10. Acids and Bases

Hypobromous acid (Ka = 2.8 × 10⁻⁹) and hydrocyanic acid (Ka = 4.9 × 10⁻¹⁰) are both weak acids. Determine if reactants or products are favored in the following reaction.

HBrO (aq) + CN⁻ (aq) ⇌ BrO⁻ (aq) + HCN (aq)

Identify a Bronsted-Lowry acid with weakest conjugate base.

Identify which of the compounds is the strongest species.

Rearrange the equation you wrote in Problem 10.50 to solve for [H₃O⁺] in terms of K_a.

Determine the pK_a given the K_b of the following bases:

i) NH₃ K_b = 1.76 × 10⁻⁵ ; NH₄⁺ pK_a = ____________

ii) C₆H₅NH₂ K_b = 3.9 × 10⁻¹⁰ ; C₆H₅NH₃⁺ pK_a = ____________