Cl – is the conjugate base of — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

# Conjugate Base of Cl⁻ **Step 1: Understand conjugate base definition** A conjugate base is formed when an acid donates a proton ($H^+$). It's the species left after $H^+$ removal. **Step 2: Work backwards from $Cl^-$** If $Cl^-$ is the conjugate base, then its conjugate acid must be the species that, when it loses one $H^+$, produces $Cl^-$: $$\text{Conjugate acid} \rightarrow Cl^- + H^+$$ **Step 3: Identify the conjugate acid** The conjugate acid of $Cl^-$ is **$HCl$** (hydrochloric acid): $$HCl \rightarrow Cl^- + H^+$$ **Therefore, $Cl^-$ is the conjugate base of $HCl$** (option B) --- **Note:** If other options included species like $HClO$, $HClO_2$, etc., those would be *different* acids with different conjugate bases ($ClO^-$, $ClO_2^-$, etc.). Only $HCl$ directly produces $Cl^-$ upon losing a proton.