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

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Answer 1 · 2016-09-21T15:16:43

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

$Ag^+ + Cl^(-) rarr AgCl(s)darr$

$"Moles of silver acetate"$ $=$ $0.078*mol*L^-1xx75.0xx10^-3L=5.85xx10^-3*mol$ .

$"Moles of magnesium chloride"$ $=$ $0.109*mol*L^-1xx55.0xx10^-3L=6.00xx10^-3*mol$ .

$"Silver acetate"$ is thus the limiting reagent, as there is stoichiometric chloride ion.

Thus $5.85xx10^-3*mol$ $AgCl(s)$ would be formed, i.e. a mass of $5.85xx10^-3*cancel(mol)xx143.32*g*cancel(mol^-1)$ $=$ $??g$

What would occur when a 75*mL75*mL volume of silver acetate at 0.078*mol*L^-10.078*mol*L^-1 concentration was mixed with 55*mL55*mL of magnesium chloride at 0.109*mol*L^-10.109*mol*L^-1 concentration. What precipitate, and what mass, would result?