What is the pH of a solution that contains 0.067 mol of HCl in 150 mL of water?

Give your answer to the correct number of significant figures.

A. 0.35
B. -0.35
C. 1.2
D. 3.4
E. 0.45
F. 0.350

Question

High School

Answer :

AlbertFrancis AlbertFrancis · Answer 1 · 2024-05-12T04:33:44-04:00

The pH of the solution that contains 0.067 mol of HCl in 150 mL of water is approximately 0.35.

To calculate the pH of the solution, we first need to calculate the concentration of H+ ions in the solution. We can use the formula:

pH = -log[H+]

Given that we have 0.067 mol of HCl in 150 mL of water, we need to convert the volume to liters:

150 mL = 0.150 L

Next, we can calculate the concentration of H+ ions:

Concentration of H+ ions = moles of HCl / volume of solution

Concentration of H+ ions = 0.067 mol / 0.150 L

Concentration of H+ ions = 0.447 mol/L

Now, we can calculate the pH:

pH = -log(0.447)

pH ≈ 0.35

Therefore, the pH of the solution is approximately 0.35.

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