Is 1.0 M `H^+` solution under `H_2SO_4` at 1.0 atm capable of oxidising silver metal in the presence of 1.0 M `Ag^+` ion
`E_(Ag^+|Ag)^0=0.80V, E_(H^+|H_2(Pt))^0=0.0V`

Can 1.0 M H^(+) solution under H_(2) gas at 1.0 atm capable of oxidising Ag metal in the presence of 1.0 M Ag^(+) ions. E_(OP_(Ag//Ag^(+)))^(@) = -0.80V .

Out of aluminium and silver vessel, which one will be more suitable to store 1 M HCl solution and why ? E_(Al^(3+)|Al)^@=-1.66V, E_(Ag^(+)|Ag)^@ =+0.80V

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]

250 mL of a waste solution obtained from the workshop of a goldsmith contains 0.1MAgNO_(3) and 0.1MAuCl . The solution was electrolyzed at 2 V by passing a current of 1 A for 15 minutes. The metal/metals electrodeposited will be : (E_(Ag^(+)//Ag)^(@)=0.80V, E_(Au^(+)//Au)^(@)=1.69V)

Determine range of E^(@) values for this reaction X_(aq)^(2+)+2e^(-)toX(s) for given conditions: (a). If the metal X dissolve in HNO_(3) but not in HCl it can displace Ag^(+) ion but not Cu^(2+) ion. (b). If te metal X is HCl acid producing H_(2)(g) but does not displace either Zn^(2+) or Fe^(2+) Given E_(Ag^(+)//Ag)^(0)=0.8V" "E_(Fe^(2+)//Fe)^(0)=-0.44 E_(Cu^(2+)//Cu)^(0)=0.34V" "E_(NO_(3)^(-)//NO)^(0)=0.96V" "E_(zn^(2+)//Zn)^(0)=-0.76V

Four different solution containing 1M each of Au^(+3), Cu^(+2), Ag^(+), Li^(+) are being electrolysed by using inert electrodes. In how many samples, metal ions would be deposited at cathode? ["Given :" E_(Ag^+//Ag)^(0) = 0.8, E_(Au^(+3)//Au)^(0) = 1.00 V E_(Cu^(+2)//Cu)^(0) = 0.34 V, E_(Li^(+)//Li)^(0)= -3.03 V ]

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