Calculating pH of a 0.23M H2SO4 Solution

[temaire]

Homework Statement

Calculate the pH of a solution of a concentration of 0.23 mol/L of H2SO4, if it completely ionizes in the solution.

Homework Equations

[H3O] = 10$$^{-pH}$$
pH = -log[H3O]

The Attempt at a Solution

The answer I got for this question is 0.34. I got this answer by first writing out the ionization equation for H2SO4, and determining how many hydronium ions are made, which I got as two. Then, I found out the concentration of the hydronium ions by multiplying 0.23 mol/L by 2. Then, I used pH = -log[H3O], and got the answer of 0.34. Am I right?

 

[symbolipoint]

Your described method is good. You are looking for the negative logarithm of 0.46 Molar.