Compare the Ka of acids?
25ml acetic acid reacted at 4.000ml of NaOH (ph of 8.95).
The equivalence point from the graph (HCl) is at the 20th marker. This is midpoint of vertical ph curve
This solution turned pink at the 19th marker with a ph of 8.88.
The pH at the equivalence point is 9.00
The volume of NaOH at the equivalence point is 15.0004 ml
The pH at the half-equivalence point is .61
molarity is 25ml HCl=.300008M
Compare the Ka of the acids in the two experiments. ???
a. Explain what accounts for the difference between the values. ???
If this makes sense to anyone. If you need more info, let me know.
Answer:
As a general postulate, HCl is going to have a higher Ka than acetic acid. This is because HCl is much more soluble in water and solutions than HC2H3O2.
HCl completely dissociates in solution, while aceitc acid does not. This accounts for the difference.
Hope that helps.
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