Home
Class 12
CHEMISTRY
A copper - silver cell is set up . The ...

A copper - silver cell is set up . The copper ion concentration in it is 0.10 M. concetration of silver ion is not known . The cell potential measured 0.422 V. determine the concentration of silver ion in the cell.
Given : `E_(Ag+//Ag)^(@)=+0.80V,E_(Cu^(2+)//Cu)^(@)=+0.34V.`

Text Solution

Verified by Experts

The given cell may be represented as
`Cu_(s)|Cu ^(2+) (0.10M)\\Ag^(+) (C )|Ag_(s)`
`E_(cell)^(@) = E_("cathode")^(@)-("anode") = 0.80V - 0.34V = 0.46 V`
`E_(cell)^(@) = E_(cell)^(@)(0.0591)/(2)log([Cu^2+])/([Ag^(+)]^(2)`
or `0.422V-0.46V- (0.0591)/(2) log (0.1)/([Ag^(+)]^(2)`
`-0.038V = -0.0295 log (0.1)/([Ag^(+) ]^(2)` or , log`(0.1)/([Ag^(+)]^(2) = (-0.038)/(-0.0295) = 1.288`
or log`(0.1)/([Ag^(+)]^(2) = ("antilog")1.288 = 19.41` `therefore ([Ag^(+))]^(2)= (0.1)/(19.41) = 5.1519xx10^(-3)`
`([Ag^(+)] = 7.1 xx10^(-2) M`
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    VMC MODULES ENGLISH|Exercise Level-0 (Long Answer Type ) (5 Marks)|1 Videos

  • ELECTROCHEMISTRY

    VMC MODULES ENGLISH|Exercise Level-1|75 Videos

  • ELECTROCHEMISTRY

    VMC MODULES ENGLISH|Exercise Level-0 ( Short Answer Type - I) (2Marks)|9 Videos

  • CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

    VMC MODULES ENGLISH|Exercise JEE ADVANCE (ARCHIVE)|30 Videos

  • ENVIRONMENTAL CHEMISTRY

    VMC MODULES ENGLISH|Exercise JEE Main (Archive)|39 Videos

Similar Questions

Explore conceptually related problems

A copper-silver cell is set up. The copper ion concentration in it is 0.10 M. The concentration of silver ions is not known.The cell potential measured is 0.422 V. Determine the concentration of silver ions in the cell. [Given E_(Ag^(+)//Ag)^(@)=0.80,E_(Cu^(2+)//Cu)^(@)=+0.34 V]

A copper - silver cell is set up. The copper ion concentrations is 0.10 M. The concentration of silver ion is not known. The cell potential when measured was 0.422 V. Determine the concentration of silver ions in the cell. Given " "E^(@)Ag^(+)//Ag=+0.80 V,E^(@)Cu^(2+)//Cu=+0.34 V

Which is/are correct among the following? Given the half cell EMFs E_(Cu^(2+)//Cu)^(@)=0.337V, E_(Cu^(+)|Cu)^(@)=0.521V

Can a solution of 1 M ZnSO_(4) be stored in a vessel made of copper ? Given that E_(Zn^(+2)//Zn)^(@) =-0.76V and E_(Cu^(+2)//Cu)^(@)=0.34 V

One half-cell in a voltaic cell is constructed from a silver wire dipped in silver nitrate solution of unknown concentration . Its other half-cell consists of a zinc electrode dipping in 1.0 M solution of Zn(NO_(3))_(2) . A voltage of 1.48 V is measured for this cell . Use this information to calculate the concentration of silver nitrate solution used. (E_(Zn^(2+)|Zn)^(@) = -0.76V , E_(Ag^(+)|Ag)^(@) = + 0.80V ).

Cu^(+) ion is not stable in aqueous solution because because of dispropotionation reaction. E^(@) value of disproportionation of Cu^(+) is [E_(Cu^(2+)//Cu^(+))^(@)=+ 0.15 V, E_(Cu^(2+)//Cu)^(@)=0.34 V]

If excess of Zn is added to 1.0M solution of CuSO_(4) , find the concentration of Cu^(2+) ions at equilibrium. Given :E^(c-)._((Zn^(2+)|Zn))=-0.76V E^(c-)._(cell)=(E^(c-)._((Cu^(2+)|Cu))=0.34V

What must be concentration of Ag^(+) in an aqueous solution containing Cu^(2+) =1.0 M so that bot the metals can be deposited on the cathode simultaneously. Given that E_(Cu//Cu^(2+))^(0)=0.34V and E_(Ag^(+)//Ag)^(0)=0.812V,T=298K

(a) When a bright silver object is placed in the solution of gold chloride, it acquires a golden tings but nothing happens when it is placed in solution of copper chloride. Explain this behaviour of silver. [Given : E_(Cu^(2+//)Cu)^(@)=+0.34 V, E_(Ag^(+//)Ag)^(@) =+0.80 V, E_(Au^(3+//)Au)^(@) =+1.40V ] (b) Consider the figure given above and answer the following questions : (i) What is the direction of flow of electrons? (ii) Which is anode and which is cathode? (iii) What will happen if the salt bridge is removed ? (iv) How will concentration of Zn^(2+) and Ag^(+) ions be affected when the cell functions ? (v) How will concentration of these ions be affected when the cell becomes dead ?