Which one is incorrect for one molar H2SO4 aqueous solution?
Correct answer: C. [H+] = [OH-]
- A. [H+] > 10-7
- B. pH < 7
- C. [H+] = [OH-]
- D. All are correct
Explanation
The correct answer is Option C: [H+] = [OH-. This is incorrect because in a strong acid solution like 1 M H2SO4, the concentration of hydrogen ions is significantly higher than that of hydroxide ions, hence [H+] > [OH-]. Option A is correct because the concentration of H+ in a 1 M sulfuric acid solution is indeed greater than 10-7. Option B is correct because strong acids have a pH less than 7. Option D is incorrect as not all the given statements are correct.
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Acid and base behaviour is explained through the Bronsted-Lowry transfer of protons and the Lewis donation or acceptance of electron pairs. The topic includes pH, pOH, ionisation and water equilibrium, plus salt formation and hydrolysis, where a salt solution may become acidic, basic or neutral.
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