For the reaction - Ag CN 2 - - Ag - - 2C N - the K c at 25oC is 4- 10 -19- - Ag - - in solution which was originally 0-1 M in KCN and 0-03 M in AgN O 3 is -

The correct option is A a = 7.5×10^ 18 ...

226

You visited us 226 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Van't Hoff Factor

For the react...

Question

For the reaction : $A g {(C N)}_{2}^{-} ⇌ {A g}^{+} + 2 C N^{-}$ , the $K_{c}$ at $25^{o} C$ is $4 \times 10^{- 19}$ . $[{A g}^{+}]$ in solution which was originally $0.1 M$ in $K C N$ and $0.03 M$ in $A g N O_{3}$ is :

a = 7.5 \times 10^{- 18}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

a = 4.5 \times 10^{- 18}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

a = 5.5 \times 10^{- 18}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

None of these

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A $a = 7.5 \times 10^{- 18}$

Suggest Corrections

Similar questions

Q. In a given reaction;

A g (C N)_{2}^{-} ⇌ A g^{+} + 2 C N^{-}

, the equilibrium constant at

25^{\circ} C

4.0 \times 10^{- 19}

, then the silver ion concentration in a solution which was originally

0.1 M

K C N

and

0.03 M

A g N O_{3}

is:

Q. For the reaction

A g {(C N)}_{2}^{-} ⇌ A {(g)}^{+} + 2 {C N}^{-}

, the

K_{c}

4 \times 10^{- 19}

. Calculate

[A {(g)}^{+}]

in solution which was originally 0.1 M in

K C N

and 0.03 M in

A g N O_{3}

Q. For the reaction,

{[A g {(C N)}_{2}]}^{-} ⇌ {A g}^{+} + 2 {C N}^{-}

, the equilibrium constant

K_{c}

25^{o} C

4 \times 10^{- 19}

. Then

{A g}^{+}

concentration in a solution which has

0.1 M

K C N

and

0.03 M

A g {N O}_{3}

is:

Q. For the reaction,

[A g (C N_{2})]^{-} ⇌ A g^{+} + 2 C N^{-}

the equilibrium constant at 298 K is

4.0 \times 10^{- 10}

. The silver ion concentration in a solution which was originally 0.12 molar n

K C N

and 0.04 molar in

A g N O_{3}

, is:

Q. For the reaction ;

{[A g {(C N)}_{2}]}_{2}^{-} \to A g^{+} + 2 C N^{-}

The equilibrium constant for the above reaction at

25^{\circ} C

4.0 \times 10^{- 19}

. Calculate the silver ion concentration in a solution which was originally 0.10 molar in

K C N

and 0.03 molar in

A g N O_{3}

Join BYJU'S Learning Program

For the reaction : Ag(CN)−2⇌Ag++2CN−, the Kc at 25oC is 4×10−19. [Ag+] in solution which was originally 0.1M in KCN and 0.03M in AgNO3 is :

The correct option is A a=7.5×10−18

For the reaction : $A g {(C N)}_{2}^{-} ⇌ {A g}^{+} + 2 C N^{-}$ , the $K_{c}$ at $25^{o} C$ is $4 \times 10^{- 19}$ . $[{A g}^{+}]$ in solution which was originally $0.1 M$ in $K C N$ and $0.03 M$ in $A g N O_{3}$ is :

The correct option is A $a = 7.5 \times 10^{- 18}$