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The half-equivalence point of a titration occurs half way to the end point, where half of...

The half-equivalence point of a titration occurs half way to the end point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.280 moles of a monoprotic weak acid (Ka = 6.2 × 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point?

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Answer #1

   HA --------> H+ + A-

I         0.28            0     0

C       -x               +x    +x

E      0.28-x         +x    +x

Ka      = [H+][A-]/[HA]

6.2*10-5     = x*x/0.28-x

1.736*10-5 -6.2*10-5x = x2

x2 +6.2*10-5 -1.736*10-5 =0

    x = 0.00413

[H+]   = X = 0.00413M

half equivalent point = 0.00413/2 = 0.002065M

PH   = -log[H+]

      = -log0.002065

PH   = 2.685

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