Question

A solution is prepared by adding 0.023 moles of (H₃textO⁻₄ ) to 3.33L of water. What is the pH of this solution?

A. 1.5
B. 2.0
C. 2.5
D. 3.0

Answer 1

The pH of the solution is approximately 2.16.

Step-by-step explanation:

To find the pH of the solution, we need to calculate the concentration of hydronium ions, which is represented by the formula [H₃O⁺]. In this case, we are given that 0.023 moles of (H₃O⁻₄) are added to 3.33L of water. By dividing the moles of (H₃O⁻₄) by the volume of the solution, we can calculate the concentration: 0.023 moles / 3.33L = 0.0069 M.

Then, we can calculate the pH using the formula pH = -log[H₃O⁺]. Plugging in the concentration of hydronium ions, we get: pH = -log(0.0069) ≈ 2.16.

Therefore, the pH of the solution is approximately 2.16. The closest option provided is B. 2.0.