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A 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH....

A 20.00-mL sample of formic acid (HCO2H) is titrated with a 0.100 M solution of NaOH. To reach the endpoint of the titration, 30.00 mL of NaOH solution is required. Ka = 1.8 x 10-4

What is the pH of the solution after the addition of 10.00 mL of NaOH solution?

What is the pH at the midpoint of the titration?

What is the pH at the equivalence point?

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