Explain Bronsted-Lowry acid base theory.

Question

Accepted Answer

>

> [!TLDR]
> Bronsted-Lowry theory: acids donate protons, bases accept protons, and every acid-base reaction generates a conjugate acid-base pair.
>
> **Statement of the theory:** According to Bronsted and Lowry, an **acid** is a substance that can **donate a proton (H+)** to another substance, and a **base** is a substance that can **accept a proton (H+)** from an acid.
>
> **Conjugate acid-base pairs:** When an acid donates a proton, what remains is its **conjugate base**; when a base accepts a proton, it becomes its **conjugate acid**. Every acid-base reaction thus involves two conjugate acid-base pairs.
>
> **Example:**
> $$\underset{	ext{acid}}{HCl} + \underset{	ext{base}}{H_2O} \longrightarrow \underset{	ext{conjugate acid}}{H_3O^+} + \underset{	ext{conjugate base}}{Cl^-}$$
>
> - HCl acts as an acid because it **donates** a proton to water.
> - H2O acts as a base because it **accepts** that proton, becoming $H_3O^+$ (its conjugate acid).
> - $Cl^-$ is the conjugate base of HCl (what remains after HCl loses its proton).
> …

Acid	Conjugate Base	Base	Conjugate Acid
$\text{HCl}$	$\text{Cl}^-$	$\text{NH}_3$	$\text{NH}_4^+$
$\text{H}_2\text{SO}_4$	$\text{HSO}_4^-$	$\text{H}_2\text{O}$	$\text{H}_3\text{O}^+$
$\text{NH}_4^+$	$\text{NH}_3$	$\text{OH}^-$	$\text{H}_2\text{O}$
$\text{H}_2\text{O}$	$\text{OH}^-$	$\text{CO}_3^{2-}$	$\text{HCO}_3^-$

Q.Explain Bronsted-Lowry acid base theory.

Concept understanding — Brønsted Lowry Conjugate Pairs

From Intuition to Precision: Brønsted–Lowry Conjugate Pairs

The Precise Statement

Seeing It in Action

A Quick Reference Table

Why This Matters …

Q.Explain Bronsted-Lowry acid base theory.

🎓Unlock everything free for 14 days

Unlock everything free for 14 days