chemistry
posted by Anonymous on .
When 10.0 mL of 0.012 M Pb(No3)2 is mixed with 10.0 mL of 0.030M KI, a yellow precipitate of PbI2(s) forms.
a. Calculate the molarity of [Pb2+]
b. calculate the initial molarity of [I]
c. On measuring the equilibrium concentration of [I] it cam out to be 8.0 x 10^3 M. Calculate the molarity of [I] precipitated.
d. Calculate the concentration of [Pb2+] precipitated.
e. calculate the equilibrium concentration of [Pb2+]
f. Calculate the Ksp of PbI2.

Where do you seem to be having problems? The problem lays it out in order for you to solve.

i need help with all of it to solve it step by step