Consider the weak bases below and their Kb values:NH3 Kb = 1.8 * 10^-5C2H5NH2 Kb = 5.6 *10^-4C5H5N Kb = 1.7 * 10^-9Arrange the conjugate acids of these weak bases in order of increasing acid

Consider the weak bases below and their Kb values:

NH₃: Kb = 1.8 × 10⁻⁵

C₂H₅NH₂: Kb = 5.6 × 10⁻⁴

C₅H₅N: Kb = 1.7 × 10⁻⁹

Arrange the conjugate acids of these weak bases in order of increasing acid

strength.

Solution:

The higher the Kb value, the stronger the base. The stronger the base, the weaker its conjugate acid is.

Conjugate acid has one more hydrogen then the base, conjugate acids are C₂H₅NH₃⁺, NH₄⁺, C₅H₅NH⁺ The answer is: C₂H₅NH₃⁺<NH₄⁺<C₅H₅NH⁺