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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
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
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Answer:
Explanation:
Hello.
In this case, we can solve this problem by applying the Boyle's law which allows us to understand the pressure-volume behavior as a directly proportional relationship:
In such away, knowing the both the initial pressure and volume and the final volume, we can compute the final pressure as shown below:
Consider that the given initial pressure is also equal to Pa:
Which stands for a pressure increase when volume decreases.
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