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Standard XII

Chemistry

Arrhenius Acid

Given below a...

Question

Given below are the dissociation constant values of few acids. Arrange them in order of increasing acidic strength.
$H_{2} S O_{3} = 1.3 \times 10^{- 2}, H N O_{2} = 4 \times 10^{- 4}$
$C H_{3} C O O H = 1.8 \times 10^{- 5}, H C N = 4 \times 10^{- 10}$

H C N < C H_{3} C O O H < H N O_{2} < H_{2} S O_{3}

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C H_{3} C O O H < H N O_{2} < H C N < H_{2} S O_{3}

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C H_{3} C O O H < H C N < H_{2} S O_{3} < H N O_{2}

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H N O_{2} < H_{2} S O_{3} < C H_{3} C O O H < H C N

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Solution

The correct option is D $H C N < C H_{3} C O O H < H N O_{2} < H_{2} S O_{3}$
Higher the $K_{a}$ value higher will be the acidic strength.
The correct order is represented by option A.

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Similar questions

Q. Calculate

[H^{+}]

of solution obtained by mixing equal volume of 0.02 M

H N O_{2}

( a weak acid) and 0.2 M

C H_{3} C O O H

solution.
Given that:

K_{a_{1}} (H N O_{2}) = 2 \times 10^{- 4}

K_{a_{2}} (C H_{3} C O O H) = 2 \times 10^{- 5}

Where ,

K_{a_{1}} a n d K_{a_{2}}

are the dissociation constants of

H N O_{2} a n d C H_{3} C O O H

respectively.

K_{a}

for

H C N

and

{C H}_{3} C O O H

are

4.9 \times 10^{- 10}

and

1.8 \times 10^{- 5}

respectively. Calculate the equilibrium constant for the reaction:

{C H}_{3} C O O H + N a C N ⇌ {C H}_{3} C O O N a + H C N

The heats of neutralisation of $C H_{3} C O O H$ , HCOOH, HCN and $H_{2} S$ are -12.8, -13.2, -3.2 and -3.9 kcal per equivalent. Arrange these acids in increasing order of strength.

Q. The dissociation constants for acetic acid and HCN at

25^{o} C

are

1.5 \times 10^{- 5}

and

4.5 \times 10^{- 10}

, respectively. The equilibrium constant for the equilibrium

C N^{-} + C H_{3} C O O H ⇌ H C N + C H_{3} C O O^{-}

would be:

Enthalpy of hydrogenation is the enthalpy change when one mole of unsaturated compound is converted to saturated compound. $Δ_{H} h y d r o g e n a t i o n$ helps to calculate resonance energy.

The heat of neutralization of $C H_{3} C O O H, H C O O H, H C N$ and $H_{2} S$ are -12.8, -13.2, -3.2 and -3.9 Kcal per equivalent. Arrange these acids in increasing order of strength.

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Given below are the dissociation constant values of few acids. Arrange them in order of increasing acidic strength.H2SO3=1.3×10−2,HNO2=4×10−4CH3COOH=1.8×10−5,HCN=4×10−10

The correct option is D HCN<CH3COOH<HNO2<H2SO3Higher the Ka value higher will be the acidic strength.The correct order is represented by option A.

Given below are the dissociation constant values of few acids. Arrange them in order of increasing acidic strength.
$H_{2} S O_{3} = 1.3 \times 10^{- 2}, H N O_{2} = 4 \times 10^{- 4}$
$C H_{3} C O O H = 1.8 \times 10^{- 5}, H C N = 4 \times 10^{- 10}$

The correct option is D $H C N < C H_{3} C O O H < H N O_{2} < H_{2} S O_{3}$
Higher the $K_{a}$ value higher will be the acidic strength.
The correct order is represented by option A.