The value of Ka for the 0.738M solution, in which 12.5% dissociation of weak acid takes place is 1.1 × 10⁻².
Value of Ka for the given reaction will be calculated as:
Ka = [H₃O⁺][A⁻] / [HA].
ICE table for given chemical reaction according to the question is:
HA + H₂O ⇄ H₃O⁺ + A⁻
Initial: 0.738 0 0
Change: -0.09225 0.09225 0.09225
Equilibrium: 0.738-0.09225 0.09225 0.09225
[HA] = 0.738-0.09225 = 0.738 (because 0.09225 is very small as compare to 0.738, so it will non countable)
On putting all the values on the above equation we get,
Ka = (0.09225)² / 0.738 = 1.1 × 10⁻²
Hence, value of Ka is 1.1 × 10⁻².
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