Which of the following is not Bronsted acid?
Correct answer: D. Cl-
- A. HCl
- B. H2O
- C. HS-
- D. Cl-
Explanation
The correct answer is Cl-. A Bronsted acid is defined as a substance that can donate a proton (H+). Cl- is the conjugate base of the strong acid HCl and lacks a proton to donate, thus it cannot act as a Bronsted acid. In contrast, HCl is a classic example of a Bronsted acid as it readily donates a proton. H2O, although neutral, can act as a Bronsted acid in some reactions by donating a proton to become OH-. Similarly, HS- can donate a proton to form S2-, playing the role of a Bronsted acid in some contexts.
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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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