What is the Difference Between Amphiprotic and Amphoteric?

The terms amphiprotic and amphoteric are often used interchangeably, but they have different meanings. Here are the key differences between the two:

• Amphiprotic: Amphiprotic substances are those that can both donate and accept protons depending on the conditions. They are Brønsted-Lowry acids and bases, meaning they can act as either an acid or a base depending on the specific situation. Examples of amphiprotic substances include water, acetic acid, and bicarbonate ions.
• Amphoteric: Amphoteric substances are those that can act both as an acid and as a base. This term is more general and does not require a substance to accept and donate protons. Examples of amphoteric substances include water, some oxides and hydroxides, and some salts.

In summary, all amphiprotic substances are amphoteric because they can act as both an acid and a base. However, not all amphoteric substances are amphiprotic, as amphoteric substances do not necessarily need to accept and donate protons.

Comparative Table: Amphiprotic vs Amphoteric

The main difference between amphiprotic and amphoteric substances lies in their ability to donate or accept protons and their overall behavior as acids or bases. Here is a summary of their differences:

Examples of amphiprotic substances include water and hydrogen sulfide, while examples of amphoteric substances include aluminum hydroxide and beryllium hydroxide.