Just as pH is the negative logarithm of [H3O+],pKa is the negative logarithm of Ka,- log KaThe Henderson-Hasselbalch equation is used tocalculate the pH of buffer solutions:How many grams of dry NH4C1 need to be added to2.00 L of a 0.600 mol L-' solution of ammonia, NH3,to prepare a buffer solution that has a pH of 8.80? Khfor ammonia is 1.8 × 10–5.pKabase]pH = pKa +log acidExpress your answer to two significant figures andinclude the appropriate units.Notice that the pH of a buffer has a value close tothe pKa of the acid, differing only by the logarithmof the concentration ratio [base]/[acid].• View Available Hint(s)?X•10nValuemass ofNHẠCI =Units

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How many grams of dry NH4C1 need to be added to 2.00 L of a 0.600 mol L¬' solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.80? Kp for ammonia is 1.8 × 10¬5. Express your answer to two significant figures and include the appropriate units.

How many grams of dry NH4C1 need to be added to 2.00 L of a 0.600 mol L¬' solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.80? Kp for ammonia is 1.8 × 10¬5. Express your answer to two significant figures and include the appropriate units.

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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