Henderson-Hasselbalch equation
pH =pKa + log [(Base)/(acid)]
4.56 = 4.76 + log[(X)/(0.49)]
log[(X)/(0.49)] = -0.2, X = 0.3 M
we have 2.4M NaOH
Let us assume required volume of NaOH = x ml
2.4M NaOH xml = 0.3 x (775+x) = 232.5 + 0.3x
x = 110.71 ml
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acetic acid solution and a 2.48 M KOH solution. If you have 575 mL
of the acetic acid solution, how many milliliters of the KOH
solution do you need to add to make a buffer of pH 6.29? The pKa of
acetic acid is 4.76.
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