The Bronsted-Lowry theory helps us understand acids and bases and how strong they are.

According to this theory:

• An acid is something that gives away protons (H⁺).
• A base is something that takes in protons.

This idea of transferring protons helps us figure out if an acid or base is strong or weak.

Key Points to Remember:

1. Strength of Acids and Bases:

   • Strong acids, like hydrochloric acid (HCl), break apart completely in water and give off all their protons.
   • Weak acids, such as acetic acid (CH₃COOH), do not break apart completely and give off only some of their protons.

2. Equilibrium Constant:

   • The strength of an acid can also be measured with something called the acid dissociation constant ($K_a$).
   • A larger $K_a$ value means a stronger acid because it shows there are more H⁺ ions in the solution.

3. Example:

   • Take sulfuric acid (H₂SO₄) as an example of a strong acid.
   • It easily donates H⁺ ions, which makes it a strong proton donor.

In short, the Bronsted-Lowry theory lets us predict how strong an acid or base is by looking at how well they donate or accept protons and checking their dissociation constants.