Find the true statements regarding the aqueous dissociation of HCN- Ka - 4-9 - 10-10 at 25oC-I- At equilibrium- -H- - -CN-II- At equilibrium- -H- - -HCN-III- HCNaq is a strong acid-

The correct option is A I onlyOnly at #160; eqb ^ m we can say #160; [ H ^ + ] =[ CN ] due to very very less ionisation of HCN (Ka ...

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Standard XII

Chemistry

Arrhenius Acid

Find the true...

Question

Find the true statements regarding the aqueous dissociation of HCN, $K_{a} = 4.9 \times 10^{- 10}$ at $25^{o}$ C.
I. At equilibrium, $[H^{+}] = [C N^{-}]$
II. At equilibrium, $[H^{+}] > [H C N]$
III. $H C N (a q)$ is a strong acid.

I only

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II only

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I and II only

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II and III only

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I, II, and III

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Solution

The correct option is A I only
Only at ${e q b}^{m}$ we can say $[H^{+}] = [C N]$ due to very very less ionisation of $H C N$ $(K a <<< 1)$

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Similar questions

Q. Which of the following is/are true regarding the aqueous dissociation of

H C N

K_{a} = 4.9 \times 10^{- 10}

, at

25^{o}

C?
I. At equilibrium,

[H^{+}] = [C N^{-}]

II. At equilibrium,

[H^{+}] > [C N^{-}]

III

H C N_{(a q)}

is a strong acid

Q. Which of the following are true regarding the aqueous dissociation of HCN,

K_{a}

= 4.9 x

10^{- 10}

25^{o} C

?
i. At equilibrium,

[H^{+}] = [C N^{-}]

ii. At equilibrium,

[H^{+}]

= [HCN]
iii.

H C N

is a strong acid

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 will be:

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

If L and H divorced, then H could marry

I) D only

II) F

III) D or G

Which of the following indicates the correct order of acidic strength of the following acids.

I. HCOOH (Ka = 1.8 $\times$ $10^{- 4}$ )

II. $C H_{3} C O O H$ (Ka = 1.8 $\times$ $10^{- 5}$ )

III : HCN (Ka = 4.8 $\times$ $10^{- 10}$ )

IV: HS- (Ka = 1 $\times$ 10-14)

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Find the true statements regarding the aqueous dissociation of HCN, Ka=4.9×10−10 at 25oC.I. At equilibrium, [H+]=[CN−]II. At equilibrium, [H+]>[HCN]III. HCN(aq) is a strong acid.

The correct option is A I onlyOnly at eqbm we can say [H+]=[CN] due to very very less ionisation of HCN (Ka<<<1)

Find the true statements regarding the aqueous dissociation of HCN, $K_{a} = 4.9 \times 10^{- 10}$ at $25^{o}$ C.
I. At equilibrium, $[H^{+}] = [C N^{-}]$
II. At equilibrium, $[H^{+}] > [H C N]$
III. $H C N (a q)$ is a strong acid.

The correct option is A I only
Only at ${e q b}^{m}$ we can say $[H^{+}] = [C N]$ due to very very less ionisation of $H C N$ $(K a <<< 1)$