How do you calculate the molarities of #CH_3COOH# and #CH_3COO^-# in buffer solution?

Answer 1

#pH=pK_a+log_10{[[AcO^-]]/[[HOAc]]}#

Well, you need starting concentrations of acetic acid and acetate, and also the #pK_a# of #"acetic acid"#, which is #4.76#. See here for the derivation of this formula.

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Answer 2

Cameron Andrews

To calculate the molarities of CH3COOH and CH3COO^- in a buffer solution, you would use the Henderson-Hasselbalch equation:

pH = pKa + log([CH3COO^-]/[CH3COOH])

Solve for [CH3COO^-] and [CH3COOH] using the known values of pH and pKa, the dissociation constant of acetic acid.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.