Given the two standard reduction potentials below, what is the `K_(sp)` of `Ag_(2)CrO_(4)` at `25^(@)C`?
`Ag_(2)CrO^(4)(s) + 2e^(-) rightarrow 2Ag(s) + CrO_(4)^(2-)(aq)` `E^(@)= + 0.446V`
`Ag^(+)(aq) + e^(-) rightarrow Ag(s)` `E^(@) = +0.799V`

Given these standard reduction potentials, what is the standard reduction potential for Co^(3+)(aq) + 3e^(-) rightarrow Co(s) ? Co^(3+)(aq) + e^(-) rightarrow Co^(2+)(aq) E^(@) = 1.82V Co^(2+)(aq) + 2e^(-) rightarrow Co(s) E^(@) = -0.28V

Write the relationship between K_(sp) and S of Ag_(2)CrO_(4) .

Given these standards reduction potentials, what is the free energy change (in kJ. Mol^(-) for the reaction: Pb(s) + 2Ag^(+)(aq) rightarrow Pb^(2+)(aq) + 2Ag(s) Ag^(+)(aq) + e^(-) rightarrow Ag(s) E^(@) = 0.80V Pb^(2+)(aq) + 2e^(-) rightarrow Pb(s) E^(@) = -0.13V

Use the standard reduction potentials: Sn^(2+)(aq) + 2e^(-) rightarrow Sn(s) E^(@) = -0.141V Ag^(+)(aq) + e^(-) rightarrow Ag(s) E^(@) = 0.800V To calcultate E^(@) for the reaction: Sn(s) + 2Ag^(+)(aq) rightarrow Sn^(2+)(aq) + 2Ag(s)

Write the solubility product expression for : (i) BaCO_(3) (s) hArr Ba^(2+) (aq) +CO_(3)^(2-) (aq) , (ii) Ag_(2)CrO_(4) (s) hArr 2Ag^(+) (aq) + CrO_(4)^(2-) (aq)

The [Ag^(+)] ion in a saturated solution of Ag_(2)CrO_(4) at 25^(@)C is 1.5xx10^(-4)M . Determine K_(SP) of Ag_(2)CrO_(4) at 25^(@)C .

The electrode potential, E^(@) , for the reduction of MnO_(4)^(-)" to "Mn^(2+) in acidic medium is +1.51V . Which of the following metal(s) will be oxidised? The reduction reactions and standard electrode potentials for Zn^(2+), Ag^(+) and Au^(+) are given as Zn_((aq))^(2+)+2e^(-)rarrZn_((s)),E^(@)=-0.762V Ag_((aq))^(+)+e^(-)hArr Ag_((x)), E^(@)=+0.80V Au_((aq))^(+)+e^(-)hArr Au_((s)), E^(@)=+1.69V

The electrode potential, E^(@) , for the reduction of MnO_(4)^(-)" to "Mn^(2+) in acidic medium is +1.51V . Which of the following metal(s) will be oxidised? The reduction reactions and standard electrode potentials for Zn^(2+), Ag^(+) and Au^(+) are given as Zn_((aq))^(2+)+2e^(-)rarrZn_((s)),E^(@)=-0.762V Ag_((aq))^(+)+e^(-)hArr Ag_((x)), E^(@)=+0.80V Au_((aq))^(+)+e^(-)hArr Au_((s)), E^(@)=+1.69V

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