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II. pH

Ch. 19 Acids & Bases. II. pH. H 2 O + H 2 O H 3 O + + OH -. A. Ionization of Water. K w = [H 3 O + ][OH - ] = 1.0  10 -14. A. Ionization of Water. Find the hydroxide ion concentration of 3.0  10 -2 M HCl. [H 3 O + ][OH - ] = 1.0  10 -14

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II. pH

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  1. Ch. 19 Acids & Bases II. pH

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

  3. 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

  4. pouvoir hydrogène (Fr.) “hydrogen power” B. pH Scale 14 0 7 INCREASING BASICITY INCREASING ACIDITY NEUTRAL pH = -log[H3O+]

  5. B. pH Scale pH of Common Substances

  6. B. pH Scale - Formulas pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14

  7. B. pH Scale • What is the pH of 0.050 M HNO3? pH = -log[H3O+] pH = -log[0.050] pH = 1.3 Acidic or basic? Acidic

  8. 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

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