Question

2. Provide a definition for a Bronstead-Lowry Acid and a Bronstead-Lowry Base. How are these different from Arrhenius Acids and Bases?

Answer 1

Explanation:

According to the Bronsted Lowry conjugate acid-base theory:

• An acid is defined as a substance which donates protons and forms conjugate base.

$HA\rightarrow H^++A^-$

• A base is defined as a substance which accepts protons and forms conjugate acid.

$BOH+H_2O\rightarrow (BOH_2)^{+}+OH^-$

According to Arrhenius concept:

• A base is defined as a substance which donates hydroxide ions $(OH^-)$ when dissolved in water.
• An acid is defined as a substance which donates hydronium ions $(H_3O^+)$ in water.