+ Base/Acid Ratios in BuffersJust as pH is the negative logarithm of [H3O+].PK₁ is the negative logarithm of Ka.PK₂ = -log KaThe Henderson-Hasselbalch equation is used to calculate the pH ofbuffer solutions:pH=pK₁ +log base[acid]Notice that the pH of a buffer has a value close to the PK₂ of the acid,differing only by the logarithm of the concentration ratio [base]/[acid].The Henderson-Hasselbalch equation in terms of pOH and PKb issimilar.lacid]pOH = pk + logadbasepH 3.74[acetic acid] ten timesgreater than [acetate]Submit✓ Correct▼ Part BpH = 4.74Previous Answers[acetate] = [acetic acid]mass of NH4Cl =pH = 5.74[acetate] ten timesgreater than [acetic acid]ValueHow many grams of dry NH4Cl need to be added to 2.00 L of a 0.100 M solution of ammonia, NH3. to prepare a buffer solution that has a pH of 8.85? Kb for ammonia is1.8 x 10-5Express your answer with the appropriate units.▸ View Available Hint(s)( 2 FTemplates Symbols undo relo reset keyboard shortcuts help7 of 39 XUnitsReview | Constants | Periodic Table

Answered: Image /qna-images/answer/76c21ffd-2f7b-4454-93c3-eb102e59c312.jpg

Part B How many grams of dry NH,CI need to be added to 2.00 L of a 0.100 M solution of ammonia, NH3. to prepare a buffer solution that has a pH of 8.85? Kb for ammonia is 1.8 x 10 Express your answer with the appropriate units. ▸ View Available Hint(s)

Part B How many grams of dry NH,CI need to be added to 2.00 L of a 0.100 M solution of ammonia, NH3. to prepare a buffer solution that has a pH of 8.85? Kb for ammonia is 1.8 x 10 Express your answer with the appropriate units. ▸ View Available Hint(s)

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

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

+ Base/Acid Ratios in Buffers
Just as pH is the negative logarithm of [H3O+].
PK₁ is the negative logarithm of Ka.
PK₂ = -log Ka
The Henderson-Hasselbalch equation is used to calculate the pH of
buffer solutions:
pH=pK₁ +log base
[acid]
Notice that the pH of a buffer has a value close to the PK₂ of the acid,
differing only by the logarithm of the concentration ratio [base]/[acid].
The Henderson-Hasselbalch equation in terms of pOH and PKb is
similar.
lacid]
pOH = pk + logad
base
pH 3.74
[acetic acid] ten times
greater than [acetate]
Submit
✓ Correct
▼ Part B
pH = 4.74
Previous Answers
[acetate] = [acetic acid]
mass of NH4Cl =
pH = 5.74
[acetate] ten times
greater than [acetic acid]
Value
How many grams of dry NH4Cl need to be added to 2.00 L of a 0.100 M solution of ammonia, NH3. to prepare a buffer solution that has a pH of 8.85? Kb for ammonia is
1.8 x 10-5
Express your answer with the appropriate units.
▸ View Available Hint(s)
( 2 F
Templates Symbols undo relo reset keyboard shortcuts help
7 of 39 X
Units
Review | Constants | Periodic Table

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