Question

Calculate the pH of an aqueous HCl solution with [HCl]=0.0037 M. Is this acidic, basic, or neutral?

Answer 1

The pH of an aqueous HCl solution with [HCl]=0.0037 M is approximately 2.43 which is acidic. To find the pH of a 0.0037 M HCl solution, we calculate pH = -log(0.0037), resulting in a pH of 2.43, indicating the solution is acidic.

Step-by-step explanation:

To calculate the pH of an aqueous HCl solution with a concentration of [HCl]=0.0037 M, we use the formula pH = -log[H3O+].

Because HCl is a strong acid, it dissociates completely in water, meaning [H3O+] equals the concentration of HCl, which is 0.0037 M.

The calculation is as follows: pH = -log(0.0037), resulting in a pH of approximately 2.43.

Given that the pH scale ranges from 0 to 14, with 7 being neutral, a pH lower than 7 indicates an acidic solution.

Therefore, this HCl solution is acidic.

Answer 2

The pH of the aqueous HCl solution with a concentration of 0.0037 M is approximately 2.43, indicating that the solution is acidic.

Step-by-step explanation:

To calculate the pH of an aqueous HCl solution with a concentration of 0.0037 M, you need to use the formula:

pH = -log[H3O+]

Since HCl is a strong acid, it dissociates completely in water, which means that [H3O+] is equal to [HCl]. Therefore, the hydrogen ion concentration [H3O+] is also 0.0037 M.

The calculation will be as follows:

pH = -log(0.0037)

The result is approximately:

pH ≈ 2.43

Since the pH is less than 7, this indicates that the solution is acidic.