Problem: Enough of a monoprotic acid is dissolved in water to produce a 0.0192 M solution. The pH of the resulting solution is 2.53. Calculate the Ka for the acid.

FREE Expert Solution

The dissociation of a monoprotic weak acid (HA) is as follows:

HA(aq) + H2O(l) ⇌ H3O+(aq) + A–(aq)


From this, we can construct an ICE table. Remember that liquids are ignored in the ICE table and Ka expression.

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Enough of a monoprotic acid is dissolved in water to produce a 0.0192 M solution. The pH of the resulting solution is 2.53. Calculate the Ka for the acid.

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