Of ammonia, hydrazine, and hydroxylamine, which reacts to the greatest extent with the weak acid HNO₂? Consult Appendix C for equilibrium constants.

Acid-base reactions involve the transfer of protons (H+) between reactants. In this context, weak acids like HNO₂ can donate protons, while bases such as ammonia, hydrazine, and hydroxylamine can accept them. Understanding the strength of these acids and bases is crucial for predicting the extent of their reactions.

Equilibrium constants (K) quantify the ratio of products to reactants at equilibrium for a given reaction. A higher K value indicates a greater tendency for the reaction to proceed towards products. By consulting Appendix C for the equilibrium constants of the reactions involving ammonia, hydrazine, and hydroxylamine with HNO₂, one can determine which compound reacts most extensively.

Basicity refers to the ability of a substance to accept protons, while nucleophilicity describes the tendency of a species to donate an electron pair to form a bond. Ammonia, hydrazine, and hydroxylamine differ in their basicity and nucleophilicity, which influences their reactivity with weak acids like HNO₂. Understanding these properties helps predict which compound will react more significantly.