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Bronsted Lowry Theory

HS-+OH-→ S2-+...

Question

$H S^{-} + O H^{-} \to S^{2 -} + H_{2} O$
In the system indicated by the equation above, brosnted acids are:

A

H S^{-} a n d H_{2} O

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B

H S^{-} a n d S^{2 -}

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C

H S^{-} a n d O H^{-}

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D

S^{2 -} a n d H_{2} O

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E

O H^{-} a n d H_{2} O

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Solution

The correct option is A $H S^{-} a n d H_{2} O$
Since bronsted acids, are proton donors, So ${H S}^{-}$ and $H_{2} O$ can act as acids
to give proton as $(S^{2 -} + H^{+})$ and $({O H}^{-} + H^{+})$ respectively.

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Similar questions

H_{2} O (l) + S^{2 -} ⇌ {H S}^{-} + {O H}^{-}

In the equation for the reaction represented above, the species acting as acids (proton donors) are:

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

K_{a 1}, K_{a 2}

K_{a 3}

are the respective ionisation constants for the following reactions;

H_{2} S ⇌ H^{+} H S^{-}

H S^{-} ⇌ H^{+} S^{2 -}

H_{2} S ⇌ 2 H^{+} S^{2 -}

The correct relationship between

K_{a 1}, K_{a 2}

K_{a 3}

State True or False.

S^{2 -}

is the conjugate base of

H S^{-}

.

N H_{3}, B e C l_{2}, C O_{2}, a n d H_{2} O,

the nonlinear molecules are :

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Bronsted Lowry Theory

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