Ch. 15 & 16 - Acids & Bases II. pH (p. 481 - 491) C. Johannesson.

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Ch. 15 & 16 - Acids & Bases II. pH (p. 481 - 491) C. Johannesson

H2O + H2O H3O+ + OH- Kw = [H3O+][OH-] = 1.0  10-14 A. Ionization of Water H2O + H2O H3O+ + OH- Kw = [H3O+][OH-] = 1.0  10-14 C. Johannesson

A. Ionization of Water Find the hydroxide ion concentration of 3.0  10-2 M HCl. [H3O+][OH-] = 1.0  10-14 [3.0  10-2][OH-] = 1.0  10-14 [OH-] = 3.3  10-13 M Acidic or basic? Acidic C. Johannesson

pouvoir hydrogène (Fr.) B. pH Scale 14 7 INCREASING ACIDITY INCREASING BASICITY NEUTRAL pH = -log[H3O+] pouvoir hydrogène (Fr.) “hydrogen power” C. Johannesson

pH of Common Substances B. pH Scale pH of Common Substances C. Johannesson

pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14 B. pH Scale pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14 C. Johannesson

B. pH Scale What is the pH of 0.050 M HNO3? pH = -log[H3O+] Acidic or basic? Acidic C. Johannesson

B. pH Scale What is the molarity of HBr in a solution that has a pOH of 9.6? pH + pOH = 14 pH + 9.6 = 14 pH = 4.4 pH = -log[H3O+] 4.4 = -log[H3O+] -4.4 = log[H3O+] [H3O+] = 4.0  10-5 M HBr Acidic C. Johannesson