Question

What is the formula of the conjugate base of HS?

Answer 1

Hint: We know that the Bronsted Lowry theory of acid and base. According to this theory an acid is a proton donor while the base is a proton acceptor. the proton is represented by the symbol ${{H}^{+}}$and we know that conjugated acid is a cation and conjugate base is an anion.

Complete answer:
The Bronsted 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 called Bronsted 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 base which bonds to hydrogen ion.
Now we see conjugated acid, according to the Bronsted Lowry theory the conjugate acid is the chemical species which is formed after the base accepts the hydrogen atom is called conjugated acid.
Acid + Base$\rightleftharpoons $Conjugate Base + Conjugate Acid.
To find the conjugate base of any acid , simply remove H$^{+}$ from the acid .
Now we apply the Bronsted Lowry theory in our question:(removing hydrogen atom)
 $HS\rightleftharpoons {{H}^{+}}+{{S}^{-}}$
In the above reaction ${{S}^{-}}$ the Bronsted Lowry base which accepts hydrogen atom from its conjugate acid $HS$.

Note:
we must know that a conjugate acid contains one hydrogen atom in addition and positive charge than the base from which it is formed. A conjugate base has one hydrogen atom less and negative charge than the acid from which it is formed and then you can easily conjugate. For example: carbonic acid and hydronium ions are formed by the reaction of bicarbonates ions with the water.