Calculate the ionization constant for each of the following acids or bases from the ionization constant of its conjugate base or conjugate acid:
(a) F-
(b) NH4 +
(c) AsO4 3-
(d) (CH3)2NH2+
(e) NO2-
(f) HC2 O4 - (as a base)
Determine whether aqueous solutions of the following salts are acidic, basic, or neutral:
(a) Al(NO3)3
(b) RbI
(c) KHCO2
(d) CH3NH3Br
What is [H3O+] in a solution of 0.075 M HNO2 and 0.030 M NaNO2? HNO2(aq) + H2 O(l) ? H3 O+(aq) + NO2 -(aq)Ka = 4.5 × 10-5
Calculate the pH of a buffer solution prepared from 0.155 mol of phosphoric acid, 0.250 mole of KH2PO4, and enough water to make 0.500 L of solution
Draw a curve similar to that shown in Figure 14.23 for a series of solutions of NH3. Plot [OH-] on the
vertical axis and the total concentration of NH3 (both ionized and nonionized NH3 molecules) on the horizontal axis. Let the total concentration of NH3 vary from 1 × 10-10 M to 1 × 10-2 M.