NEET > Chemistry Class 11 > The Bronsted - Lowry Acids & Bases
The Bronsted - Lowry Acids & Bases Video Lecture - Chemistry Class 11 - NEET
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FAQs on The Bronsted - Lowry Acids & Bases Video Lecture - Chemistry Class 11 - NEET
| 1. What is the difference between a Bronsted acid and a Bronsted base? |  |
Ans. A Bronsted acid is a substance that donates a proton (H+) in a chemical reaction, while a Bronsted base is a substance that accepts a proton (H+) in a chemical reaction. In other words, an acid is a proton donor, and a base is a proton acceptor.
| 2. How does a Bronsted acid react with a Bronsted base? | |
Ans. When a Bronsted acid reacts with a Bronsted base, the acid donates a proton to the base. This forms a new bond between the acid and the base, resulting in the formation of a conjugate acid-base pair.
| 3. Can water act as both a Bronsted acid and a Bronsted base? | |
Ans. Yes, water can act as both a Bronsted acid and a Bronsted base. In a reaction, water can donate a proton to a base, making it an acid. Conversely, water can also accept a proton from an acid, making it a base. This behavior is known as amphiprotic or amphoteric.
| 4. What is the significance of the Bronsted-Lowry theory in acid-base chemistry? | |
Ans. The Bronsted-Lowry theory provides a broader definition of acids and bases compared to the earlier Arrhenius theory. It allows for the characterization of acids and bases in a wider range of solvents, not just water. This theory also emphasizes the transfer of protons in acid-base reactions, which is crucial in many chemical reactions and biological processes.
| 5. Can you give an example of a Bronsted acid-base reaction? | |
Ans. One example of a Bronsted acid-base reaction is the neutralization of hydrochloric acid (HCl) with sodium hydroxide (NaOH) to form water (H2O) and sodium chloride (NaCl). In this reaction, HCl donates a proton to NaOH, forming water and NaCl. The HCl is the Bronsted acid, and NaOH is the Bronsted base in this reaction.
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