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Arrhenius Acid

Conjugate bas...

Question

Conjugate base of $H C l$ in the following reaction is:
$H C l (a q) + H_{2} O \to C l^{-} (a q) + H_{3} O^{+}$ .

A

H_{3} O^{+}

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B

H_{2} O

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C

C l^{-}

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D

HCl

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Solution

The correct option is C $C l^{-}$
Hydrochloric acid, HCl, starts with a proton that ends up on a water molecule, which acts as a Bronsted - Lowry base and forms hydronium ions.

HCl is a strong acid. When it donates a proton, a Cl– ion is produced, and so Cl– is the conjugate base.

Hence, option $C$ is correct.

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Similar questions

Q. Identify the correct statement(s) for the given reaction.

H C l + H_{2} O \to H_{3} O^{+} + C l^{-}

a) Conjugate base of

H C l

C l^{-}

b) Conjugate acid-base pair is

H_{3} O^{+}

H_{2} O

c) Conjugate base of

H_{2} O

H_{3} O^{+}

d) Conjugate acid-base pair is

H C l

H_{3} O^{+}

Q. For the reaction given below, identify the correct statement(s):

H C l + H_{2} O \to H_{3} O^{+} + C l^{-}

Q. If we add 1*10^-8of HCl into pure water in the following reaction:
HCl (aq) + H₂O (l) to give H₃O⁺ (aq) + Cl^- (aq)
and assuming that volume doesn't change when HCl is added, why is H₃O⁺= HCl = 10^-8? Shouldn't it be H₃O⁺+ HCl = 10^-8 because HCl is dissolved with water?

Q. Which choice or choices demonstrate amphoterism?
i.

H C l + H_{2} O \to H_{3} O^{+} + C l^{-}

H_{2} O + N_{3} \to O H^{-} + N H_{4}^{-}

H S^{-} + H C l \to C l^{-} + H_{2} S

H S^{-} + N H_{3} \to N H_{4}^{+} + S^{2 -}

H C l + N a O H \to N a C l + H_{2} O

N a C l + H_{2} O \to H C l + N a O H

Q. In a reaction :

H C O_{3}^{-} + H_{2} O \to C O_{3}^{2 -} + H_{3} O^{+}

H C O_{3}^{-}

is the conjugate acid of which Bronsted base ?

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