Consider the cell `|{:(H_(2)(Pt)),(1atm):} :|: {:(H_(3)O^(+)(aq)),(pH =5.5):}:||{:(Ag^(+)),(xM):}:|Ag` . The measured `EMF` of the cell is `1.023 V`. What is the value of `x`?
`E_(Ag^(+),Ag)^(@) +0.799 V.[T = 25^(@)C]`

Calculate emf of given cell at 25^(@)C : [Given: E_(Ag^(+)//Ag)^(@)) = 0.80V]

The emf of the cell, Pt|H_(2)(1atm)|H^(+) (0.1M, 30mL)||Ag^(+) (0.8M)Ag is 0.9V . Calculate the emf when 40mL of 0.05M NaOH is added.

The measured voltage of the cell, Pt(s)|H_2(1.0"atm")|H^+(aq)||Ag^+(1.0M)|Ag(s) is 1.02 V " at " 25^@C . Given E_("cell")^@ is 0.80 V, calculate the pH of the solution .

Voltage of the cell Pt, H_(2) (1atm)|HOCN(1.3 xx 10^(-3)M)||Ag^(+) (0.8M) |Ag(s) is 0.982V . Calculate the K_(a) for HOCN , neglect [H^(+)] because of oxidation of H_(2)(g) Ag^(+) +e^(-) rarr Ag(s) = 0.8V

Calcualte the EMF of the cell at 298K Pt|H_(2)(1atm) | NaOH(xM), NaCl(xM) | AgCl(s) | Ag E_(Cl^(-)|AgCl|Ag)^(@) = +0.222V

An alloy of Pb-Ag weighing 1.08g was dissolved in dilute HNO_(3) and the volume made to 100 mL.A ? Silver electrode was dipped in the solution and the emf of the cell dipped in the solution and the emf of the cell set-up as Pt(s),H_(2)(g)|H^(+)(1M)||Ag^(+)(aq.)|Ag(s) was 0.62 V . If E_("cell")^(@) is 0.80 V , what is the percentage of Ag in the alloy ? (At 25^(@)C, RT//F=0.06 )

The E_(cell)^(@) value for Pt, H_(2)|H^(+)||Ag^(+)|Ag is __________. [E_(Ag//Ag^(+))^(@) = -0.799 V]