Calculate the pH of a buffer that is 0.13 M in lactic acid and 0.11 M in sodium lactate.
Answer (3)
acidity of lactic acid = pKa = 3.85 Ca = 0.13M Cs = 0.11M Henderson-Hasselbalch equation: pH = pKa + log(Cs/Ca) pH = 3.85 + log(0.11M/0.13M) = 3.85 + log0,846 = 3.85 - 0.073 = 3.777
The pH value of the** buffer **is mathematically given as
pH= 3.77
What is the pH value of the** buffer**?
Question Parameters:
The pH of a buffer that is 0.13 M in lactic acid and 0.11 M in sodium lactate
Generally, the equation for the pH Value is mathematically given as
pH = pKa + log(Cs/Ca)
Where
Ca = 0.13M
Cs = 0.11M
Therefore
pH = 3.85 + log(0.11M/0.13M)
pH= 3.85 + log0,846
pH= 3.85 - 0.073
pH= 3.77
Read more about pH value
https://brainly.com/question/15845370
The pH of the buffer solution consisting of 0.13 M lactic acid and 0.11 M sodium lactate is approximately 3.79, calculated using the Henderson-Hasselbalch equation. The pKa of lactic acid is typically 3.86, which is used in the calculation. The result shows how the ratio of concentrations of the acid and its conjugate base affects the pH of the buffer.
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