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4.0 x 10 and K2 = 8.2 x 109 For the diprotic weak acid H2A, Kal What is the pH of a 0.0700 M solution of H,A? Enter numeric v

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Answer #1


H2A is diprotic acid

H2A -------------------> HA- + H+

I 0.0700                           0          0

C     -x                              +x        +x

E ( 0.0700-x)                    x          x

Ka1 = [H+] [ HA- ] / [ H2A ]

=> 4.0*10-6 = [ x2 ] / [0.07-x]

=> 4.0*10-6 * [0.07-x] = [ x2 ]

=> x = 0.00053 M

[H+ ] = 0.00053 M

pH = -log [H+]

pH = -log [0.00053 ]

pH = 3.27

     HA- ------------------->    A2- + H+

I 0.00053                           0         0.00053

C     -x                                +x        +x

E ( 0.00053-x)                    x          (0.00053+x)

Ka2 = [H+] [ A2- ] / [ HA- ]

=> 8.2*10-9 = (0.00053+x)(x) / (0.00053-x)

=> x = 8.2*10-9 M

[A2-] = 8.2*10-9

answers =>

pH = 3.27

[H2A] = 0.06947 M

[A2-] = 8.2*10-9 M

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