[Kingjim9]

Hi, I was hoping someone could help me with this one question I can't seem to figure out:

Equal volumes of 0.12M AgNO₃ and 0.14M ZnCl₂ solution are mixed.  Calculate the equilibrium concentrations of Ag⁺, Cl^-, Zn²⁺, and NO₃^-

I started it off by calculating the moles of AgNO₃ to be .07 mol (.12M * .5L = .06) Assuming there was half a liter of each to make 1 liter of solution total.
I got moles of ZnCl₂ the same wayand got .07 moles.

Then I set up my reaction:  Ag(NO₃) + ZnCl₂ AgCl₂ + Zn(NO₃)

I tried setting up an I.C.E. table to try to figure out the equilibrium concentrations but i can't seem to get any farther than that point.  That is all the information i'm given about the problem and I don't know any kind of K_sp or anything.

Any Help will be appreciated,

Thanks,

Jim

[Borek]

Try to do it as a limiting reagent question.

In general you should also account for AgCl Ksp, but seems like AgCl can be treated (in the presence of excess of one reactants) as completely insoluble.