(a) At equivalence point the pH of the solution suddenly increases indicating all the acetic acid has been consumed and pH increases only due to excess hydroxide OH- ions.
From the given data, sudden increase in pH occurs at pH = 9.98
pH at equivalence point = 9.98
(b) volume of NaOH at equivalence point = 30 mL
(c) Moles of NaOH at the equivalence point = 0.00300 mol
(d) Moles of HC2H3O2 at equivalence point = 0.00300 mol
(e) volume of NaOH added to reach equivalence point = 30 mL
volume of NaOH added to reach half-equivalence point = (volume of NaOH added to reach equivalence point) / 2
volume of NaOH added to reach half-equivalence point = (30 mL) / 2
volume of NaOH added to reach half-equivalence point = 15 mL
From the data, when volume of NaOH added is 15 mL, then pH = 4.47
pH at half equivalence point = 4.47
We know that pKa of weak acid is the pH at half equivalence point
pKa = pH at half equivalence point = 4.47
pKa = 4.47
(f) Ka of HC2H3O2 = 10-pKa
Ka of HC2H3O2 = 10-4.47
Ka of HC2H3O2 = 3.4 x 10-5
Volume NaOH added Moles of NaOH added 0.00010 Concentration of NaOH-0.1 M Concentration of HC H10.-01 M a) What is...
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Concentration of HCl is 0.09655 M. Concentration of NaOH is 0.100 M. a) What is the pH at equivalence point? b) Moles of HCl at equivalence point? c) Moles of NaOH at equivalence point? d) Volume of NaOH at equivalence point? 1.15 Volume NaOH added (mL) pH Moles of NaOH added 0.89 0.89 0.00010 0.89 0.00020 0.90 0.00030 0.91 0.00040 0.93 0.00050 0.94 0.00060 0.96 0.00070 0.98 0.00080 1.01 0.00090 1.03 0.00100 1.06 0.00110 1.08 0.00120 1.11 0.00130 0.00140 1.19...
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please help, thank you Consider a titration of 0.0200 moles HC H302 (a weak acid) with NaOH (a strong base). At the equivalence point, the total volume of the solution is 78.9 mL. What is the pH of this solution at this equivalence point? (Data: K = 1.8.10 for HC H302 and Kb = 5.56 . 10-10 for CH202)
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