Lecture_Notes_092809b

Lecture_Notes_092809b - Lecture Note 9/30/2009

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APPLICATIONS OF AQUEOUS EQUILIBRIA Zumdahl Chapter 15
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Common Ion y Common Ion – an ion that comes from more than one source in the formation of a solution y Common Ion Effect – the equilibrium position shift caused by the presence of a common ion
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How will the pH of a solution containing 0.10 M HCl and 0.07 M KCl compare to that of a solution containing only 0.10 M HCl? Hi g her L o we r The same 28% 10% 63% 1. Higher 2. Lower 3. The same
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How will the pH of a solution containing 0.20 M HF and 0.10 M KF, compare to that of a solution containing only 0.20 M HF? Hi g her L o we r The same 29% 36% 35% 1. Higher 2. Lower 3. The same
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Common Ion y In 0.15 M NH 3 , 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 ammonia in a solution that is 0.15 M NH 3 and 0.45 M NH 4 Cl.
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Common Ion
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Buffers y Buffered Solution – a solution that resists changes to its pH. It contains a weak acid and its conjugate base or a weak base and its conjugate acid.
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This note was uploaded on 10/14/2009 for the course CHEM 105BLG at USC.

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Lecture_Notes_092809b - Lecture Note 9/30/2009

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