[" 12.115.The e.m.f.of the cell Ag/Ag=(0.1M) // "],[" Ag+ (IM)/Ag at "298K" is "]

Find the solubility product of a saturated solution of Ag_2CrO_4 in water at 298 K if the e.m.f of the cell : [Ag|Ag^+ (sat. Ag_2CrO_4)|Ag^+ (0.1M)|Ag is 0.164 Vat 298 K .

EMF of the cell |Ag|AgNO_(3)(0.1M)||K Br(1 N),AgBr(s)|Ag is -0.6V at 298K AgNO_(3) is 80% and KBr is 60% dissociated. Calculate a. Solubility and b. K_(sp) of AgBr at 298 K .

EMF of the cell |Ag|AgNO_(3)(0.1M)||K Br(1 N),AgBr(s)|Ag is -0.6V at 298K AgNO_(3) is 80% and KBr is 60% dissociated. Calculate a. Solubility and b. K_(sp) of AgBr at 298 K .

EMF of the cell |Ag|AgNO_(3)(0.1M)||K Br(1 N),AgBr(s)|Ag is -0.6V at 298K AgNO_(3) is 80% and KBr is 60% dissociated. Calculate a. Solubility and b. K_(sp) of AgBr at 298 K .

The e.m.f. of the cell at 25^(@)C Cu"|"Cu^(2+)(0.01M)"||"Ag^(+)(0.1M)"|"Ag is [E^(@)(Cu^(2+)"|"Cu)=0.34V, E^(@)(Ag^(+)"|"Ag)=0.80V]

Calculate the e.m.f. of the cell, Mg//Mg^(2+)(0.1 M)||Ag^(+)(1.0xx10^(-3)M)//Ag The values of E_(Mg^(2+)//Mg)^(@) and E_(Ag^(+)//Ag)^(@) are -2.37 " V" and +0.80 " V " respectively.

Given that (at T = 298 K) Cu(s) | Cu^(2+)(1.0M) || Ag^(+)(1.0M)| Ag(s) underset(E_(cell)^(@) = 0.46V Zn(s) | Zn^(2+) (1.0M) || Cu^(2+) (1.0M) | Cu(s) underset(E_(cell)^(@) = 1.10V Then E_(cell) for, Zn | Zn^(2+)(0.1M) || Ag^(+)(0.1M) | Ag at 298 K will be:

Given that (at T = 298 K) Cu(s) | Cu^(2+)(1.0M) || Ag^(+)(1.0M)| Ag(s) underset(E_(cell)^(@) = 0.46V Zn(s) | Zn^(2+) (1.0M) || Cu^(2+) (1.0M) | Cu(s) underset(E_(cell)^(@) = 1.10V Then E_(cell) for, Zn | Zn^(2+)(0.1M) || Ag^(+)(1.0 M) | Ag at 298 K will be:

Calculate the e.m.f. of the following cell at 298 K Co//Co^(2+)(0.1M)"||"Ag^(+) (0.1M)//Ag Given E_(Co^(2+)//Co)^(Theta)= -0.28 V, E_(Ag^(+)//Ag)^(Theta)=0.8V R = 8.31JK^(-1)"mol"^(-), F = 96500 coulombs.