key term - 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

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.