Question

Which of the following is/are methods of preparation of acids?
This question has multiple correct options
A.Neutralizing a soluble acid with a soluble base (alkali)
B.Action of acidic oxides with water
C.Mixing solutions of two soluble compounds
D.Oxidation of non-metal with oxy acids

Answer 1

Hint:We can define acid as acid is any substance showing the presence of hydrogen which has the tendency of donation of proton to another substance. Acidic substance generally has a sour taste. An acid donates an ion of ${H^ + }$ and it turns blue litmus to red.

Complete answer:Neutralizing a soluble acid with soluble base would result in the formation of soluble salt. Option (A) is incorrect.
When we dissolve acidic oxide in water, we can prepare acids. Certain oxides are dissolved in water to form acids. We can call these oxides acidic oxides. For example, sulfuric acid is formed by dissolving sulfur trioxide in water. We can write the chemical equation as,
${H_2} + C{l_2}\xrightarrow{\text{electric spark}}2HCl$
Option (B) is correct.
When we mix a solution containing two soluble compounds, we get an insoluble salt as a product and the process is known as precipitation. Option (C) is incorrect.
We have to know that all non-metal produce covalent oxides with oxygen that react with water to produce acids. Most nonmetal oxides are acidic in nature and they produce oxyacids that in turn form hydronium ions in aqueous solution. We can prepare acid by oxidation of nonmetals by reacting with oxyacids. Option (D) is correct.
Hence, the correct answer are option B and D.

Note: We can prepare acids by direct combination of elements. For example, when hydrogen and reacts with each other hydrogen chloride is formed that is absorbed in water to form hydrochloric acid. We can write the chemical equation as,
${H_2} + C{l_2}\xrightarrow{{electric\,spark}}2HCl$
We can also prepare acids by displacement of weaker or more volatile acid from its salt in the presence of stronger (or) less volatile acid. For example,
$NaCl\left( s \right) + {H_2}S{O_4}\left( {aq} \right) \to NaHS{O_4}\left( {aq} \right) + HCl\left( {aq} \right)$
When insoluble sulfide is displaced from a metallic salt by hydrogen sulfide, we obtain acids. For example,
$Pb{\left( {{C_2}{H_3}{O_2}} \right)_2}\left( {aq} \right) + {H_2}S\left( g \right) \to PbS\left( s \right) + C{H_3}COOH\left( {aq} \right)$.