Question

Determine the pH of an HF solution of each of the following concentrations:

a. 0.300 M
b. 4.70 × 10⁻² M
c. 2.60 × 10⁻² M

Answer 1

The pH of an HF solution can be determined using the equation pH = -log[H+]. For the given concentrations of HF, the pH values are: 0.300 M HF has a pH of 3.5, 4.70x10^(-2) M HF has a pH of 2.1, and 2.60x10^(-2) M HF has a pH of 2.3.

Step-by-step explanation:

The pH of an HF solution can be determined using the equation:

pH = -log[H+]

where [H+] is the concentration of hydronium ions in the solution. To find the pH, we need to convert the concentration of HF to the concentration of [H+].

For a concentration of 0.300 M HF, the concentration of [H+] can be calculated using the dissociation constant for HF, which is approximately 3.2x10^(-4) M. Taking the negative logarithm of this value gives a pH of 3.5.

For a concentration of 4.70x10^(-2) M HF, the concentration of [H+] can be calculated to be approximately 7.4x10^(-3) M, which corresponds to a pH of 2.1.

For a concentration of 2.60x10^(-2) M HF, the concentration of [H+] can be calculated to be approximately 5.2x10^(-3) M, which corresponds to a pH of 2.3.