Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
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Chapter 15 Solutions
Chemistry: An Atoms-Focused Approach
Ch. 15 - Prob. 15.1VPCh. 15 - Prob. 15.2VPCh. 15 - Prob. 15.3VPCh. 15 - Prob. 15.4VPCh. 15 - Prob. 15.5VPCh. 15 - Prob. 15.6VPCh. 15 - Prob. 15.7VPCh. 15 - Prob. 15.8VPCh. 15 - Prob. 15.9VPCh. 15 - Prob. 15.10VP
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- Without doing calculations, determine the pH of a buffer made front equimolar amounts of these acid-base pairs. (a) Phosphoric acid and sodium dihydrogen phosphate (b) Sodium monohydrogen phosphate and sodium dihydrogen phosphate (c) Sodium phosphate and sodium monohydrogen phosphatearrow_forwardCalculate the pH of these buffers.arrow_forward7. Describe a buffered solution. Give three examples of buffered solutions. For each of your examples, write equations and explain how the components of the buffered solution consume added strong acids or bases. Why is buffering of solutions in biological systems so important?arrow_forward
- Without doing calculations, determine the pH of a buffer made front equimolar amounts of these acid-base pairs. (a) Nitrous acid and sodium nitrite (b) Ammonia and ammonium chloride (c) Formic acid and potassium formatearrow_forwardA buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?arrow_forwardWhich of the following acids and its conjugate base would you use to make a buffer with a pH of 3.00? Explain your reasons: formic acid, lactic acid, nitrous acid.arrow_forward
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