Which reaction is not possible for acetic anhydride ?

(C H_{3} O | | C)_{2} O + 2 H N (C H_{3})_{2} \to O | | C H_{3} C N (C H_{3})_{2} + C H_{3} C O_{2}^{-} + H_{2} + N (C H_{3})_{2}

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(C H_{3} O | | C)_{2} O + C H_{3} C H_{2} O H \to O | | C H_{3} C O (C H_{2})_{3} + C H_{3} C O_{2} H

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(C H_{3} O | | C)_{2} O + C_{6} O_{6} A l C_{3} - -- \to C H_{3} O | | C C_{6} H_{5} + C H_{3} C O_{2} H

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(C H_{3} O | | C)_{2} O + N a C l \to C H_{3} O | | C C l + C H_{3} C O_{2}^{-} N a^{+}

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Solution

The correct option is D $(C H_{3} O | | C)_{2} O + N a C l \to C H_{3} O | | C C l + C H_{3} C O_{2}^{-} N a^{+}$
There is no chance of a reaction taking place between acetic acid and common salt even at high temperatures.
$N a C l$ is a salt of the strong acid, hydrochloric acid, and acetic acid is quite a weaker acid.
A weaker acid does not displace a stronger acid from the latter's salt. So you only get a homogeneous clear mixture of acetic acid and $N a C l$ , when you mix them.

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Similar questions

\to

C H_{3} O | | C) O C H C H_{3} 1

C H_{3} O | | C C l 2

C H_{3} O | | C N H C H_{3} 3

C H_{3} O ∥ C C H_{3}

C H_{3} O ∥ C O H

C H_{3} O ∥ C C H_{3} I_{2} / N a O H - ----- \to △, H^{+}

C H_{3} O ∥ C C H_{3} C r_{2} O_{7}^{2 -} / H^{+} - ------ \to

C H_{3} O ∥ C C H_{3} A g (N H_{3})_{2}^{+} - ----- \to

Arrange in decreasing order of basicity,

$H_{2} O, O H^{-}, C H_{3} O H, C H_{3} O^{-}$

C H_{3} C | | O - O^{-}

C H_{3} O^{-}

C N^{-}

C H_{3} N H_{2}

C_{6} H_{5} C H_{2} N H_{2}

p - C H_{3} O - C_{6} H_{4} - N H_{2}

m - C H_{3} O - C_{6} H_{4} - N H_{2}

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