2.643 grams of potassium butanoate (KCH3(CH2)2CO2 ) is fully dissolved in 50.00 mL of
water, which is carefully transferred to a conical flask. Then 100.00 mL of 0.120 M HCℓ is
added dropwise to this solution from a burette.
Given: Ka(butanoic acid) = 1.5 × 1O−5 .
2.1 Showing all your calculations and reasoning, determine the pH of the solution that
results after the addition of all the acid mentioned above.
[10]
2.2 Suppose that the titration continues. Determine the pH of the solution in the flask at the
equivalence point.
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