Why is acetate, CH3COO–, a weak base?
Solutions of sodium hydroxide and acetic acid are mixed.
Acetic acid is a weak acid. If equal volumes of equal molar solutions are mixed, will the
solution pH be >7, 7, or <7? Explain
Wouldn't the solution be less than 7 because acetic acid is an acid? Thanks.
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The reaction is: NaOH(aq) + HC2H3O2(aq) ==> H2O(l) + NaC2H3O2(aq)
The acetate ion produced, C2H3O2-, will react slightly with water (i.e. act as a weak base by accepting a H+ from H2O) to produce a small amount of OH-.
C2H3O2-(aq) + H2O(l) <==> HC2H3O2(aq) + OH-(aq)
This small amount of OH- produced makes the solution slightly alkaline.
Because it has two equivalent resonating structures which make it exceptionally stable and hence dusnt abstract protons readily frm water
the solution will be greater than 7 since sodium hydroxide is strongly basic and acetic acid is a weak acid hence making the solution basic. hope this helped :)
Acetate is a strong base! It releases 3 H+ ions for every acetate molecule.