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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 ( 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
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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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
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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