Strong base is dissolved in 645 mL of 0.200 M weak acid (K₂ = 3.64 × 10-5) to make a buffer with a pH of 4.11. Assume that the volume remains constant when the base is added. HA(aq) + OH-(aq) → H₂O(1) + A¯(aq) Calculate the pK, value of the acid, and determine the number of moles of acid initially present. pK₂ - initial amount: When the reaction is complete, what is the concentration ratio of conjugate base to acid? [A] [HA] How many moles of strong base were initially added? amount added: mol HA mol OH™
Strong base is dissolved in 645 mL of 0.200 M weak acid (K₂ = 3.64 × 10-5) to make a buffer with a pH of 4.11. Assume that the volume remains constant when the base is added. HA(aq) + OH-(aq) → H₂O(1) + A¯(aq) Calculate the pK, value of the acid, and determine the number of moles of acid initially present. pK₂ - initial amount: When the reaction is complete, what is the concentration ratio of conjugate base to acid? [A] [HA] How many moles of strong base were initially added? amount added: mol HA mol OH™
General, Organic, and Biological Chemistry
7th Edition
ISBN:9781285853918
Author:H. Stephen Stoker
Publisher:H. Stephen Stoker
Chapter10: Acids, Bases, And Salts
Section: Chapter Questions
Problem 10.118EP: Using the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer...
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Strong base is dissolved in 645 mL of 0.200 M weak acid (Ka
the volume remains constant when the base is added.
PK₂
HA(aq) + OH-(aq) →→→ H₂O(1) + A- (aq)
Calculate the pK, value of the acid, and determine the number of moles of acid initially present.
=
initial amount:
[A]
[HA]
=
When the reaction is complete, what is the concentration ratio of conjugate base to acid?
How many moles of strong base were initially added?
3.64 x 10-5) to make a buffer with a pH of 4.11. Assume that
amount added:
mol HA
mol OH](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff2298601-e616-44f1-82ae-40cb5a91e850%2F04c84c00-0655-47aa-8559-532a78ef3cdc%2F54sypqq_processed.png&w=3840&q=75)
Transcribed Image Text:Macmillan Learning
Strong base is dissolved in 645 mL of 0.200 M weak acid (Ka
the volume remains constant when the base is added.
PK₂
HA(aq) + OH-(aq) →→→ H₂O(1) + A- (aq)
Calculate the pK, value of the acid, and determine the number of moles of acid initially present.
=
initial amount:
[A]
[HA]
=
When the reaction is complete, what is the concentration ratio of conjugate base to acid?
How many moles of strong base were initially added?
3.64 x 10-5) to make a buffer with a pH of 4.11. Assume that
amount added:
mol HA
mol OH
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Step 1: Defining buffer solution
VIEWStep 2: Finding out the pKa value
VIEWStep 3: Moles of weak acid used initially
VIEWStep 4: Calculation for the ratio of molar concentration of conjugate base and acid
VIEWStep 5: Calculation for the moles of conjugate base in buffer solution
VIEWStep 6: Formation of BCA table
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