Sure, let's identify the acids and bases in the given chemical equation using the Brønsted-Lowry definition of acids and bases. Here's the equation:
[tex]$HCl + C_5H_5N \rightleftharpoons Cl^- + HC_5H_5N^+$[/tex]
1. [tex]$HCl$[/tex] (Hydrochloric acid):
- HCl donates a proton (H⁺), so it acts as an acid.
2. [tex]$C_5H_5N$[/tex] (Pyridine):
- C_5H_5N accepts a proton (H⁺) from HCl, so it acts as a base.
3. [tex]$Cl^- (Chloride ion):
- Cl^- is the ion that remains after HCl donates a proton, so it acts as a conjugate base.
4. $[/tex]HC_5H_5N^+[tex]$ (Pyridinium ion):
- HC_5H_5N^+ forms when C_5H_5N accepts a proton, making it a conjugate acid.
Now we'll place the labels on the equation:
$[/tex][tex]$HCl + C_5H_5N \rightleftharpoons Cl^- + HC_5H_5N^+$[/tex][tex]$
$[/tex][tex]$\text{acid} \quad \text{base} \quad \square \quad \square \quad$[/tex][tex]$
$[/tex][tex]$\square \quad \square \quad \text{base} \quad \text{acid}$[/tex][tex]$
So, the completed labeling is:
$[/tex][tex]$\text{acid} \quad \text{base} \quad \text{base} \quad \text{acid} \quad$[/tex][tex]$
Thus, for the equation:
$[/tex][tex]$\text{HCl} + \text{C}_5\text{H}_5\text{N} \rightleftharpoons \text{Cl}^- + \text{HC}_5\text{H}_5\text{N}^+$[/tex]$
- HCl is the acid.
- C_5H_5N is the base.
- Cl^- is the conjugate base.
- HC_5H_5N^+ is the conjugate acid.
