Brønsted-Lowry base

Definition

A Brønsted-Lowry base is a substance that can accept a proton (hydrogen ion, $H^+$) from another substance. It plays a crucial role in acid-base reactions by undergoing protonation.

5 Must Know Facts For Your Next Test

1. Brønsted-Lowry bases are proton acceptors.
2. When a Brønsted-Lowry base gains a proton, it becomes its conjugate acid.
3. Common examples of Brønsted-Lowry bases include hydroxide ions ($OH^-$), ammonia ($NH_3$), and water ($H_2O$).
4. The strength of a Brønsted-Lowry base is determined by its tendency to accept protons.
5. In aqueous solutions, the presence of more basic species shifts equilibrium towards the formation of more water.

Review Questions

• What defines a substance as a Brønsted-Lowry base?
• Provide an example of a common Brønsted-Lowry base and its conjugate acid.
• How does the presence of a strong Brønsted-Lowry base affect equilibrium in an aqueous solution?

Related terms

Brønsted-Lowry Acid: A substance that donates a proton (hydrogen ion, $H^+$) to another substance.

Conjugate Acid-Base Pair: A pair consisting of an acid and its conjugate base or a base and its conjugate acid, differing by one $H^+$ ion.

$pK_b$: $pK_b$ is the negative logarithm of the base dissociation constant ($K_b$), indicating the strength of a Brønsted-Lowry base.