A beaker with 1.80x102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 5.10 mL of a 0.490 MHCI solution to the beaker. How much will the pH change? The pK, of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus ( View Available Hint(s) ApH= Submit 5 ΑΣΦ -0.27 Previous Answers ) sign if the pH has decreased.
A beaker with 1.80x102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 5.10 mL of a 0.490 MHCI solution to the beaker. How much will the pH change? The pK, of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus ( View Available Hint(s) ApH= Submit 5 ΑΣΦ -0.27 Previous Answers ) sign if the pH has decreased.
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
Chapter15: Acid-base Equilibria
Section: Chapter Questions
Problem 4RQ: A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If...
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![A beaker with 1.80x102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid
and conjugate base in this buffer is 0.100 M. A student adds 5.10 mL of a 0.490 MHCI solution to the beaker. How
much will the pH change? The pK, of acetic acid is 4.740.
Express your answer numerically to two decimal places. Use a minus ( ) sign if the pH has decreased.
View Available Hint(s)
ApH=
Submit
5 ΑΣΦ
-0.27
Previous Answers
* Incorrect; Try Again; 3 attempts remaining
First calculate the number of moles of conjugate acid and conjugate base in the initial buffer. Next, determine the
effect of the addition of the acid, HCl, on the total number of moles of conjugate acid and conjugate base.
Finally, use the Henderson-Hasselbalch equation to determine the new pH,
pH=pK+ log
conjugate base)
conjugate acid](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fefe48ce5-c1e8-4c52-aeb2-02053ba21519%2F8c71d4e0-99c9-499f-b0ed-8d44744c23ce%2Fiatongp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A beaker with 1.80x102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid
and conjugate base in this buffer is 0.100 M. A student adds 5.10 mL of a 0.490 MHCI solution to the beaker. How
much will the pH change? The pK, of acetic acid is 4.740.
Express your answer numerically to two decimal places. Use a minus ( ) sign if the pH has decreased.
View Available Hint(s)
ApH=
Submit
5 ΑΣΦ
-0.27
Previous Answers
* Incorrect; Try Again; 3 attempts remaining
First calculate the number of moles of conjugate acid and conjugate base in the initial buffer. Next, determine the
effect of the addition of the acid, HCl, on the total number of moles of conjugate acid and conjugate base.
Finally, use the Henderson-Hasselbalch equation to determine the new pH,
pH=pK+ log
conjugate base)
conjugate acid
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