"Calculate the ionization constant for each of the following acids or bases from the ionization constant of its conjugate base or conjugate acid:
(CH3)3NH+"```plaintext
To calculate the ionization constant (Ka) for (CH3)3NH+ (trimethylammonium ion) as an acid, we need the Kb value of its conjugate base, (CH3)3N (trimethylamine).
The relationship between the ionization constants of a conjugate acid-base pair is given by:
Ka × Kb = Kw
where Kw is the ionization constant for water, which is 1.0 × 10^−14 at 25°C.
The Kb for (CH3)3N (trimethylamine) is approximately 7.4 × 10^−4.
Now, we can calculate Ka for (CH3)3NH+ using the equation:
Ka = Kw / Kb
Ka = (1.0 × 10^−14) / (7.4 × 10^−4)
Ka = 1.35 × 10^−11
Thus, the ionization constant for (CH3)3NH+ as an acid is 1.35 × 10^−11.
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