Given the cell reactions
`MX_((s))+e^(-)rarrM_((s))+X_((aq))^(-),E^(@)=0.207V`
and `M_((aq))^(+)+e^(-)rarrM_((s)),E^(@)=0.799V`
The solubility of `MX_((s))` at 298K is

The standard reduction potential for two reactions are given below AgCl(s)+e^(-)rarrAg(s)+Cl^(-)(aq) ,E^(@)=0.22V Ag^(+)(aq)+e^(-)rarrAg(s),E^(@)=0.80V The solubility product of AgCl under standard conditions of temperature is given by

Consider a voltaic cell based on these half - cell reactions Ag^(+)(aq)+e^(-)rarrAg(s): E^(@)=+0.80V Cd^(+2)(aq)+2e^(-)rarrCd(s), E^(@)=-0.40V identify the anode and give the voltage of this cell under standard condition.

The reduction potential of the two half cell reaction (occurring in an electrochemical cell) are PbSO_(4)(s)+2e^(-)rarrPb(s)+SO_(4)^(2-)(aq)(E^(@)=-0.31V) Ag^(+)(aq)+e^(-)rarrAg(s)(E^(@)=0.80V) The feasible reaction will be

The standard reduction potentials for two reactions are given below: AgCl(s) + e^(-) to Ag(s) + Cl^(-) , E^@ = 0.22 V Ag^(+)(aq) e^(-) +e^(-) to Ag(s) , E^@ = 0.80V The solubility product of AgCl under standard conditions of temperature (298 K) is given by