Which of the following statements about the equilibrium constant of an acid is true?
a. The equilibrium constant of a weak acid is large.
b. The equilibrium constant of a strong acid is small.
c. The equilibrium constant of a weak acid is small.
d. The more an acid ionizes, the smaller is the equilibrium constant.
ANS: C
The KA is small because the H2CO3 concentration is quite large with respect to the numerator of reaction (3). The value of KA is always the same for H2CO3 at equilibrium, regardless of the ini-tial concentration of H2CO3. A strong acid, such as HCl, has a large KA because the denominator [HCl] is extremely small, compared with the numerator ([H+] ⋅ [Cl−]).
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