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Chemistry Chapter 16

Chemistry Chapter 16. Acid-Base Titration and pH. Self-Ionization of Water. H 2 O + H 2 O  H 3 O + + OH -. Ion Concentration in Water. K w – Ionization Constant for Water. In pure water at 25 C:. [H 3 O + ] = 1 x 10 -7 mol/L. [OH - ] = 1 x 10 -7 mol/L.

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Chemistry Chapter 16

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  1. Chemistry Chapter 16 Acid-Base Titration and pH

  2. Self-Ionization of Water H2O + H2O  H3O+ + OH-

  3. Ion Concentration in Water

  4. Kw – Ionization Constant for Water In pure water at 25 C: [H3O+] = 1 x 10-7 mol/L [OH-] = 1 x 10-7 mol/L Kw is a constant at 25 C: Kw = [H3O+][OH-] Kw = (1 x 10-7)(1 x 10-7) = 1 x 10-14

  5. H+, OH-, and pH

  6. pH Scale

  7. Calculating pH, pOH pH = -log10(H3O+) pOH = -log10(OH-) Relationship between pH and pOH pH + pOH = 14 Finding [H3O+], [OH-] from pH, pOH [H3O+] = 10-pH [OH-] = 10-pOH

  8. pH + pOH = 14

  9. Measuring pH with wide-range paper

  10. Narrow-Range pH Paper

  11. pH Indicators and theirranges

  12. Titration Calculations

  13. Titration Curves

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