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In the Laboratory

pH. In the Laboratory. Ionization of Water. Equllibrium Constant, K eq. Ion Product of Water, K W. pH. Acidity. Measuring pH. Indicater Dyes; Methyl Red, Phenol Red, etc. pH Paper (Litmus Paper) pH Meter. pH Meter. Voltmeter with electrode

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In the Laboratory

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  1. pH In the Laboratory

  2. Ionization of Water

  3. Equllibrium Constant, Keq

  4. Ion Product of Water, KW

  5. pH

  6. Acidity

  7. Measuring pH • Indicater Dyes; Methyl Red, Phenol Red, etc. • pH Paper (Litmus Paper) • pH Meter

  8. pH Meter • Voltmeter with electrode • Measures electrical potential difference across electrode due to protons • 1 pH unit = 60 mV • pH also dependent on temperature

  9. pH Electrode • Filled with reference solution (4 M KCl, sat. AgCl) • Glass semi permable (protons cannot cross) • Glass protected by plastic sleeve • Some are sensitive to Tris buffer

  10. pH Standards • Color coded 4, 7, and 10 • Potassium Hydrogen Pthalate • Standardize everyday • Bracket pH range

  11. pH of Strong Acids • HCl <-> H+ +Cl- • Assume complete dissociation • 1 M HCl, pH = -log [H+] = -log 1 = ? • 0.5 M HCl, pH = -log 0.5 = ? • 6 M HCl, pH = -log 6 = ?

  12. pH of Strong Bases • NaOH <-> Na+ + OH- • Assume complete dissociation • pKW = pH + pOH = 14 • pH = 14 – (-log [OH-]) • 1 M NaOH, pH = 14 – (-log 1) = ? • 0.01 M NaOH, pH = 14 – (-log 0.01) = ? • 6 M NaOH, pH = 14 – (-log 6) = ?

  13. pH of a Weak Acid

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