mar1308 - percent ionization = Ionized acid concentration...

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percent ionization = Ionized acid concentration at equilibrium Initial concentration of acid x 100% For a monoprotic acid HA Percent ionization = [H + ] [HA] 0 x 100% [HA] 0 = initial concentration 11.7
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11.11
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The common ion effect is the shift in equilibrium caused by the addition of a compound having an ion in common with the dissolved substance. Consider mixture of CH 3 COONa (strong electrolyte) and CH 3 COOH (weak acid). CH 3 COONa ( s ) Na + ( aq ) + CH 3 COO - ( aq ) CH 3 COOH ( aq ) H + ( aq ) + CH 3 COO - ( aq ) common ion 13.1 The presence of a common ion suppresses the ionization of a weak acid or a weak base. WHY?
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To calculate the pH of such solutions:       Ex.:  Calculate the pH of a buffer solution that is 0.050 M in  HAc and 0.20 M in NaAc.  (K a = 1.8 x 10 -5  ) Ac = acetate See blackboard notes in lecture.
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Consider mixture of salt NaA and weak acid HA. HA ( aq ) H + ( aq ) + A - ( aq ) NaA ( s ) Na + ( aq ) + A - ( aq ) K a = [H + ][A - ] [HA] [H + ] = K a [HA] [A - ] -log [H + ] = -log K a - log
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This note was uploaded on 05/30/2008 for the course CHEM 116 taught by Professor Lalancette during the Spring '08 term at Rutgers.

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mar1308 - percent ionization = Ionized acid concentration...

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