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.

Verified step by step guidance

1. Identify the reactants: Hydrofluoric acid (HF) is the acid, and ammonia (NH₃) is the base.
2. Write the unbalanced equation for the proton transfer: HF + NH₃ \rightarrow F^- + NH₄^+.
3. Balance the equation: Ensure that the number of atoms and charges are balanced on both sides of the equation.
4. Identify the conjugate acid-base pairs: HF and F^- form one pair, while NH₃ and NH₄^+ form the other pair.
5. Determine the direction of the equilibrium: Compare the strengths of the acids and bases involved to decide if the forward or reverse reaction is favored.

Key Concepts

Proton Transfer Reaction

A proton transfer reaction, also known as an acid-base reaction, involves the transfer of a proton (H⁺) from an acid to a base. In this context, hydrofluoric acid (HF) acts as the acid, donating a proton, while ammonia (NH₃) serves as the base, accepting the proton. Understanding this concept is crucial for writing the balanced equation and identifying the conjugate acid-base pairs.

Conjugate Acid-Base Pairs

Conjugate acid-base pairs consist of two species that differ by the presence of a proton. In the reaction between HF and NH₃, HF donates a proton to form its conjugate base, fluoride ion (F⁻), while NH₃ accepts the proton to form its conjugate acid, ammonium ion (NH₄⁺). Identifying these pairs is essential for understanding the dynamics of the reaction and the equilibrium established.

Equilibrium Arrows

Equilibrium arrows (↔) indicate that a reaction can proceed in both the forward and reverse directions, establishing a dynamic balance between reactants and products. In this case, the direction favored can be indicated by the relative strengths of the acids and bases involved. Understanding how to represent these arrows helps in analyzing the reaction's tendency to favor either the formation of products or the reformation of reactants.