Calculating pH of a 0.23M H2SO4 Solution

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SUMMARY

The pH of a 0.23M H2SO4 solution, which completely ionizes, is calculated to be 0.34. This calculation involves determining the concentration of hydronium ions, which is twice the concentration of sulfuric acid due to its complete ionization, resulting in 0.46M of H3O+. The formula used for calculating pH is pH = -log[H3O]. The method described is accurate and confirms the calculated pH value.

PREREQUISITES
  • Understanding of acid-base chemistry and ionization
  • Familiarity with the concept of molarity
  • Knowledge of logarithmic functions
  • Proficiency in using the pH formula: pH = -log[H3O]
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  • Study the properties of strong acids and their ionization in solutions
  • Learn about calculating pH for polyprotic acids
  • Explore the relationship between pH and hydronium ion concentration
  • Investigate the effects of dilution on pH in strong acid solutions
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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[tex]^{-pH}[/tex]
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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