A solution of AgNO_3 was stirred with iron rod. Will it cause any change in the concentration of silver and nitrate ions? (`(E^0)_((Fe^(2+))/(Fe)=-0.44V)` , `((E^0)_((Ag^+)/(Ag))=0.80V)`

Out of aluminium and silver vessel which one will be more suitable to store 1(M) HCl solution . (E^0)_((Al^(+3))/(Al) =-1.66v) , (E^0)_((Ag^+)/(Ag))=0.80V

600 ml of a 0.1 (N) solution of AgNO_3 is added to 500 mL of 0.1 (N) KCI solution. The concentration of nitrate in the resulting solution is

Can Fe^(2+) be produced in the reaction of Fe with 1(M) HCl solution? Explain. Given : E_(Fe^(2+)|Fe)^(@)=-0.44V

It the reaction, 2Ag(s)+Fe^(2+)(aq)rarr2Ag^(+)(aq)+Fe(s) possible? Given : E_(Fe^(2+)|Fe)^(@)=-0.44V and E_(Ag^(+)|Ag)^(@)=+0.80V .

A silver electrode is immersed in a 0.1 (M) AgNO_(3) solution at 25^(@)C . If AgNO_(3) dissociates almost completely in the solution, then determine the potential of the silver electrode. Given : E_(Ag^(+)|Ag)^(@)=0.80V .

If Fe is allowed to react with 1(M) HCl solution, will Fe be oxidised to Fe^(2+)? E_(Fe^(+2)|Fe)^(@)=-0.44V

Between Fe and Mn which can be converted to +2 oxidation state easily ? Given : E_(Fe^(2+)|Fe)^(@) =-0.44" V & "E_(Mn^(2+)|Mn)^(@)= - 1.20 V

Consider the galvanic cell Cu|Cu^(2+)(0.13M)||Ag^(+)(0.01M)|Ag (i) Calculate the reduction potential of each electrode and EMF of the cell (ii) Is is reaction representing the cell spontaneous ? ["Given : "E_(Cu^(2+)|Cu)^(@)=+0.34V and E_(Ag^(+)|Ag)^(@)=+0.80V]

Write down the appropriate Nernst equation for the following voltaic cell and calculate the e.m.f. of the cell at 298 K. Fe(s)|Fe^(2+)(0.002M)||Ag^+(0.02M)|Ag (s) (Given : E_(Fe^(2+)//fe)^@ =-0.44V and E_(Ag^+//Ag)^@ =0.80V at 298 K) 1+2

Write down the appropriate Nernst equation for the followign volataic cell and calcualte the emf of the cell at 298K. Fe(s)|Fe^(2+) (0.002 M)||Ag^+(0.02 M) |Ag(s) Given E^@_(Fe^(2+)//Fe) = 0.44 V and E^@_(Ag^(2+)//Ag) = 0.80v at 298K.