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Lesson: Chapter - 6

The Chemistry of Acids and Bases

Acid-Base Theories

Let’s start our discussion of acids and bases by defining some terms that are essential to the topics that follow.

Arrhenius acids and bases are:

acid—a substance that increases the concentration of protons (H+) in water

base—a substance that increases the concentration of hydroxide ions in water (OH-)

These definitions are limited to aqueous solutions.

Brønsted and Lowry acids and bases as:

acid—a substance that donates a proton to another substance

base—a substance that accepts a proton

These definitions can also apply to reactions that are not aqueous, so they are more accurate.

Lewis acids and bases are:

acid—a substance that accepts an electron pair

base—a substance that donates an electron pair

Here are some other terms that you’ll need to be familiar with:

hydronium (H3O+)—H+ riding “piggyback” on a water molecule; water is polar, and the positive charge of the naked proton is greatly attracted to one of the negative electron pairs on adjacent oxygen

monoprotic—describes acids that can donate one H+

diprotic—describes acids that can donate two H+ ions

polyprotic—describes acids that can donate more than one H+ion

amphiprotic—describes a substance that can act as either an acid or a base. This means it can either lose a proton or gain one. Water is amphiprotic: it can form either a hydroxide ion or a hydronium ion. Other examples of amphiprotic substances are

Next to display next topic in the chapter.

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