What is the pH of a 1% sulfuric acid solution?

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A 1% (mass or volume) sulfuric acid solution can be calculated in moles by assuming a 1L volume, leading to 10g of sulfuric acid. Given that the molar mass of sulfuric acid (H2SO4) is approximately 98 g/mol, this results in a concentration of about 0.102 moles per liter. Since sulfuric acid is a strong acid, it is assumed to fully dissociate in the first step, contributing to the hydrogen ion concentration. However, the second dissociation is weaker, with approximately 76% existing in the HSO4- form. To determine the pH, the formula pH = -log([H+]) is applied, taking into account the dissociation characteristics of sulfuric acid. The density of the solution can be assumed to be 1 g/mL for simplification, or checked against tables for more accuracy.
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Can anyone tell me what a 1% (mass or volume) sulfuric acid solution is in moles? I want to find out the pH of a 1% (mass or volume) sulfuric acid solution?
 
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Correct me if I'm wrong but...
I think you can assume you have a solution 1L in volume. If 1% of that solution is sulfuric acid, you can find the molar concentration. Sulfuric acid is a strong acid so assume 100% dissociation of H+. Then just use the formula pH = -log([H+]) to get the pH.
 
spectre101 said:
Sulfuric acid is a strong acid so assume 100% dissociation of H+.

First dissociation step is strong, but the second is relatively weak. In this particular case about 76% is in the HSO4- form.

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