The pH of a 0.17-M solution of maleic acid (H2C4H2O4) is measured to be 1.40. Use...

The pH of a 0.17-M solution of maleic acid (H₂C₄H₂O₄) is measured to be 1.40. Use this information to determine a value of K_a for maleic acid.

H₂C₄H₂O₄(aq) + H₂O(l) ((double arrow)) HC₄H₂O₄^-(aq) + H₃O⁺(aq) K_a =

Expert Solution

pH = 1.40

use:

pH = -log [H3O+]

1.40 = -log [H3O+]

[H3O+] = 0.0398 M

H2C4H2O4(aq) + H2O(l) —> HC4H2O4-(aq) + H3O+(aq)

0.17 0 0 (initial)

0.17-x x x (at equilibrium)

here,

[H3O+] = x = 0.0398 M

Ka = [HC4H2O4-][H3O+]/[H2C4H2O4]

Ka = x*x / (0.17-x)

Ka = 0.0398* 0.0398 / (0.17-0.0398)

Ka = 0.012

Answer: 0.012

queen_honey_blossom answered 2 years ago

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