Question

Generally metals react with acids to give salt and hydrogen gas. Which of the following acids does not give hydrogen gas on reacting with metals (except Mn and Mg)?
A. ${H_2}S{O_4}$
B. $HCl$
C. $HN{O_3}$
D. All the above

Answer 1

Hint: Chemical properties of acids mentioned in the question can be used to find the correct answer. For example nitric acid is a strong oxidizing agent that uses the properties to find the correct option.

Complete answer:
Nitric acid reacts with most metals but is dependent on the metal's acidity and nature. Dilute nitric acid in its reaction to most metals acts like a normal acid for example during reaction with Magnesium, manganese and zinc ${H_2}$ liberates but for reaction with other metals it releases other oxides of nitrogen because nitric acid is a strong oxidizing agent so, as soon as hydrogen gas is formed in the reaction between the metal and dilute $HN{O_3}$, and in the reaction $HN{O_3}$ oxidizes this hydrogen to water.
$Mg + 2HN{O_3} \to Mg{\left( {N{O_3}} \right)_2} + {H_2}$

Hence, option C is the correct option.

Note: In the given above conversation $HCl$ and ${H_2}S{O_4}$ shows different chemical properties like;
Diluted sulfuric acid reacts with several metals as with other traditional acids through a single displacement reaction, creating hydrogen gas and salts (the metal sulfate). It attacks reactive metals such as iron, aluminum, zinc, manganese, magnesium, and nickel at positions above copper in the reactivity series.
$Fe + {H_2}S{O_4} \to {H_2} + FeS{O_4}$
Acids like hydrochloric acid react with metal to form salt and hydrogen gas, metals are more active than acids and can go under a single displacement reaction $Zn + 2HCl \to ZnC{l_2} + {H_2}$.