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Buffers

Buffers. The Normal pH Range of Some Body Fluids. 1 ml 1.0 M. 1 ml 1.0 M NaOH. 13. 0. 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 14. in 1 liter water. HCl in 1 liter water. ACIDIC. BASIC. Buffer Solutions.

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Buffers

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  1. Buffers

  2. The Normal pH Range of Some Body Fluids

  3. 1 ml 1.0 M 1 ml 1.0 M NaOH 13 0 1 2 3 4 5 6 7 8 9 10 11 12 14 in 1 liter water HCl in 1 liter water ACIDIC BASIC Buffer Solutions Buffer: a solution that is capable of maintaining its pH at a fairly constant value even when small amounts of acids or bases are added

  4. CH3COOH – CH3COONa HCN – KCN H2PO4- – HPO42- NH3 – NH4Cl Acidic Alkaline Buffer Solutions Acidic buffer solution consists of a weak acid and a salt of the acid Alkaline buffer solution sonsists of a weak base and a salt of the base

  5. [H+] = Ka [base] [acid] [salt] [salt] [acid] - log [H+] = - log Ka - log [salt] [base] [OH-] = Kb - log [OH-] = - log Kb - log [salt] [salt] pH = pKa + log [acid] [salt] pOH = pKb + log [base] • pH or pOH of a buffer Henderson-Hasselbach equations

  6. 1 pH = pKa + log = pKa + log 10-1 = pKa-1 10 10 pH = pKa + log = pKa + 1 1 • Buffer range is a range of pH values over which a particular buffer system will function. In general, the ratio of ionic species to molecular species for an effective buffer should be between 1/10and 10/1 • Buffer capacity is amount of acid or base which reduces or increases the pH of 1 liter buffer solution with one pH unit

  7. Acidosis

  8. Alkalosis

  9. The carbonic acid/bicarbonate buffer system

  10. The phosphate buffer system

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