Consider the cell Ag - AgBr s Br- - AgCls Cl- - Ag at 25oC- The solubility product of AgCl and AgBr are 1 - 10-10 and 5 - 10-13 respectively- For what ratio of concentration of Br- and Cl- ions would the emf of cell be zero- give ans in1-litre

The expression for the cell potential is E=E^0 0.0592nlog[Ag^+]_L[Ag^+]_R Substitute values in the above expression 0=0 0.05921log[Ag^+]_L[Ag^+]_R Henc ...

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

Byju's Answer

Standard XII

Chemistry

Electrode Potential

Consider the ...

Question

Consider the cell $A g | A g B r (s) B r^{-} | | A g C l (s) C l^{-} | A g$ at $25^{o}$ C. The solubility product of AgCl and AgBr are $1 \times 10^{- 10}$ and $5 \times 10^{- 13}$ respectively. For what ratio of concentration of $B r^{-}$ and $C l^{-}$ ions would the emf of cell be zero? give ans in(1/litre)

Open in App

Solution

The expression for the cell potential is
$E = E^{0} - \frac{0.0592}{n} l o g \frac{[A g^{+}]_{L}}{[A g^{+}]_{R}}$
Substitute values in the above expression
$0 = 0 - \frac{0.0592}{1} l o g \frac{[A g^{+}]_{L}}{[A g^{+}]_{R}}$
Hence, $\frac{[A g^{+}]_{L}}{[A g^{+}]_{R}} = 1$
or $[A g^{+}]_{L} = [A g^{+}]_{R}$
Hence, $\frac{K_{s p, A g B r}}{[B r^{-}]} = \frac{K_{s p, A g C l}}{[C l^{-}]}$
$\frac{[C l^{-}]}{[B r^{-}]} = \frac{K_{s p, A g C l}}{K_{s p, A g B r}} = \frac{1 \times 10^{- 10}}{5 \times 10^{- 3}} = 200$

Suggest Corrections

Similar questions

Q. Consider the cell

A g (s) | A g B r (x) | B r^{-} (a q) | | C l^{-} (a q) | A g C l (s) | A g (s)

at 25

^{o}

C. The solubility product constants of

A g B r

and

A g C l

are

5 \times 10^{- 13}

and

1 \times 10^{- 10}

respectively. For what ratio of the concentrations of Br

^{-}

and Cl

^{-}

ions, would the emf of the cell be zero?

Q. Consider the cell

A g (s) | A g B r (s) | | B r^{-} (a q) | | A g C l (s) | C l^{-} (a q) | A g (s) 25^{\circ} C

.The solubility product constants of AgBr and AgCl are respectively

5 \times 10^{- 13}

and

1 \times 10^{- 10}

. For what ratio of the concentration of

B r^{-}

and

C l^{-}

ions would the emf of the cell be zero?

A g_{(s)} | A g B r_{(s)} | B r_{(0.01 M)}^{-} | | C l_{(0.2 M)}^{-} | A g C l_{(s)} | A g_{(s)}

K_{s p}

A g B r

and

A g C l

25^{\circ} C

are

10^{- 12}

and

10^{- 10}

respectively, then find which of the following option(s) is/are true for above cell at

25^{\circ} C

.
(Given :

log 2 = 0.3

)

Q. The concentration of

{A g}^{+}

ions in a given saturated solution of

A g C l

25^{0} C

1.06 \times 10^{- 5}

gm ion litre. The solubility product of

A g C l

is:

Q. Which of the following statements are true for a solution saturated with AgCl & AgBr. If their solubilities in mole/litre present in separate solutions are x & y respectively. The solubility product values of AgBr and AgCl are

5 \times 10^{- 13}

and

5 \times 10^{- 10}

respectively.

Join BYJU'S Learning Program

Consider the cell Ag|AgBr(s)Br−||AgCl(s)Cl−|Ag at 25oC. The solubility product of AgCl and AgBr are 1×10−10 and 5×10−13 respectively. For what ratio of concentration of Br− and Cl− ions would the emf of cell be zero? give ans in(1/litre)

The expression for the cell potential is E=E0−0.0592nlog[Ag+]L[Ag+]RSubstitute values in the above expression0=0−0.05921log[Ag+]L[Ag+]RHence, [Ag+]L[Ag+]R=1or [Ag+]L=[Ag+]RHence, Ksp,AgBr[Br−]=Ksp,AgCl[Cl−][Cl−][Br−]=Ksp,AgClKsp,AgBr=1×10−105×10−3=200