To what final concentration of nh3 must a solution be adjusted to just dissolve 0.060mol of nic2o4 (ksp = 4×10−10) in 1.0 l of solution? (hint: you can neglect the hydrolysis of c2o42− because the solution will be quite basic.)

In this problem ,we are given with the solubility constant of nickel dichromate which when dissolved in ammonia results to dichromate ion and nickel ion. In this case, with the given initial concentration 0.06 M, the equation becomes. 4x10^-10 = x^2/ (0.06-x) where c is the final concentration of NH3. x is equal to 4.89 x 10^-6 M.

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