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Acids & Bases

Acids & Bases. pH. H 2 O + H 2 O H 3 O + + OH -. Ionization of Water. K w = [H 3 O + ][OH - ] = 1.0  10 -14. Kw=ionization constant for H2O. Acidic or Basic. [H 3 O + ][OH - ] = 1.0  10 -14 ACIDIC [H+] is greater than [OH-] [H+] is greater than 1.0  10 -7 BASIC

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Acids & Bases

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  1. Acids & Bases pH

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

  3. Acidic or Basic [H3O+][OH-] = 1.0  10 -14 • ACIDIC • [H+] is greater than [OH-] • [H+] is greater than 1.0  10 -7 • BASIC • [OH-] is greater than [H+] • [H+] is less than 1.0  10 -7

  4. 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 ([H+] > 1 EE -7)

  5. Problem • Colas are slightly acidic. If the [H+] in a solution is 1.0 x 10 -5 M, is the solution acidic basic or neutral? What is the [OH-] of this solution? Answer 1: Because 1.0 x 10-5 M is greater than 1.0 x 10-7 M, the solution is acidic Known: [H+] = 1.0 x 10-5 M Kw = [H+] x [OH-] = 1 x 10-14 Answer 2: [OH-] = 1 x 10 -14 1.0 x 10 -5 = 1.0 x 10 -9 M

  6. pH Scale 14 0 7 INCREASING BASICITY INCREASING ACIDITY NEUTRAL pH = -log [H+]

  7. pH Scale pH of Common Substances

  8. pH Scale pH = -log [H+] pOH = -log [OH-] pH + pOH = 14 [ ] = concentration

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

  10. pH Scale • What is the molarity (conc) of HBr in a solution that has a pOH of 9.6? pH = -log[H+] 4.4 = -log[H+] - 4.4 = log[H+] - 4.4 (10x key)= [H+] [H+] = 4.0  10-5 M HBr pH + pOH = 14 pH + 9.6 = 14 pH = 4.4 Acidic

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