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Drill: A 0.100 M solution of HZ ionizes 20.0 %. Calculate: KaHZ
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Buffer Solutions
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A solution that resists changes in pH
Buffer Solution A solution that resists changes in pH
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Made from the combination of a weak acid & its salt
Buffer Solution Made from the combination of a weak acid & its salt
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Made from the combination of a weak base & its salt
Buffer Solution Made from the combination of a weak base & its salt
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Buffer Examples Mix acetic acid & sodium acetate
Mix ammonia & ammonium chloride
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A buffer solution works best when the acid to salt ratio is
1 : 1
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A buffer solution works best when the base to salt ratio is
1 : 1
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Buffer Solution The buffering capacity of a solution works best when the pH is near the pKa
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pKa or pKb pKa = - log Ka pKb = - log Kb
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Calculate the pH of a solution containing
Buffer Problems Calculate the pH of a solution containing 0.10 M HAc in 0.10 M NaAc: Ka = 1.8 x 10-5
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AP CHM HW Problem: 9 Page: 421
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CHM II HW Problem: 11 Page: 818
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Calculate the pH of 0.10 M NH3 in
Buffer Problems Calculate the pH of 0.10 M NH3 in 0.20 M NH4NO3: Kb = 1.8 x 10-5
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Calculate the pH of a solution containing
Buffer Problems Calculate the pH of a solution containing 0.10 M HBz in 0.20 M NaBz: Ka = 6.4 x 10-5
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Calculate the pH of a solution containing
Drill: Calculate the pH of a solution containing 0.30 M HZ in 0.10 M NaZ: Ka = 3.0 x 10-5
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Calculate the pH of a solution containing
Buffer Problem Calculate the pH of a solution containing 0.50 M R-NH2 in 0.10 M R-NH3I: Kb = 4.0 x 10-5
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HA H+ + A- [H+][A-] [HA] Ka =
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HA H+ + A- [Ka][HA] [A-] [H+]=
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HA H+ + A- [HA] [A-] [H+] = (Ka)
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pH = [HA] [A-] pKa - log
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Henderson-Hasselbach Eq
pH = pKa + log
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Henderson-Hasselbach Eq
pOH = pKb+ log
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Buffer Problems Calculate the salt to acid ratio to make a buffer solution with pH = 5.0 Ka for HBZ = 2.0 x 10-5
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AP CHM HW Read: Chapter 14 Problem: 23 Page: 421
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CHM II HW Read: Chapter 19 Problem: 21 Page: 819
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Buffer Problems Calculate the salt to base ratio to make a buffer solution with pH = 9.48 Kb for MOH = 2.0 x 10-5
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Drill: Calculate the pH of a buffer solution containing 0.50 M HX in 0.25 M KX. Ka = 2.5 x 10-5
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Test Friday
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Point at which the # of moles of the two titrants are equal
Equivalence Point Point at which the # of moles of the two titrants are equal
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Titration Curves
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Calculate the HCO3- to H2CO3 ratio in blood with pH = 7.40
Ka1 for H2CO3 = 4.4 x 10-7
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150 ml of 0. 10 M NaOH is added to 100. 0 ml of 0. 10 M H2CO3
150 ml of 0.10 M NaOH is added to ml of 0.10 M H2CO3. Calculate pH. Ka1 for H2CO3 = 4.4 x 10-7 Ka2 for H2CO3 = 4.8 x 10-11
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AP CHM HW Read: Chapter 14 Problem: 33 Page: 422
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CHM II HW Read: Chapter 19 Problem: 31 Page: 819
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