If the ka of a monoprotic weak acid is 1.2 × 10-6, what is the ph of a 0.23 m solution of this acid?

The pH of a 0.23 M  monoprotic acid, whose Ka is 1.2 × 10⁻⁶, is 3.3.

Let's consider the dissociation reaction for a generic monoprotic weak acid.

HA(aq) ⇄ H⁺(aq) + A⁻(aq)

Given that the acid dissociation constant (Ka) is 1.2 × 10⁻⁶ and the concentration of the acid (Ca) is 0.23 M, we can calculate the concentration of H⁺ using the following expression.

The pH of the solution is:

The pH of a 0.23 M  monoprotic acid, whose Ka is 1.2 × 10⁻⁶, is 3.3.

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the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.

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