071608 - 1874 – 1962 Danish Chemist Henderson-Hasselbalch...

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APPLICATIONS OF AQUEOUS EQUILIBRIA Zumdahl Chapter 15
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Common Ion y Common Ion – y Common Ion Effect –
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Common Ion 0.025 M HCN 0.025 M HCN 0.010 M NaCN
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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 –
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Buffers y Calculate the concentrations of all species present, the pH, and the percent dissociation of HCN (K a = 4.9 x 10 -10 ) in a solution of 0.025 M HCN and 0.010M NaCN.
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Buffers y Calculate the pH change that occurs when 0.010 mol HCl is added to 1.0 L 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 1.0 L of water.
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Buffers
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Buffers
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Henderson-Hasselbalch Equation Lawrence Joseph Henderson 1878 – 1942 American Biochemist Karl Albert Hasselbalch
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Unformatted text preview: 1874 – 1962 Danish Chemist Henderson-Hasselbalch Equation y Use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution that is 0.25 M in formic acid (HCHO 2 ) and 0.50M in sodium formate (NaCHO 2 ). Henderson-Hasselbalch Equation y What happens to the pH of the solution on the previous slide when the solution is diluted by a factor of two? Buffering Capacity Buffering Capacity y Which of the following solutions has the greater buffer capacity? { 100 mL of 0.30 M HNO 2 /0.30 M NaNO 2 { 100 mL of 0.10 M HNO 2 /0.10 M NaNO 2 Preparing a Buffer y In what volume ratio should you mix 1.0 M solutions of NH 4 Cl and NH 3 to produce a buffer solution having a pH 9.80. (NH 3 K b = 1.8 x 10-5 ) Preparing a Buffer y Using the following table determine the best acid and its conjugate base that would best form a buffer with a pH of 2.9. Buffers: A Summary...
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