Final answer:
The question is about the equilibrium and ionization constants in acid-base chemistry at the college level, dealing with reactions in aqueous solutions.
Step-by-step explanation:
The subject of the question is Chemistry, specifically focusing on chemical equilibria and the ionization constants of weak acids and bases. The concept at hand involves the reversible reaction between nitrous acid (HNO₂) and ammonia (NH₃) to form ammonium (NH₄⁺) and nitrite ions (NO₂⁻). The question references the ionization of nitrite in water and how the addition of strong bases can shift the equilibrium of weak acids.
From the given information, it is apparent that the reaction occurs in an aqueous solution and also that the constants and the extent of ionization play a critical role in calculating the final concentrations of the involved species. For instance, the provided data points, such as ionization percentage, concentration of ion species (like [NH₃], [NO₂], [H₃O⁺]), and the reaction of nitrous acid with hydroxide ions, signify the importance of understanding acid-base equilibria.
To address problems like these effectively, a college-level understanding of acid-base reactions, equilibrium constants (K), and associated calculations are required.