You mix 1.00 L of 2.00 M BaCl2 with 1.00 L of 2.00 M AgNO3. What compounds remain in solution, and what are their concentrations?
2 answers
Both compounds are soluble, thus you have a double replacement reaction. Do stochiometry with the balanced reaction to find the concentrations.
mols BaCl2 = 1 L x 2M = 2 mols.
mols AgNO3 = 1 L x 2M = 2 mols.
......BaCl2 + 2AgNO3 ==>2AgCl + Ba(NO3)2
initial.2......2.........0.......0
change.-1.....-2.........2.......1
equil...1......0.........2.......1
AgCl is a solid. You should be able to take it from here.
mols AgNO3 = 1 L x 2M = 2 mols.
......BaCl2 + 2AgNO3 ==>2AgCl + Ba(NO3)2
initial.2......2.........0.......0
change.-1.....-2.........2.......1
equil...1......0.........2.......1
AgCl is a solid. You should be able to take it from here.