$H C l (a q) + Z n (s) \to Z n {C l}_{2} (a q) + H_{2} (g)$
In the reaction above, which term best describes the role of $H C l (a q)$ ?

Bronsted acid

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Oxidizing agent

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Reducing agent

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Precipitate

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Cathode

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Solution

The correct option is B Oxidizing agent
Option B is the correct answer.
In the left-hand side of the equation, $Z n$ has an oxidation number of $0$ (since it is in elementary form). In the right-hand side, $Z n$ has an oxidation number of $+ 2$ . (Because in $Z n C l_{2}$ each Chlorine atom has an oxidation number of $- 1$ , thus $Z n$ will have an oxidation number of $+ 2$ , to make the molecule neutral). Hence, $Z n$ gets oxidised from $0$ to $+ 2$ .
Thus $H C l$ is acting as the oxidizing agent. It itself gets reduced but oxidizes $Z n$ from $0$ to $+ 2$ .

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