Calculate the ph of a solution containing 0.75 m lactic acid and 0.25 m sodium lactate.
Question
Calculate the ph of a solution containing 0.75 m lactic acid and 0.25 m sodium lactate.
Solution
To calculate the pH of a solution containing lactic acid and sodium lactate, we need to use the Henderson-Hasselbalch equation, which is:
pH = pKa + log([A-]/[HA])
Where:
- [A-] is the concentration of the base (sodium lactate in this case)
- [HA] is the concentration of the acid (lactic acid in this case)
- pKa is the acid dissociation constant. For lactic acid, pKa is approximately 3.86.
Let's plug the values into the equation:
pH = 3.86 + log(0.25/0.75)
First, calculate the value of the log term:
log(0.25/0.75) = log(0.33) = -0.48
Then, substitute this value back into the equation:
pH = 3.86 - 0.48 = 3.38
So, the pH of the solution is approximately 3.38.
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