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

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Discussion Overview

The discussion revolves around determining the pH of a 1% sulfuric acid solution, focusing on the conversion of concentration to moles and the implications of sulfuric acid's dissociation in solution.

Discussion Character

  • Technical explanation
  • Mathematical reasoning

Main Points Raised

  • One participant inquires about the molarity of a 1% sulfuric acid solution and its pH.
  • Another participant suggests that solution density is necessary for conversion, proposing either to assume a density of 1 g/mL or to consult density tables.
  • A participant proposes assuming a 1L solution volume to calculate molar concentration, indicating that sulfuric acid is a strong acid and suggesting 100% dissociation of H+ for pH calculation.
  • Another participant notes that while the first dissociation of sulfuric acid is strong, the second dissociation is relatively weak, estimating that about 76% exists in the HSO4- form.

Areas of Agreement / Disagreement

Participants express differing views on the extent of dissociation of sulfuric acid in solution, indicating that there is no consensus on the exact pH calculation method.

Contextual Notes

Assumptions about solution density and the degree of dissociation of sulfuric acid are not fully resolved, which may affect the pH calculation.

Mik0
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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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