Choose which one of the following can not be classed as buffer solution:
Correct answer: B. NaClO4/HClO4
- A. KH2PO4/H3PO4
- B. NaClO4/HClO4
- C. CH3COOH/CH3COONa
- D. NH4OH/NH4Cl
Explanation
The correct answer is Option B: NaClO4/HClO4. A buffer solution consists of a mixture of a weak acid and its conjugate base, or a weak base and its conjugate acid. NaClO4 and HClO4 do not form a buffer because they are products of a strong acid and a strong base, which do not resist pH changes effectively when an acid or base is added. In contrast, the other options contain either a weak acid and its conjugate base or a weak base and its conjugate acid, which are able to maintain a stable pH.
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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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