Which is correct about a 1.0 × 10⁻³ M HCl solution & a 1.0 × 10⁻⁵ M HClO₄ solution?
Correct answer: B. The HCl solution is 100 times more acidic than the HClO₄ solution
- A. The HCl solution is less acidic than the HClO₄ solution
- B. The HCl solution is 100 times more acidic than the HClO₄ solution
- C. The HClO₄ solution is 100 times more acidic than the HCl solution
- D. None of these
Explanation
Acidity is determined by the H⁺ concentration. Since both are strong acids, the [H⁺] is equal to their molarity. The ratio of concentrations is (1.0 × 10⁻³) / (1.0 × 10⁻⁵) = 100. Thus, the HCl solution is 100 times more concentrated in H⁺ and more acidic.
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About Acids, Bases and Salts
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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