Learning Goal:To understand how buffers use reserves ofconjugate acid and conjugate base to counteractthe effects of acid or base addition on pH.A buffer is a mixture of a conjugate acid-base pairIn other words, it is a solution that contains a weakacid and its conjugate base, or a weak base and itsconjugate acid. For example, an acetic acid bufferconsists of acetic acid, CH₂COOH, and itsconjugate base, the acetate ion CH,COOBecause 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 pairwork together to neutralize the addition of HorOH ions. Thus, for example, it Hions areadded to the acetate buffer described above, theywill be largely removed from solution by thereaction of H with the conjugate base:H+CH₂COO-CH₂COOHSimilarly, any added OH ions will be neutralizedby a reaction with the conjugate acidOH +CH₂COOH-CH₂COO+H₂OThis butter system is described by the Henderson-Hasselbalch equationpH=pK, +loggate adconjugate basePart AA 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 acidand 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 Howmuch will the pH change? The pK, of acetic acid is 4.740Express your answer numerically to two decimal places. Use a minus (-) sign if the pH has decreased.View Available Hint(s)ApH-VALSubmit Previous AnswersX Incorrect; Try Again; 6 attempts remainingProvide Feedback?Next >

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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

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter20: Acidity And Pka Of Phenols

Section: Chapter Questions

Problem 3CTQ

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If you wanted to make a buffer with an even higher buffering capacity, what change(s) would you make to the recipe?
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What questions and topics where asked on the interview and how did you think you did? Converted to an essay question? This question is about a buffer solution made by mixing together solutions containing ethanoic acid and sodium ethanoate. a) If you add a small amount of an acid such as dilute hydrochloric acid to this, the pH doesn't change much. Explain what happens to the extra hydrogen ions you have added (think in terms of pkas, acid/base and conjugate acid/base). . b) If you add a small amount of an alkali such as sodium hydroxide solution to the buffer solution, again the pH doesn't change much. There are two ways in which the extra hydroxide ions can be removed. What are they?
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Please answer the following questions as correct as possible. Thank you. What is the effect of total concentration of the buffer components on its buffering capacity? What is the effect of the ratio of conjugate base to acid on buffering capacity?
Within what pH range is a HOCl – NaOCl buffer effective? Answer: pH 6.5 – pH 8.5 (Please explain. Thank you.)