Question

What is the conjugate acid of $H{{S}^{-1}}$ ?

Answer 1

Hint : We know that the Brønsted-Lowry theory of acid and base. According to Brønsted Lowry acid base theory, acid is a proton donor and base is a proton acceptor. When an acid loses a proton, a conjugate base is obtained. When a base accepts a proton, a conjugate acid is obtained.

Complete Step By Step Answer:
The Brønsted-Lowry theory is based on an acid and base reaction. We know that, an acid is a species which has the capacity of donating a proton that is hydrogen ion is called Brønsted-Lowry acid and a base is species which has the capacity of accepting proton and a base it needs to have a lone pair of electrons on the base which bonds to the hydrogen ion.
Now, we see Conjugate acid. According to Brønsted-Lowry theory the conjugate acid is the chemical species which is formed after the base accepts the hydrogen atom is called conjugate acid.
$Acid\text{ }+\text{ }Base\text{ }\text{ }Conjugate\text{ }Base\text{ }+\text{ }Conjugate\text{ }Acid.$
Apply the Brønsted-Lowry theory to find the conjugate acid $H{{S}^{-1}}$ . Hydrogen sulfuric acid dissociated into hydrogen sulfate ion. The conjugate acid of the hydrogen sulfate ion is the hydrogen sulfuric acid.
$HS_{(aq)}^{-1}+{{H}_{2}}{{O}_{(l)}}\rightleftharpoons {{H}_{2}}{{S}_{(aq)}}+OH_{(aq)}^{-}$
Hydrosulphuric acid is the conjugate acid of the hydrogen sulfite ion it dissociates into in solution. A conjugate acid is merely connected to the base in question. We know acids have an ${{H}^{+}}$ ion that they lose upon dissociation.

Note :
Remember that Brønsted Lowry acid base theory is similar to Arrhenius concept of acid and base. The Arrhenius concept is limited to aqueous solutions. However, Brønsted Lowry theory can also be applied to no aqueous solutions. In Arrhenius theory, a base gives a hydroxide ion. In Brønsted Lowry theory, a base accepts a proton.