A beaker with 105 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. Astudent adds 5.80 mL of a 0.420 M HCl 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)

Chemistry: An Atoms First Approach
2nd Edition
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Author:Steven S. Zumdahl, Susan A. Zumdahl
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Chapter14: 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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Item 1
II Review | Constants | Periodic Table
Part A
A beaker with 105 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 5.80
mL of a 0.420 M HCl 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)
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Transcribed Image Text:Item 1 II Review | Constants | Periodic Table Part A A beaker with 105 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 5.80 mL of a 0.420 M HCl 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 ( Return to Assignment Provide Feedback
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