$A g | A g {B r}_{(s)}, K B r (0.01 M) ∥ K C l (0.002 M), A g {C l}_{(s)} | {A g}_{(s)}$ . 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 $\frac{2.303 R T}{F} = 0.06$

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Solution

Given, $K_{s p} (A g C l) = 4.8 \times 10^{- 10}$
$[{C l}^{(-)}] = 0.002 M$
$∴ {[{A g}^{+}]}_{{C l}^{(-)}} = \frac{K_{s p}}{[{C l}^{(-)}]} = 2.4 \times 10^{- 7} M$
$K_{s p} [A g B r] = 2.4 \times 10^{- 14}$
$[{B r}^{-}] = 0.01 M$
${[{A g}^{+}]}_{{B r}^{-}} = 2.4 \times 10^{- 12} M$
$A g + A g C l ⟶ A g B r + A g$
$E_{c e l l} = E^{0} - \frac{0.06}{1} l o g [\frac{({A g}^{+}) B r}{({A g}^{+}) C l}]$
$E_{c e l l} = - 0.06 l o g [\frac{2.4 \times 10^{- 12}}{2.4 \times 10^{- 7}}]$
$E_{c e l l} = - 0.06 l o g [10^{- 5}]$
$E_{c e l l} = + 0.3 V$

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Similar questions

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}

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

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[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. 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)}

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?

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

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

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

The answer is -m.n

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Then n-m =

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Ag|AgBr(s),KBr(0.01M)∥KCl(0.002M),AgCl(s)|Ag(s). Calculate the EMF of given cell at 25oC:[Given: Ksp(AgCl)=4.8×10−10M2,Ksp(AgBr)=2.4×10−14M2 and 2.303RTF=0.06

Given, Ksp(AgCl)=4.8×10−10[Cl(−)]=0.002M∴[Ag+]Cl(−)=Ksp[Cl(−)]=2.4×10−7MKsp[AgBr]=2.4×10−14[Br−]=0.01M[Ag+]Br−=2.4×10−12MAg+AgCl⟶AgBr+AgEcell=E0−0.061log[(Ag+)Br(Ag+)Cl]Ecell=−0.06log[2.4×10−122.4×10−7]Ecell=−0.06log[10−5]Ecell=+0.3V

$A g | A g {B r}_{(s)}, K B r (0.01 M) ∥ K C l (0.002 M), A g {C l}_{(s)} | {A g}_{(s)}$ . 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 $\frac{2.303 R T}{F} = 0.06$