Consider a liter of a buffered solution that is 0.110 M in formic acid and 0.100 M in sodium formate. What is the pH of the original buffer after the addition of 0.015 mol NaOH?
The Ka of formic acid is 1.8 x 10^4. I'm pretty sure the HendersenHasselbalch equation is supposed to be used here. I'm not sure what to plug in for the log(base/acid) though.
The Ka of formic acid is 1.8 x 10^4. I'm pretty sure the HendersenHasselbalch equation is supposed to be used here. I'm not sure what to plug in for the log(base/acid) though.
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@khal Kha L. asked the question.