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What is the pH of a solution that is initially 6.76×10–4 M HClO4 and 1.887 M...

What is the pH of a solution that is initially 6.76×10–4 M HClO4 and 1.887 M HCOOH? The Ka of HCOOH is 1.8×10–4 . 1.73

The answer is 1.73. Please include work and explanation. Thank you!

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Homework Answers

Answer #1

HClO4 is strong acid . so H+ concentration = 6.76×10–4 M

HCOOH is weak acid . H+ concentratin = sqrt (Ka x C)

[H+] = sqrt (1.8×10–4 x 1.887)

         = 0.0184 M

compared to H+ from HCOOH , HClO4 H+ concetration is very less so we can neglect that

total [H+] = 0.0184 + 6.76 x 10^-4

               = 0.0184 M (nearly)

pH = -log [H+]

pH = -log (0.0184)

pH = 1.73

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