What is the pH of 0.060 M NH4Cl?

* ? (What is the pH of 0.060 M NH4Cl (pKb=4.74 5.35 O 5.42 5.24 5.06 * Pure water is known as a strong electrolyte True False

Answer:

Explanation

Final answer: The pH of the 0.060 M NH4Cl solution can be calculated by considering the dissociation of NH4+ and the equilibrium constant. NH4Cl is a strong electrolyte that completely dissociates into NH4+ and Cl- ions. The initial concentration of NH4+ is equal to the concentration of NH4Cl, which is 0.060 M. By using the equilibrium constant and the concentration of NH4+, we can determine the pH of the solution.

Explanation:

To calculate the pH of the solution, we need to consider the dissociation of NH4Cl into NH4+ and Cl- ions. NH4Cl is a salt that dissociates completely in water, meaning it fully breaks apart into its constituent ions. The NH4+ ion can act as a weak acid, while the Cl- ion is the conjugate base. The dissociation of NH4+ can be represented by the following equation: NH4+ (aq) → NH3 (aq) + H+ (aq) The equilibrium constant for this dissociation is given by the expression: Ka = [NH3][H+] / [NH4+] Since NH4Cl is a strong electrolyte, it completely dissociates into NH4+ and Cl- ions. Therefore, the initial concentration of NH4+ is equal to the concentration of NH4Cl, which is 0.060 M. Now, we can calculate the pH of the solution using the equilibrium constant and the concentration of NH4+.
← Propane chemistry exploring carbon composition Calculating density of a copper penny →

More Posts: