What would occur when a 75*mL volume of silver acetate at 0.078*mol*L^-1 concentration was mixed with 55*mL of magnesium chloride at 0.109*mol*L^-1 concentration. What precipitate, and what mass, would result?

Sep 21, 2016

Formation of insoluble silver chloride would be quantitative. Almost a $1 \cdot g$ mass would precipitate.

Explanation:

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

$\text{Moles of silver acetate}$ $=$ $0.078 \cdot m o l \cdot {L}^{-} 1 \times 75.0 \times {10}^{-} 3 L = 5.85 \times {10}^{-} 3 \cdot m o l$.

$\text{Moles of magnesium chloride}$ $=$ $0.109 \cdot m o l \cdot {L}^{-} 1 \times 55.0 \times {10}^{-} 3 L = 6.00 \times {10}^{-} 3 \cdot m o l$.

$\text{Silver acetate}$ is thus the limiting reagent, as there is stoichiometric chloride ion.

Thus $5.85 \times {10}^{-} 3 \cdot m o l$ $A g C l \left(s\right)$ would be formed, i.e. a mass of $5.85 \times {10}^{-} 3 \cdot \cancel{m o l} \times 143.32 \cdot g \cdot \cancel{m o {l}^{-} 1}$ $=$ ??g