How does the Arrhenius model of Acids and Bases differ from the Bronsted-Lowry model?

1. The Arrhenius Model: This model was proposed by Svante Arrhenius in 1884. According to this model, an acid is a substance that increases the concentration of hydrogen ions (H+) when dissolved in water, while a base is a substance that increases the concentration of hydroxide ions (OH-) when dissolved in water. This model is limited to aqueous solutions and does not explain the behavior of acids and bases in non-aqueous solvents.

2. The Bronsted-Lowry Model: This model was proposed by Johannes Bronsted and Thomas Lowry in 1923. According to this model, an acid is a substance that can donate a proton (H+), and a base is a substance that can accept a proton. This model is more general than the Arrhenius model as it can explain the behavior of acids and bases in both aqueous and non-aqueous solvents.

In summary, the main difference between the two models is that the Arrhenius model defines acids and bases in terms of the ions they produce in water, while the Bronsted-Lowry model defines them in terms of their ability to donate or accept protons.