Chapter 15

Chapter 15 - Chapter 15 - Buffers [8M] 2/29/2008, 10:11 AM...

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Chapter 15 - Buffers common ion : an ion that comes from more than one source in solution common ion effect : the equilibrium shift caused by the presence of a common ion ex) In 0.15M NH3, the pH is 11.21 and the percent dissociation is 1.1%. Calculate the concentration of all species present, the pH, and the percent dissociation of ammonnia in a solution that is 0.15M NH3, and 0.45M NH4Cl. Common Ion [8M] 2/29/2008, 10:11 AM Chapter 15 Page 1
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resists changes to its pH contains a weak acid and its conjugate base or a weak base and its conjugate acid Buffered Solution : if we add H+ it will shift to the left, taking up A- ions ad making more HA molecules. If we add OH-, it will shift ot the right, taking up H+ ions and need to lose HA molecules to make up for the difference. ex) Calculate concentrations of all species present, the pH, and the percent dissociation of HCN (Ka=4.9x10-10) in a solution of 0.025M HCN and 0.010M NaCN. ex) Calculate the pH change that occurs when 0.010 mol HCl is added to 1.0L of the buffered solution described on the previous slide. Compare this pH change with that which occurs when 0.010 mol HCl is added to 1.0L of water. Chapter 15 Page 2
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Chapter 15 - Chapter 15 - Buffers [8M] 2/29/2008, 10:11 AM...

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