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NH3 has a Kb of 1.8x10^-5. What is the pH of a 1.5 M solution of NH3? Given that Kb = 6.3x10^-5, find the concentration of the hydroxide anion in a 0.25 M solution of (CH3)3N.

Multiply the Kb value by the total ammonia concentration and the number 4. The total concentration is the sum of [NH4+] and [NH3] in the solution. This concentration must be。

The larger the Kb, the stronger the base and the higher the OH − concentration at equilibrium. The values of Kb for a number of common weak bases are given in Table 16.5.2.

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