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?

Question

2826 views around the world

You can reuse this answer
Creative Commons License

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*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?