Question

How does Ka relate to acid strength?

Answer 1

Hey mate here is Ur ans

*Relating Ka and pKa

A related value is pKa, which is the logarithmic acid dissociation constant:

pKa = -log10Ka

Using Ka and pKa To Predict Equilibrium and Strength of Acids

Ka may be used to measure the position of equilibrium:

#If Ka is large, the formation of the products of the dissociation is favored.

#If Ka is small, the undissolved acid is favored.

Ka may be used to predict the strength of an acid:

#If Ka is large (pKa is small) this means the acid is mostly dissociated, so the acid is strong. Acids with a pKa less than around -2 are strong acids.

#If Ka is small (pKa is large), little dissociation has occurred, so the acid is weak. Acids with a pKa in the range of -2 to 12 in water are weak acids.

#Ka is a better measure of the strength of an acid than pH because adding water to an acid solution doesn't change its acid equilibrium constant, but does alter the H+ ion concentration and pH.

#Ka Example

The acid dissociation constant, Ka of the acid HB is:

HB(aq) ↔ H+(aq) + B-(aq)

Ka = [H+][B-] / [HB]

For the dissociation of ethanoic acid:

CH3COOH(aq) + H2O(l) = CH3COO-(aq) + H3O+(aq)

Ka = [CH3COO-(aq)][H3O+(aq)] / [CH3COOH(aq)]

I hope this will helps you

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