Write a balanced equation for the proton transfer reaction between hydrofluoric acid (HF) and ammonia (NH₃). Identify each conjugate acid-base pair, and rewrite the equilibrium arrows to indicate if the forward or reverse reaction is favored.

Acid-base theory explains the behavior of acids and bases in chemical reactions. According to the Brønsted-Lowry theory, an acid is a proton donor, while a base is a proton acceptor. In the reaction between hydrofluoric acid (HF) and ammonia (NH₃), HF donates a proton to NH₃, forming the conjugate base fluoride (F⁻) and the conjugate acid ammonium (NH₄⁺). Understanding this theory is essential for identifying conjugate acid-base pairs.

Conjugate acid-base pairs consist of two species that differ by the presence of a proton (H⁺). In the reaction between HF and NH₃, HF and F⁻ form one conjugate pair, while NH₃ and NH₄⁺ form another. Recognizing these pairs is crucial for analyzing the reaction's dynamics and understanding how the strength of acids and bases influences the equilibrium position.

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. In the context of the HF and NH₃ reaction, the equilibrium can be shifted depending on the relative strengths of the acids and bases involved. By rewriting the equilibrium arrows to indicate whether the forward or reverse reaction is favored, one can predict the direction of the reaction based on the stability of the conjugate acids and bases.