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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 0.540 moles of a monoprotic weak acid (Ka = 7.2 × 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point

​(answer is not 4.65)

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Answer #1

                         HA-----> H+ + A-

initial            0.54      0      0

change        -x        +x      +x

at equilibrium   0.54-x   +x     +x

Ka     = [H+][A-]/[HA]

7.2*10-5   = x*x/0.54-x

3.88*10-5 -7.2*10-5 x =x2

x2 +7.2*10-5 x-3.88*10-5 =0

x = 0.0061M

[H+]    = 0.0061M

PH   = -log[H+]

        = -log0.0061  

PH    = 2.214 >>> answer

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