Question

What is the pH of a solution of 0.33 M H₂SO₄ (sulfuric acid)?

A) 0
B) 1
C) 2
D) 3

Answer 1

The pH of a 0.33 M solution of H2SO4 (sulfuric acid) is approximately 0.

Step-by-step explanation:

The pH of a solution can be determined by the concentration of hydrogen ions ([H+]). In the case of sulfuric acid (H2SO4), it is a strong acid that dissociates completely in water. Each molecule of H2SO4 will produce 2 H+ ions in solution. Since the concentration of H2SO4 is 0.33 M, the concentration of H+ ions is twice that, which is 0.66 M.

Now, to find the pH, we take the negative logarithm (base 10) of the hydrogen ion concentration:

pH = -log [H+]

Substituting the concentration value, we get:

pH = -log (0.66) ≈ 0.18

Therefore, the pH of a 0.33 M solution of H2SO4 (sulfuric acid) is approximately 0.