If K sp AgCl -10-12 K sp AgBr -10-15- then the emf of the cell Ag s - AgBr s - Br 0-4 M - Cl 2 M - AgCl s - Ag s isA- 0 VB- 0-04135 VC- Data insufficientD- 0-136 V

The correct option is D 0.136 VAgCl(s) nbsp;K_sp=10^ 12⇌ Ag^+ (aq) + Cl^ (aq) when [Cl^ ] = 2M, Ag^+ = 10^ 122M AgBr(s) nbsp;K_sp=10^ 15⇌ Ag^+ (aq) + Br^ ...

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Electrochemical Cells, Galvanic Cells

If K sp AgCl ...

Question

If $K_{s p} (A g C l) = 10^{- 12} K_{s p} (A g B r) = 10^{- 15}$ , then the emf of the cell $A g_{(s)} | A g B r_{(s)} | B r_{0.4 M}^{-} | | C l_{2 M}^{-} | A g C l_{(s)} | A g_{(s)}$ is

0 V

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

0.136 V

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

0.04135 V

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

Data insufficient

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

Open in App

Solution

The correct option is B $0.136 V$
$A g C l (s) K_{s p} = 10^{- 12} ⇌ A g^{+} (a q) + C l^{-} (a q)$
when $[C l^{-}] = 2 M, A g^{+} = \frac{10^{- 12}}{2} M$
$A g B r (s) K_{s p} = 10^{- 15} ⇌ A g^{+} (a q) + B r^{-} (a q)$
when $[B r^{-}] = 0.4 M, A g^{+} = \frac{10^{- 15}}{0.4} M$
For cell reaction $A g_{(s)} | A g B r_{(s)} | B r_{(0.4 M)}^{-} | | C l_{(2 M)}^{-} | A g C l_{(s)} | A g_{(s)}$
Which is equivalent to $A g_{(s)} | A g_{\frac{10^{- 15}}{0.4}}^{+} | | A g_{\frac{10^{- 12}}{2}}^{+} | A g_{(s)}$
So cell reaction $A g_{(s)} + A g_{(\frac{10^{- 12}}{2})}^{+} \to A g_{(\frac{10^{- 15}}{0.4})}^{+} + A g_{(s)}$ which concentration cell
$E_{c e l l} = E_{c e l l}^{o} - \frac{0.0591}{n} l o g Q_{c} = 0 - \frac{0.0591}{1} l o g \frac{\frac{10^{- 15}}{0.4}}{\frac{10^{- 12}}{2}} = 0.0591 l o g \frac{10^{- 2}}{2}$
$E_{c e l l} = 0.136 V$

Suggest Corrections

Similar questions

A g | A g {B r}_{(s)}, K B r (0.01 M) ∥ K C l (0.002 M), A g {C l}_{(s)} | {A g}_{(s)}

. Calculate the EMF of given cell at

25^{o} C

:
[Given:

K_{s p (A g C l)} = 4.8 \times 10^{- 10} M^{2}, K_{s p (A g B r)} = 2.4 \times 10^{- 14} M^{2}

and

\frac{2.303 R T}{F} = 0.06

Q. For the galvanic cell,

A g | A g C l (s), K C l (0.2 M) | | K B r (0.001 M), A g B r (s) | A g

Calculate the emf generated and assign correct polarity to each electrode for a spontaneous process after taking into account the cell reaction at

25^{0} C

[K_{s p} (A g C l) = 2.8 \times 10^{- 10}, K_{s p} (A g B r) = 3.3 \times 10^{- 13}]

Q. For the galvanic cell,

A g | A g C l (s), K C l (0.2 M) | | K B r (0.001 M), A g B r (s) | A g

Calculate the emf generated and assign correct polarity to each electrode for the spontaneous process after taking into account the cell reaction at

25^{\circ} C

.
Given,

K_{s p A g C l} = 2.8 \times 10^{- 10}; K_{s p A g B r} = 3.3 \times 10^{- 13}

For the galvanic cell :

Ag 1 AgCl(s), KCl(0.2 M)II KBr (0.001 M), AgBr(s) I Ag, the EMF (in V) generated for a spontaneous process after taking into account the cell reaction at $25^{\circ} C$ will be $37 \times 10^{- x}$ , then what is the value of x?