The solubility product constant, Ksp, for nickel (II) carbonate, NiCO3, is 1.3 x 10-7 at 25C.

Question

a. Write the balanced chemical equation for this dissolving process

b. Write the equilibrium expression

c. Find the maximum molar concentration of all ions in solution

Please help!

Answer 1

, Ksp, for nickel (II) carbonate, NiCO3, is 1.3 x 10-7 at 25C.
a. Write the balanced chemical equation for this dissolving process
b. Write the equilibrium expression
c. Find the maximum molar concentration of all ions in solution
...............NiCO3(s) + H2O ==> Ni^2+(aq) + [CO3]^2-(aq)
I...................solid..........(l)............0....................0
C..................solid(-x)....(l).............x....................x
E...................solid..........(l).............x....................x
Ksp = (Ni^2+)[CO3]^2- = 1.3E-7. Substitute from the E line into Ksp expression.
1.3E-7 = (x)(x) = x^2
x = sqrt(1.3E-7) = ? M
So (Ni^2+) = x = [CO3]^2- = approx 3.6E-4 M
NOTE: I don't know exactly how your prof writes these equations or expressions so you may need to adjust what I wrote to match how your class usually does it. For example I don't usually write H2O in the dissolution process. Also, I show -x for the solid change but solid-x still is a solid.

Answer 2

thank you so much!