Bronsted-Lowry acid-base reactions are all about the transfer of protons ($H^+$). A Bronsted-Lowry acid is a proton donor, meaning it gives away a proton. A Bronsted-Lowry base is a proton acceptor, meaning it grabs a proton. When an acid donates a proton, what's left is called its conjugate base. When a base accepts a proton, it becomes its conjugate acid. Understanding these pairs is key to predicting reaction outcomes! Let's practice identifying these in different reactions.
Match the term with its correct definition:
| Term | Definition |
|---|---|
| 1. Bronsted-Lowry Acid | A. Species that accepts a proton ($H^+$) |
| 2. Bronsted-Lowry Base | B. The species formed when an acid donates a proton |
| 3. Conjugate Acid | C. Species that donates a proton ($H^+$) |
| 4. Conjugate Base | D. A substance that can act as either an acid or a base. |
| 5. Amphoteric | E. The species formed when a base accepts a proton |
Match the numbers with the corresponding letters (e.g., 1-C, 2-A, etc.)
Complete the following paragraph using the words provided below:
In a Bronsted-Lowry acid-base reaction, a(n) __________ donates a(n) __________ to a(n) __________. The substance that accepts the proton becomes the __________ __________, and the substance that donates the proton becomes the __________ __________. Water is an example of a(n) __________ substance because it can act as both an acid and a base.
Words: acid, proton, base, conjugate acid, conjugate base, amphoteric
Water ($H_2O$) can act as both an acid and a base. Write balanced chemical equations to show water acting as an acid with ammonia ($NH_3$) and as a base with hydrochloric acid ($HCl$). Indicate the conjugate acid-base pairs in each reaction.
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