a). Sketch the titration curve that is expected when a 10.00 mL mixture of 0.0100 M HNO3 and 0.0100 M diprotic oxalic acid H2C2O4 are both titrated to a final equivalence point.
The Ka's for oxalic acid are Ka1 = 0.0540; Ka2 = 5.4 x 10â5.
The titrant is 0.010 M NaOH.
b). Calculate pH at the following points in the titration and clearly indicate these points on your sketch.
(a) Starting point, 0.00 mL titrant added. (Hint: the first H+ on oxalic acid is "not-so-weak")
(b) The first equivalence point. (Hint: What species is/are present? How many mL titrant added?)
(c) The second equivalence point. (Hint: what species is/are present?)
(d) The pH when a 10.0 mL excess is added, beyond the final equivalence point. (Hint: how many equivalence points should be observed?)
a). Sketch the titration curve that is expected when a 10.00 mL mixture of 0.0100 M HNO3 and 0.0100 M diprotic oxalic acid H2C2O4 are both titrated to a final equivalence point.
The Ka's for oxalic acid are Ka1 = 0.0540; Ka2 = 5.4 x 10â5.
The titrant is 0.010 M NaOH.
b). Calculate pH at the following points in the titration and clearly indicate these points on your sketch.
(a) Starting point, 0.00 mL titrant added. (Hint: the first H+ on oxalic acid is "not-so-weak")
(b) The first equivalence point. (Hint: What species is/are present? How many mL titrant added?)
(c) The second equivalence point. (Hint: what species is/are present?)
(d) The pH when a 10.0 mL excess is added, beyond the final equivalence point. (Hint: how many equivalence points should be observed?)
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