Calculate the K for each reaction. H_2 AsO_4^- (aq) + OH^- (aq) doubleheadarow HAsO_4^2- (aq) + H_2O(l) CH_3 NH_2 (aq) + H_3O^-(aq) doubleheadarow CH_3NH_3^+ (aq) + H_2O(l) Consider the reaction: HA(aq) + H_2O(l) doubleheadarrow H_3O^+ (aq) + A^- (aq) A 0.10 M solution of the weak acid, HA, is in equilibrium as shown above. What will happen to [A^-] and [H_3O^+] if the system is changed in the indicated manner? solid NaA is added HA is added solid sodium hydroxide is added HCl is added Calculate the concentrations of all species in 0.085 M [H_3PO_4], [H_2 PO_4^-], [HPO_4^2-], [PO_4^2-], [H_3O^+], [OH^-] Calculate the K_a for an unknown acid HX, given that a 0.25 M salt solution NaX has a pH of 8.48. A solution is mixed to initially contain both 0.050 M HCl and 0.250 M acetic acid. Calculate the pH and the concentration of acetate ions in the resulting solution. Abbreviated solutions: reactants products 6.3 Times 10^4 2.0 Times 10^-6 [NO_2] = [O_2] = 2.4 Times 10^-17