I am not sure if I have done this correctly. Any hints would be helpful.
Question: A 100.0mL solution of 1.00mol/L aqueous sodium sulfate, is added to a 200.0mL solution of 1.00mol/L aqueous barium chlordie. Barium sulfate precipitates from the mixture .Ksp of barium sulfate is 1.1x10^-10. Calculate the mass of the precipitate of barium sulfate.
I have calculated the Q/trial ion product and used that to find the mass.
Thanks for any help/hints.
First I set up initial conc of barium ions to be 1.0M and sulfate is 1.0M
Then the final concentrations are barium = (1.0)(200/300) =0.67M
sulfate = (1.0)(100/300) =0.33M
trial ion product = [Ba][SO4] n = cv = (0.2211M)(0.3L) = 0.06633 mol
=0.67 x 0.33 MM = 233.40 for barium sulfate
= 0.2211 M
m = n (MM) = 15.5 g