consider the reaction Ag2O(s) H2O  2Ag 2OH-Ksp = 3.8 x 10-16 a. If Ag2O forms to an appreciable extent what effect will this equilibrium have on the solubility of AgCN? Explain your reasoning. Judging by the equilibrium reaction shown, would you expect the effect of this equilibrium on the solubility of AgCN to be pH dependent? b. Pick the solution from Table 1 where your reasoning suggests that the precipitation of Ag2 O will be most significant. You can easily figure out [OH–O will actually occur. ] from the pH and [Ag ] that is given you, so calculate the ion product suggested by the reaction above and determine whether or not precipitation of Ag2O will actually occur