Final answer:
The pH of a 0.050 M aqueous solution of ammonium chloride (NH4Cl) is expected to be within the acidic range, likely between 4 and 6, due to the partial ionization of NH4Cl in water and its acid dissociation constant Ka being 5.6 × 10⁻¹⁰.
Step-by-step explanation:
To determine the pH range of a 0.050 M aqueous solution of ammonium chloride (NH4Cl), we need to consider how NH4Cl affects the solution's pH. Ammonium chloride dissociates in water to form ammonium ions (NH4+) and chloride ions (Cl-). The ammonium ion is the conjugate acid of ammonia and can donate a proton to water, producing hydronium ions (H3O+) and making the solution acidic.
The pH of the solution can be estimated using the equilibrium equation for the reaction of ammonium ions with water and the known value of the acid dissociation constant (Ka) for the ammonium ion, which is 5.6 × 10⁻¹⁰. Using this Ka value and the initial concentration of ammonium ions, which equals the concentration of NH4Cl since it completely ionizes, we can use an ICE table (Initial, Change, Equilibrium) to calculate the concentration of hydronium ions and then determine the pH of the solution.
Since NH4Cl is a weak acid and 0.050 M is a relatively low concentration, we would expect the pH to be acidic but not extremely so, likely within the range of 4 to 6. This is because weak acids do not completely ionize in water, and so the pH change they cause is less significant compared to strong acids.