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A beaker with 130x10 mL of an acetic acid butter 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 8.10 mil. of a 0.460 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 pit has decreased. View Available Hint(s) ApH- Submit AI- ΑΣΦ ProA -8? X Incorrect; Try Again; 6 attempts remaining

A beaker with 130x10 mL of an acetic acid butter 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 8.10 mil. of a 0.460 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 pit has decreased. View Available Hint(s) ApH- Submit AI- ΑΣΦ ProA -8? X Incorrect; Try Again; 6 attempts remaining

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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Learning Goal: To understand how buffers use reserves of conjugate acid and conjugate base to counteract the effects of acid or base addition on pH. A buffer is a mixture of a conjugate acid-base pair In other words, it is a solution that contains a weak acid and its conjugate base, or a weak base and its conjugate acid. For example, an acetic acid buffer consists of acetic acid, CH₂COOH, and its conjugate base, the acetate ion CH,COO Because ions cannot simply be added to a solution, the conjugate base is added in a salt form (e.g. sodium acetate NaCH₂COO) Buffers work because the conjugate acid-base pair work together to neutralize the addition of Hor OH ions. Thus, for example, it Hions are added to the acetate buffer described above, they will be largely removed from solution by the reaction of H with the conjugate base: H+CH₂COO-CH₂COOH Similarly, any added OH ions will be neutralized by a reaction with the conjugate acid OH +CH₂COOH-CH₂COO+H₂O This butter system is described by the Henderson- Hasselbalch equation pH=pK, +loggate ad conjugate base Part A A beaker with 1.30x10 mL of an acetic acid butter 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 8.10 mL of a 0.460 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- VAL Submit Previous Answers X Incorrect; Try Again; 6 attempts remaining Provide Feedback ? Next >
Transcribed Image Text:Learning Goal: To understand how buffers use reserves of conjugate acid and conjugate base to counteract the effects of acid or base addition on pH. A buffer is a mixture of a conjugate acid-base pair In other words, it is a solution that contains a weak acid and its conjugate base, or a weak base and its conjugate acid. For example, an acetic acid buffer consists of acetic acid, CH₂COOH, and its conjugate base, the acetate ion CH,COO Because ions cannot simply be added to a solution, the conjugate base is added in a salt form (e.g. sodium acetate NaCH₂COO) Buffers work because the conjugate acid-base pair work together to neutralize the addition of Hor OH ions. Thus, for example, it Hions are added to the acetate buffer described above, they will be largely removed from solution by the reaction of H with the conjugate base: H+CH₂COO-CH₂COOH Similarly, any added OH ions will be neutralized by a reaction with the conjugate acid OH +CH₂COOH-CH₂COO+H₂O This butter system is described by the Henderson- Hasselbalch equation pH=pK, +loggate ad conjugate base Part A A beaker with 1.30x10 mL of an acetic acid butter 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 8.10 mL of a 0.460 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- VAL Submit Previous Answers X Incorrect; Try Again; 6 attempts remaining Provide Feedback ? Next >
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