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# When Ag reacts with conc. HCl, then products will be :A)${\text{AgCl,}}\,{\text{C}}{{\text{l}}_{\text{2}}}$B) ${\text{AgCl,}}\,{{\text{H}}_{\text{2}}}$C) ${\text{AgCl,}}\,{{\text{H}}_{\text{2}}},\,{\text{C}}{{\text{l}}_{\text{2}}}$D) None of these

Last updated date: 15th Aug 2024
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Hint: We know that when an acid undergoes reaction with a metal, then the formation of a salt and hydrogen gas takes place in case of all metals which are more reactive than hydrogen. In this reaction, the metal displaces the hydrogen from the acid and forms a salt. Here, we have to compare the reactivity of silver and hydrogen.

When Ag reacts with conc. HCl, then white precipitate of AgCl is formed, ${{\text{H}}_{\text{2}}}$
​ or ${{\text{Cl}}_{\text{2}}}$ is not formed as Ag is a less reactive metal.

Reduction Potential ${{\text{E}}_{{\text{Ag}}}}$= 0.8 V
Reduction Potential ${E_{{\text{Cl}}}}$= 1.36 V
Reduction Potential ${E_{{{\text{H}}_{\text{2}}}}}$= 0 V

So, Silver (Ag) cannot oxidise ${\text{C}}{{\text{l}}^ - }$ and cannot reduce ${{\text{H}}^ + }$.

So, the correct answer is Option d.

${\text{A }} + {\text{ B}} - {\text{C }} \to {\text{ A}} - {\text{C }} + {\text{ B}}$