Chemistry 32 Wednesday, November 15, 2006

Chemistry 32 Wednesday, November 15, 2006 - Wednesday,...

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Wednesday, November 15, 2006 Chemistry pH BALANCED How do you calculate pH? How do you rank pH? What’s a buffered solution? Text: Section 12.9 CALCUALTING pH OF ACIDS 1. pH a. a measure of how many H 3 O 1+ ions are in solution (how acidic) pH = -log[H 3 O 1+ ] “concentration of” 2. a logarithmic scale [H 3 O 1+ ]: 1M .1M .01M 10 -12 M pH: O 1 2 12 3. pH of strong acids: a. completely react with H 2 O to form H 3 O 1+ ) [H 3 O 1+ ] = [original acid] What is the pH of a 0.15 M solution of HCl? pH = -log[H 3 O 1+ ] = -log(0.15) = 0.82 Will 0.25 M HCl have a higher or lower pH? Lower Measure pH usually different than calculation of pH Because of ion pairing (some H 3 O 1+ and Cl 1- touching) 4. pH of weak acids: a. partially react with H 2 O [H 3 O 1+ ] ≠ [original acid] Need to calculate using Ka - CH201
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Wednesday, November 15, 2006 5. comparing pH’s of weak acids: a. larger Ka = greater % of H 3 O 1+ formed 0.1M solutions of” HC 2 H 3 O 2 NH 4 Cl Acid NH 4 1+ Cl
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This note was uploaded on 03/20/2008 for the course CH 101 taught by Professor Bigham during the Fall '08 term at N.C. State.

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Chemistry 32 Wednesday, November 15, 2006 - Wednesday,...

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