Part E A diprotic acid has a pKa1 -2.80 and pka2 6.50. What is the pH of a 0.10 M solution of thi...

Question

Question

Part E A diprotic acid has a pKa1 -2.80 and pka2 6.50. What is the pH of a 0.10 M solution of this acid that has been one qua

Answer 1

Answer #1

Answer

pH = 2.80

Explanation

Dissociation of diprotic acid is as follows

H2A <------> HA^- + H⁺ pKa1 = 2.80

HA^- <-------> A^2- + H⁺ pKa2 = 6.50

at half neutralization

H2A = HA^-

Henderson - Hasselbalch equation is

pH = pKa + log([HA^-]/[H2A])

pH = 2.80 + log1

pH = 2.80

Therefore

at quarter neutralization point , pH = 2.80

Answer 2

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