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ira [324]
2 years ago
6

Look at Table 4 in the procedure portion of the experiment. Calculate the pH you would expect each of the buffer solutions (A, B

, C, D, and E) to be using the Henderson-Hasselbalch equation, assuming that the solutions of acetic acid and sodium acetate are equimolar.
Chemistry
1 answer:
ivann1987 [24]2 years ago
4 0

The pH of the buffer solutions as determined using the Henderson–Hasselbalch equation are:

  • A. pH = 4.75
  • B. pH = 4.05
  • C. pH = 3.75
  • D. pH = 5.75
  • E. pH = 5.45

<h3>What is the pH of the solutions?</h3>

The pH of a buffer is determined using the Henderson–Hasselbalch equation shown below:

  • pH = pKₐ + log([A⁻]/[HA])

A. Volume of acetic acid = 5 mL; Volume of sodium acetate = 5 mL; pka of acetic acid = 4.75

The solutions of acetic acid and sodium acetate are equimolar;

pH = 4.75 + log(1)

pH = 4.75

B. Volume of acetic acid = 5 ml; Volume of sodium acetate = 1 mL; pka of acetic acid = 4.75

The solutions of acetic acid and sodium acetate are equimolar;

pH = 4.75 + log(1/5)

pH = 4.05

C. Volume of acetic acid = 10 ml; Volume of sodium acetate = 1 mL; pka of acetic acid = 4.75

The solutions of acetic acid and sodium acetate are equimolar;

pH = 4.75 + log(1/10)

pH = 3.75

D. Volume of acetic acid = 1 ml; Volume of sodium acetate = 10 mL; pka of acetic acid = 4.75

The solutions of acetic acid and sodium acetate are equimolar;

pH = 4.75 + log(10/1)

pH = 5.75

E. Volume of acetic acid = 1 ml; Volume of sodium acetate = 5 mL; pka of acetic acid = 4.75

The solutions of acetic acid and sodium acetate are equimolar;

pH = 4.75 + log(5/1)

pH = 5.45

In conclusion, the pH of the buffer solutions are determined using the Henderson–Hasselbalch equation.

Learn more about buffers at: brainly.com/question/22390063

#SPJ1

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