Two buffers are prepared by adding an equal numberof moles of formic acid (HCOOH) and sodium formate(HCOONa) to enough water to make 1.00 L of solution.Buffer A is prepared using 1.00 mol each of formic acid andsodium formate. Buffer B is prepared by using 0.010 mol ofeach. (a) Calculate the pH of each buffer. (b) Which bufferwill have the greater buffer capacity? (c) Calculate thechange in pH for each buffer upon the addition of 1.0 mLof 1.00 M HCl. (d) Calculate the change in pH for each bufferupon the addition of 10 mL of 1.00 M HCl.
Two buffers are prepared by adding an equal numberof moles of formic acid (HCOOH) and sodium formate(HCOONa) to enough water to make 1.00 L of solution.Buffer A is prepared using 1.00 mol each of formic acid andsodium formate. Buffer B is prepared by using 0.010 mol ofeach. (a) Calculate the pH of each buffer. (b) Which bufferwill have the greater buffer capacity? (c) Calculate thechange in pH for each buffer upon the addition of 1.0 mLof 1.00 M HCl. (d) Calculate the change in pH for each bufferupon the addition of 10 mL of 1.00 M HCl.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Two buffers are prepared by adding an equal number
of moles of formic acid (HCOOH) and sodium formate
(HCOONa) to enough water to make 1.00 L of solution.
Buffer A is prepared using 1.00 mol each of formic acid and
sodium formate. Buffer B is prepared by using 0.010 mol of
each. (a) Calculate the pH of each buffer. (b) Which buffer
will have the greater buffer capacity? (c) Calculate the
change in pH for each buffer upon the addition of 1.0 mL
of 1.00 M HCl. (d) Calculate the change in pH for each buffer
upon the addition of 10 mL of 1.00 M HCl.
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