Calculating pH of a 0.23M H2SO4 Solution

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To calculate the pH of a 0.23M H2SO4 solution, it is essential to recognize that sulfuric acid completely ionizes, producing two hydronium ions per molecule. This results in a hydronium ion concentration of 0.46M (0.23M x 2). The pH can then be calculated using the formula pH = -log[H3O]. The correct pH for this solution is approximately 0.34, confirming the method used in the calculations. Understanding the ionization of strong acids is crucial for accurate pH determination.
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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?
 
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Your described method is good. You are looking for the negative logarithm of 0.46 Molar.
 

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