Which of the following ions can act both as bronsted acid and base in solvent water?
Correct answer: C. HCO3-
- A. CN-
- B. SO42-
- C. HCO3-
- D. PO43-
Explanation
The correct answer is HCO3- because it can function as both a Bronsted acid and a Bronsted base in water. As a Bronsted acid, it donates a proton (H+) to form CO32-. As a Bronsted base, it accepts a proton to form H2CO3. The other options do not have this dual capability:CN-: Functions mainly as a Bronsted base by accepting protons.SO42-: Predominantly acts as a Bronsted base and is the conjugate base of a strong acid.PO43-: Primarily acts as a Bronsted base by accepting protons.
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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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