Question

According to Arrhenius theory, acids are those compounds which give
a.) Oxygen ions
b.) Hydrogen ions
c.) Hydroxide ions
d.) None of these

Answer 1

Hint: Arrhenius theory was first introduced by the Swedish scientist Svante Arrhenius in the year 1887. He introduced the well-known theory of “Electronic dissociation”.

Complete step by step answer:
Let us look at Arrhenius ' theory.
According to Arrhenius theory, acid is a substance that gives ${{\text{H}}^{\text{ + }}}$ ion on dissolving in aqueous solution. It increases the concentration of ${{\text{H}}^{\text{ + }}}$ ions in the solution. The base is a substance that ionizes ${\text{O}}{{\text{H}}^{\text{ - }}}$ ions by dissolving in the aqueous solution. The concentration of ${\text{O}}{{\text{H}}^{\text{ - }}}$ ions is high in the solution. So, acids are those compounds which give ${{\text{H}}^{\text{ + }}}$ions. Therefore, the correct option for this question is option (b).

Additional Information:
We know that acids are those substances whose pH is less than 7.
Also, acids will turn blue litmus paper to red.
Arrhenius theory is only applicable only in aqueous solution, for example, according to the Arrhenius theory, HCl is an acid in the aqueous solution but not in benzene, even though it donates ${{\text{H}}^{\text{ + }}}$ ion to the benzene. Also, under Arrhenius’s definition, the solution of sodium amide in liquid ammonia is not alkaline, even though amide ion deprotonates the ammonia.
So, for the acidic and basic properties, the presence of water is necessary.
This theory does not explain acidic and basic character of substances in non-aqueous solvents.

Note: There are different theories for acids and bases. The Bronsted-Lowry theory and Lewis theory are the theories explaining acids and bases. According to Bronsted-Lowry theory, acids defined as a proton donor and base as a proton acceptor and Lewis theory defined an acid as a compound that can accept a pair of electrons and base can donate a pair of electrons.