Just as pH is the negative logarithm of H3O+],pKa is the negative logarithm of Ka,pKa = – log KaThe Henderson-Hasselbalch equation is used tocalculate the pH of buffer solutions:pH = pK, +logbase][acid]%3DNotice 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]. SubmitPrevious Answersv CorrectPart BHow many grams of dry NH, Cl need to be added to 1.60 L of a 0.100 mol L- solution of ammonia, NH3 , to preparea buffer solution that has a pH of 8.54? K, for ammonia is 1.8 x 10-5.Express your answer to two significant figures and include the appropriate units.• View Available Hint(s)HAmass of NH4CI =ValueUnits%3DSubmitPrevious AnswersIncorrect; Try Again; 5 attempts remaining

We have a buffer solution of base NH3 and salt NH4Cl. From henderson hasselbalch equation ,…

How many grams of dry NH,Cl need to be added to 1.60 L of a 0.100 mol L- solution of ammonia, NH3 , to prepare a buffer solution that has a pH of 8.54? K, for ammonia is 1.8 x 10. Express your answer to two significant figures and include the appropriate units.

How many grams of dry NH,Cl need to be added to 1.60 L of a 0.100 mol L- solution of ammonia, NH3 , to prepare a buffer solution that has a pH of 8.54? K, for ammonia is 1.8 x 10. 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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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Just as pH is the negative logarithm of H3O+],
pKa is the negative logarithm of Ka,
pKa = – log Ka
The Henderson-Hasselbalch equation is used to
calculate the pH of buffer solutions:
pH = pK, +log
base]
[acid]
%3D
Notice that the pH of a buffer has a value close to
the pKa of the acid, differing only by the logarithm
of the concentration ratio [base]/[acid].

Submit
Previous Answers
v Correct
Part B
How many grams of dry NH, Cl need to be added to 1.60 L of a 0.100 mol L- solution of ammonia, NH3 , to prepare
a buffer solution that has a pH of 8.54? K, for ammonia is 1.8 x 10-5.
Express your answer to two significant figures and include the appropriate units.
• View Available Hint(s)
HA
mass of NH4CI =
Value
Units
%3D
Submit
Previous Answers
Incorrect; Try Again; 5 attempts remaining

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