dium acetate (NaC2H3O2) is a basic salt. When sodium acetate is dissolved in water, it dissociates into its component ions. This reaction goes to completion, as indicated by the one-way arrow in the following equation: NaC2H3O2(s) ==========> Na+(aq) + C2H3O2-(aq) The Na+, being the conjugate acid of a strong base (NaOH) is too weak to react with water. However, the C2H3O2-, being the conjugate base of a weak acid (HC2H3O2) is strong enough to react slightly with water. The equation for this equilibrium reaction is C2H3O2-(aq) + H2O(l) <----------> HC2H3O2(aq) + OH-(aq) The equilibrium constant for the above reaction (Kb for C2H3O2-) is normally not published in tables, because it can be calculated from two other values that ARE published: the ionization constants for H2O and HC2H3O2. 2H2O(l) <----------> H3O+(aq) + OH-(aq) Kw = 1.0 x 10-14 HC2H3O2(aq) + H2O(l) <----------> H3O+(aq) + C2H3O2-(aq) Ka = 1.8 x 10-5 By combining these two equations in the appropriate way, it is possible to obtain the desired reaction, and hence, its equilibrium constant. What is the hydronium ion concentration ([H3O+]) in a 4.75 M NaC2H3O2 solution? answers: 3.8 x 10-13 mol/L 4.2 x 10-12 mol/L 1.9 x 10-10 mol/L 5.1 x 10-5 mol/L 2.4 x 10-3 mol/L can some one please explain how to do this step by step? thankyou