Correct arrangement of the following acids in correct $K_{3}$ order is :
$(I) H 3 N^{⨁} C H_{2} C O O H (I I) N C C H 2 C O O H (I I I) H_{3} C C H_{2} C O O H (I V) ⊝ O O C C H_{2} C O O H$

I > II > III > IV

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II > I > III > IV

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I > III > II > IV

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IV > III > II > I

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Solution

The correct option is A I > II > III > IV
$H_{3} N^{+} C H_{2} C O O H$ is positive charged ion tend to release $H^{+}$ and accept negative charge, similarly $^{-} O O C C H_{2} C O O H$ has negative charge and do not tend to accept the other negative charge. The electron density of $- O H$ in $C H_{3} - C H_{2} - C O O H$ increases and $H^{+}$ becomes more difficult to donate. Electron-releasing groups reduce acidity of a carboxylic acid. $N C C H_{2} C O O H$ has $C N$ electron withdrawing group. therefore the order of acidic strength is $I > I I > I I I > I V$

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Similar questions

C H \equiv C - C O O H; C H_{2} = C H - C O O H; C H_{3} C H_{2} C O O H

In the following molecules:
$C H_{3} B r, C H_{3} F, C H_{3} C l, C H_{3} I I, I I, I I I, I V$
The correct order of dipole moment will be:

K_{2} C O_{3} (I), M g C O_{3} (I I), C a C O_{3} (I I I), B e C O_{3} (I V)

In the following molecules:
$B F_{3}, B C l_{3}, B B r_{3}, B I_{3} I, I I, I I I, I V$
The correct order of Lewis acidic strength will be:

I . Z n O

I I . K_{2} O

I I I . P_{2} O_{5}

I V . M g O

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