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. A Malate buffer solution (pKa₁ = 3.51 and pKa2 = 5.03) contains 480.00 mM Malic acid and 640.00 mM Malate (conjugate base). a. What is the pH of the buffer? b. If you were to take 2.40 L of the buffer in part A and add 100.00 mL of 3.00 M HCI, what would the new pH be? c. If you then added 80.00 mL of 10.00 M NaOH to your solution from part B, what would the final pH be?

. A Malate buffer solution (pKa₁ = 3.51 and pKa2 = 5.03) contains 480.00 mM Malic acid and 640.00 mM Malate (conjugate base). a. What is the pH of the buffer? b. If you were to take 2.40 L of the buffer in part A and add 100.00 mL of 3.00 M HCI, what would the new pH be? c. If you then added 80.00 mL of 10.00 M NaOH to your solution from part B, what would the final pH be?

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Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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3. A Malate buffer solution (pKa₁ = 3.51 and pka2 = 5.03) contains 480.00 mM Malic acid and 640.00 mM Malate (conjugate base). a. What is the pH of the buffer? b. If you were to take 2.40 L of the buffer in part A and add 100.00 mL of 3.00 M HCI, what would the new pH be? c. If you then added 80.00 mL of 10.00 M NaOH to your solution from part B, what would the final pH be?
Transcribed Image Text:3. A Malate buffer solution (pKa₁ = 3.51 and pka2 = 5.03) contains 480.00 mM Malic acid and 640.00 mM Malate (conjugate base). a. What is the pH of the buffer? b. If you were to take 2.40 L of the buffer in part A and add 100.00 mL of 3.00 M HCI, what would the new pH be? c. If you then added 80.00 mL of 10.00 M NaOH to your solution from part B, what would the final pH be?
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