When dealing with a buffer, we use the Henderson-Hasselbalch equation:
The reaction between HC2H3O2 and NaOH is shown below:
HC2H3O2(aq) + NaOH(aq) → C2H3O2-(aq) + H2O(l)
(weak acid) (conjugate base)
**Na+ is not included in the reaction because it is a neutral ion
Calculate the initial amount of HC2H3O2 in moles:
moles HC2H3O2 = 2.0 mol HC2H3O2
We need to construct an ICF chart to determine the amounts of the species after the reaction:
Substitute values in the Henderson-Hasselbalch equation:
**log is a base of 10, when you divide a number by log, you will take 10 raised to the power of the number
What quantity (moles) of NaOH must be added to 1.0 L of 2.0 M HC2H3O2 to produce a solution buffered at each pH?
a. pH = pKa
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