7.46. The ionization constant of acetic acid is 1.74 x 10-5. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH.
7.46. The ionization constant of acetic acid is 1.74 x 10-5. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH.
The dissociation equilibrium is
CH3? COOH? CH3? COO− + H+.
Let α be the degree of dissociation.
The equilibrium concentrations of CH3? COOH, CH3COO− and H+ are c (1−α), c (α) and c (α) respectively.
The equilibrium constant expression is Kc? = [CH3? COO−] [H+]? / [CH3? COOH].
Kc? = (cα) (cα) / c (1−α)?
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