A beaker with 1.60x10^2mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of an acid and conjugate base in this buffer is 0.100M. A student adds 6.80mL of 0.490M HCI solution to the beaker. How much will the pH change? The pka of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus sign if the pH has decreased.

A beaker with 1.60x10^2mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of an acid and conjugate base in this buffer is 0.100M. A student adds 6.80mL of 0.490M HCI solution to the beaker. How much will the pH change? The pka of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus 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

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

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

A beaker with 1.60x10^2mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of an
acid and conjugate base in this buffer is 0.100M. A student adds 6.80mL of 0.490M HCI solution to the beaker. How
much will the pH change? The pKa of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a
minus sign if the pH has decreased.

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Step 1: Given data

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Step 2: Finding concentration of acetate ions

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Step 3: Finding concentration of acetic acid

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Step 4: Finding moles of acetate ions and acetic acid and HCl

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Step 5: Moles of acetic acid and acetate ions after the addition of HCl

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Step 6: pH of solution after addition of HCl

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Step 7: Finding change in pH

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