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Acids & Bases

Acids & Bases. Calculating pH and Naming. Finding the pH of Solutions. Self- ionization of water – the simple dissociation of water H 2 O H + + OH - Concentration of ea. ion in pure water: [H + ] = 1.0 x 10 -7 M + [OH - ] = 1.0 x 10 -7 M

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Acids & Bases

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  1. Acids & Bases Calculating pH and Naming

  2. Finding the pH of Solutions Self- ionization of water – the simple dissociation of water H2O H+ + OH- Concentration of ea. ion in pure water: [H+] = 1.0 x 10-7M + [OH-] = 1.0 x 10-7M Ion-product constant for water (Kw),Where Kw = 1.0 x 10-14 Kw = [H+] [OH-] Acid [H+] > [OH-] Base [H+] < [OH-] Neutral [H+] = [OH-]

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

  4. Example 1. If the [H+]in a solution is 1.0 x 10-5M, is the solution acidic, basic or neutral? 1.0 x 10-5 M What is the concentration of the [OH-]? Use the ion-product constant for water (Kw): Kw = [H+] [OH-] 1.0 x 10-14 = [1.0 x 10-5] [OH-] 1.0 x 10-14 = [OH-] 1.0 x 10-5 1.0 x 10-(14-5) pH 5 = acidic 1.0 x 10-9 OH-

  5. Examples 2. If the pH is 9, what is the concentration of the hydroxide ion? Kw = [H+] [OH-] 1.0 x 10-14 = [1.0 x 10-9] [OH-] 1.0 x 10-5 = [OH-] 14 = pH + pOH 14 = 9 + pOH 5 = pOH 3. If the pOH is 4, what is the concentration of the hydrogen ion? Kw = [H+] [OH-] 1.0 x 10-14 = [H+] [1.0 x 10-4] 1.0 x 10-10 = [H+] 14 = pH + pOH 14 = pH + 4 10 = pH

  6. Example 4. A solution has a pH of 4. Calculate the pOH, [H+] and [OH-]. Is it acidic, basic, or neutral? • pOH = 14.00- 4 = 9 • acidic

  7. Fill in the chart. 1.0 X 10 -8 1.0 X 10 -6 6 2 12 1.0 X 10 -2

  8. Naming Acids • Binary acids • Contains 2 different elements: H and another • Always has “hydro-” prefix • Root of other element’s name • Ending “-ic” • Examples: HI, H2S, HBr

  9. Naming Acids • Ternary Acids - Oxyacids • Contains 3 different elements: H, O, and another • No prefix • Name of polyatomic ion • Ending “–ic” for “-ate” and “–ous” for “-ite” • Examples: HClO4, H3PO4, HNO2

  10. H2SO3 Sulfurous acid HF Hydrofluoric acid H2Se Hydroselenic acid Perchloric acid HClO4 Carbonic acid H2CO3 Hydrobromic acid HBr Practice

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