1. Formation of Water: The key feature of an Arrhenius acid-base reaction is the production of water as a product. This occurs through the reaction of a hydrogen ion (H+) from the acid and a hydroxide ion (OH-) from the base.

2. Acid Definition: An Arrhenius acid is defined as a substance that donates hydrogen ions (H+) when dissolved in water. Examples include hydrochloric acid (HCl), sulfuric acid (H2SO4), and nitric acid (HNO3).

3. Base Definition: An Arrhenius base is defined as a substance that donates hydroxide ions (OH-) when dissolved in water. Examples include sodium hydroxide (NaOH), potassium hydroxide (KOH), and calcium hydroxide (Ca(OH)2).

4. General Reaction: The general equation for an Arrhenius acid-base reaction is:

```

Acid + Base → Salt + Water

```

Example:

The reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) is a classic example of an Arrhenius acid-base reaction:

```

HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)

```

Limitations of the Arrhenius Theory:

While the Arrhenius theory was groundbreaking in its time, it has limitations:

* It is restricted to reactions in water: The theory doesn't explain reactions in non-aqueous solvents.

* It doesn't account for all acids and bases: There are substances that can act as acids or bases without donating H+ or OH- ions, respectively.

Broader Theories:

The Brønsted-Lowry theory and the Lewis theory of acids and bases provide a more comprehensive understanding of acid-base reactions and extend the definitions beyond the strict Arrhenius model.