Write the conjugate acid and conjugate base of each of the following: (a) OH- (b) H2O (c) HCO3- (d) H2O2

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> [!TLDR]
> The conjugate acid of a species is formed by adding one $H^+$ to it; the conjugate base is formed by removing one $H^+$ from it (Brønsted–Lowry theory).
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> By the Brønsted–Lowry definition, an acid is a proton ($H^+$) donor and a base is a proton acceptor. For any species $X$: its **conjugate acid** is $X + H^+$, and its **conjugate base** is $X - H^+$.
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> **(a) $OH^-$:**
> - Conjugate acid (add $H^+$): $OH^- + H^+ \rightarrow H_2O$
> - Conjugate base (remove $H^+$): $OH^- \rightarrow O^{2-} + H^+$
>
> **(b) $H_2O$:**
> - Conjugate acid: $H_2O + H^+ \rightarrow H_3O^+$
> - Conjugate base: $H_2O \rightarrow OH^- + H^+$
>
> **(c) $HCO_3^-$ (bicarbonate):**
> - Conjugate acid: $HCO_3^- + H^+ \rightarrow H_2CO_3$
> - Conjugate base: $HCO_3^- \rightarrow CO_3^{2-} + H^+$
> …

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.Write the conjugate acid and conjugate base of each of the following:

Concept understanding — Brønsted Lowry Conjugate Pairs

From Intuition to Precision: Brønsted–Lowry Conjugate Pairs

The Precise Statement

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A Quick Reference Table

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Q.Write the conjugate acid and conjugate base of each of the following:

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