Home
Class 12
CHEMISTRY
Consider the cell Ag|AgBr(s)Br^(-)||AgCl...

Consider the cell `Ag|AgBr(s)Br^(-)||AgCl(s)Cl^(-)|Ag` at 298 K the solubility product of AgCl and AgBr are `1xx10^(-10)` and `5xx10^(-13)` respectively. What should be the ratio of concentration of `Br^(-)` and `Cl^(-)` by which emf of the cell becomes zero?

A

200

B

`(1)/(200)`

C

`(1)/(300)`

D

none of these

Text Solution

Verified by Experts

The correct Answer is:
B
let x and y are the concentration of `Br^(-)` and `Cl^(-)` at equilibrium when `E_(cell)=0`
`therefore[Ag^(+)]_(LHS)=(K_(sp)(ArBr))/([Br^(-)])=(5xx10^(-13))/(x)`
`[Ag^(+)]_(RHS)=(K_(sp)(AgCl))/([Cl^(-)])=(1xx10^(-10))/(y)`
Also `E_(cell)=E_(Ag//Ag^(+))^(@)(RHS)+E_(Ag//Ag^(+))^(@)(LHS)+(0.0591)/(1)log(([Ag^(+)]_(RHS))/([Ag^(+)]_(LHS)))`
`0=0+(0.0591)/(1)log((1xx10^(-10)xx x)/(5xx10^(-13)xxy))`
`therefore(x)/(y)=(1)/(200)`
Promotional Banner

Topper's Solved these Questions

  • STOICHIOMETRY AND BALANCING REDOX REACTION

    FIITJEE|Exercise SINGLE INTEGER ANSWER TYPE QUESTIONS|5 Videos

  • THERMODYNAMICS AND THERMOCHEMISTRY

    FIITJEE|Exercise SINGLE INTEGER ANSWER TYPE QUESTIONS|5 Videos

Similar Questions

Explore conceptually related problems

Consider the cell AG|AgBr(s)|Br^(-)||AgCI(s)|CI^(-)|Ag at 25^(@)C . The solubility product constants of AgBr & AgCI are respectively 5 xx 10^(-13) & 1 xx 10^(-10) . For what ratio of the concentration of Br^(-) & CI^(-) ions would the emf of the cell be zero?

Consider the cell Ag(s)|AgBr(s)|Br^(-)(aq)||AgCl(s)|Cl^(-)(aq)|Ag(s) at 25^(@)C . The solubility product constants of AgBr & AgCl are respectively 5xx10^(-13)&1xx10^(-10) for what ratio of the concentrations of Br^(-) & Cl^(-) ionns would the emf of the cell be zero? (A). 1:200 (B). 1:100 (C). 1:500 (D). 200:1

The solubility product constant of Ag_(2)CrO_(4) and AgBr are 1.1xx10^(-12) and 5.0xx10^(-13) respectively. Calculate the ratio of the molarities of their saturated solutions.

Consider the cell Ag(s)|AgBr(s)Br^(c-)(aq)||AgCl(s),Cl^(c-)(aq)|Ag(s) at 298 K . The K_(sp) of AgBr and AgCl , respectively are 5xx10^(-13) and 1xx10^(-10) . At what ratio of [Br^(c-)] and [Cl^(c-)] ions, EMF_(cell) would be zero ?

At 25^(@) , the solubility product values of AgCl and AgCNS are 1.8xx10^(-10) and 1.6xx10^(-11) respectively. When a solution is saturated with both solids, calculate the ratio ([Cl^(-)])/([CNS^(-)]) and also [Ag^(+)] in the solution.