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?

1 Answer
anor277
Sep 21, 2016

Formation of insoluble silver chloride would be quantitative. Almost a 1*g1⋅g mass would precipitate.

Explanation:

Ag^+ + Cl^(-) rarr AgCl(s)darrAg++Cl−→AgCl(s)⏐↓

"Moles of silver acetate"Moles of silver acetate == 0.078*mol*L^-1xx75.0xx10^-3L=5.85xx10^-3*mol0.078⋅mol⋅L−1×75.0×10−3L=5.85×10−3⋅mol.

"Moles of magnesium chloride"Moles of magnesium chloride == 0.109*mol*L^-1xx55.0xx10^-3L=6.00xx10^-3*mol0.109⋅mol⋅L−1×55.0×10−3L=6.00×10−3⋅mol.

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

Thus 5.85xx10^-3*mol5.85×10−3⋅mol AgCl(s)AgCl(s) would be formed, i.e. a mass of 5.85xx10^-3*cancel(mol)xx143.32*g*cancel(mol^-1) = ??g

Related questions
See all questions in Double Replacement Reactions
Impact of this question
3289 views around the world
You can reuse this answer
Creative Commons License