction. Write the net ionic equation. Will precipitate form if Ksp AgCl is 1.6x10^-10?

Jun 18, 2016

$A {g}^{+} + C {l}^{-} \rightarrow A g C l \left(s\right) \downarrow$

#### Explanation:

${K}_{s p} = 1.6 \times {10}^{-} 11$.

A precipitate WILL form if $\left[A {g}^{+}\right] \left[C {l}^{-}\right] > {K}_{s p}$.

$\left[A {g}^{+}\right] = \frac{4.0 \times {10}^{-} 4 \cdot m o l \cdot {L}^{-} 1 \times 0.082 \cdot L}{0.082 \cdot L + 0.018 \cdot L} = 3.28 \times {10}^{-} 3 \cdot m o l \cdot {L}^{-} 1$

$\left[C {l}^{-}\right] = \frac{1.0 \times {10}^{-} 4 \cdot m o l \cdot {L}^{-} 1 \times 0.018 \cdot L}{0.082 \cdot L + 0.018 \cdot L} = 1.8 \times {10}^{-} 6 \cdot m o l \cdot {L}^{-} 1$

Note that I have added the volumes together, but we still have units of $m o l \cdot {L}^{-} 1$ in each case; i.e. a concentration.

So the ion product $Q$ $=$ $1.8 \times {10}^{-} 6 \times 3.28 \times {10}^{-} 3$

If $\text{calculated ion product} > {K}_{s p}$ precipitatiion will occur.