Final answer:
The pH of a 0.14 M NH4Cl solution can be calculated by considering the dissociation of NH4Cl in water and the reaction of NH4+ ions with water. The concentration of NH4+ ions is equal to the concentration of H3O+ ions, which is 0.14 M. Using the formula pH = -log[H3O+], the pH of the solution is 0.85.
Step-by-step explanation:
The pH of a solution can be determined using the formula:
pH = -log[H+]
In the case of NH4Cl, it is a salt that is formed from the reaction of ammonia (NH3) and hydrochloric acid (HCl).
NH4Cl dissociates in water to form NH4+ and Cl- ions. The NH4+ ions can react with water to form NH3 and H3O+ ions. Since NH3 is a weak base, it will partially react with water to form OH- ions as well.
The pH of the solution can be calculated by considering the concentration of NH4+ ions and the reaction with water to form H3O+ ions. Since NH4Cl is a strong electrolyte, it dissociates completely in water.
Step-by-step calculation:
1. Write the dissociation equation of NH4Cl in water:
NH4Cl --> NH4+ + Cl-
2. Calculate the concentration of NH4+ ions:
0.14 M * (1 mol NH4+ / 1 mol NH4Cl) = 0.14 M
3. Consider the reaction of NH4+ ions with water:
NH4+ + H2O --> NH3 + H3O+
4. Calculate the concentration of H3O+ ions:
The concentration of H3O+ ions will be equal to the concentration of NH4+ ions, which is 0.14 M.
5. Calculate the pH using the formula:
pH = -log[H3O+]
pH = -log(0.14) = 0.85