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Brønsted–Lowry acids and bases Video Lecture | Chemistry for JEE Main & Advanced
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FAQs on Brønsted–Lowry acids and bases Video Lecture - Chemistry for JEE Main & Advanced
| 1. What is the Brønsted–Lowry theory of acids and bases? |  |
Ans. The Brønsted–Lowry theory defines an acid as a substance that can donate a proton (H+) and a base as a substance that can accept a proton.
| 2. How does the Brønsted–Lowry theory differ from the Arrhenius theory of acids and bases? | |
Ans. The Brønsted–Lowry theory is more general than the Arrhenius theory as it can explain acid-base reactions in non-aqueous solvents as well. In contrast, the Arrhenius theory only applies to aqueous solutions.
| 3. Can a substance be both an acid and a base according to the Brønsted–Lowry theory? | |
Ans. Yes, according to the Brønsted–Lowry theory, a substance can act as an acid in one reaction by donating a proton and as a base in another reaction by accepting a proton.
| 4. How do conjugate acid-base pairs relate to the Brønsted–Lowry theory? | |
Ans. In the Brønsted–Lowry theory, a conjugate acid-base pair consists of two species that differ by the presence or absence of a proton. The acid donates a proton to form its conjugate base, while the base accepts a proton to form its conjugate acid.
| 5. Can you give an example of a Brønsted–Lowry acid and base? | |
Ans. An example of a Brønsted–Lowry acid is hydrochloric acid (HCl), which donates a proton to form its conjugate base, chloride ion (Cl-). An example of a Brønsted–Lowry base is ammonia (NH3), which accepts a proton to form its conjugate acid, ammonium ion (NH4+).
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Nov 24, 2024 Last updated |
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