Assume the titrations today used a known HCl concentration of 0.1 M. Using the experimental data what would the concentration of the NaOH titrant be?
Assume the titrations today used a known HCl concentration of 0.1 M. Using the experimental data what would the concentration of the NaOH titrant be?
Reaction equations are shown in net ionic form.
H+ (aq) + OH– (aq) → H2O(l)
HC2H3O2(aq) + OH– (aq) → H2O(l) + C2H3O2– (aq)
Volume of HCl = 5ml
NaOH Concentration = 0.100 M
Volume of NaOH at Endpoint for HCl Trial = 4.79ml
Volume of NaOH at Equivalence point for HCl Trial = 5.083ml
Equivalence point pH for HCl Trial = 6.57
pH 1/2 Equivalence point for HCl Trial = 3.285
Volume for HC2H3O2= 5ml
NaOH Concentration = 0.100 M
Volume of NaOH at Endpoint for HC2H3O2 Trial = 3.67ml
Volume of NaOH at Equivalence point for HC2H3O2 Trial= 4.025ml
Equivalence point pH for HC2H3O2 Trial = 4.13
pH 1/2 Equivalence point for HC2H3O2 Trial = 2.065
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