Copper (I) chloride, CuCL, has Ksp = 1.9 x 10^ -7.calculate the molar solubility of CuCL in A)pure water, B)0.0200M HCl solution C) 0.200M HCl solution, and d) 0.150M CaCl2 solution.

Question

I used the ice table and for a) i got 0.000435 M

sort of lost for the rest

Answer 1

for the rest, you are starting with a chloride concentration (you have to compute that concentration from the given Molarities).

Then, you can add such CuCl to reach the max allowed by ksp, no more.
if you started with yy Cl concentration, then the dissociation equation is something like this..

Ksp= (x)(x+yy)/(x)

then you compute x, the moles/liter of CuCl that actually dissolved.
Here is an example of the common ion effect: https://www.boundless.com/chemistry/textbooks/boundless-chemistry-textbook/acid-base-equilibria-16/solubility-equilibria-120/effect-of-a-common-ion-on-solubility-492-1528/