AgCl --> Ag^+ + Cl^-
Ksp = (Ag^+)(Cl^-) = about1.8E-10
Compare Qsp with Ksp.
In soution (and I'm assuming that adding the salts to 200 mL H2O is the same as producing 200 mL solution).
Ag^+ = 1.7/170 = about 0.01 mols.
You should go through these calculations yourself; I've rounded molar masses and the answers.
Cl^- = 14.5/58.5 = about 0.25 mols.
(Ag^+) = 0.01 mols/0.200L = about 0.05M
(Cl^-) = 0.25 mols/0.200L = about 1.25M
Qsp = (0.05)(1.25) = 0.06 which is larger than Ksp at 1.8E-10 and a ppt should occur.
Does it produce precipitate if 1.7 g of AgNO3 and 14.5 g of NaCl solvated in 200 mL water to get a solution in 25 oC ?
thank you
1 answer
1 answer