`MnO_(4)^(-) + 8H^(+) + 5e^(-) rightarrow Mn^(2+) + 4H-(2)O`,
If `H^(+)` concentration is decreased from 1 M to `10^(-4)` M at `25^(@)C`, whereas concentration of `Mn^(2+)` and `MnO_(4)^(-)` remains 1M, then:

MnO_4^(-) + 8H^(=) + 5e^(-) rarr Mn^(2+) + 4 H_2 O If H^(+) concentration is decreaded from 1M to 10^(-4) M at 25^@ C .

If the H^(+) concentration is decreased from 1 M to 0^(-4)M at 25^(@)C for the couple MnO_(4)^(-) then the oxidation power of the MnO_(4)^(-)/ Mn^(2+) couple decrease by :

If the H^(+) concentration is decreased from 1 M to 0^(-4)M at 25^(@)C for the couple MnO_(4)^(-) then the oxidation power of the MnO_(4)^(-)/ Mn^(2+) couple decrease by :

The magnitude of the change in oxidising power of the MnO_4^(-)//Mn^(2+) couple is x xx 10^(-4)V , if the H^(+) concentration is decreased from 1M to 10^(-4) M at 25^(@)C . (Assume concentration of MnO_4^(-) and Mn^(2+) to be same on change in H^(+) concentration ) . The value of x is ___________. (Rounded off to the nearest integer ) [Given : (2.303 RT)/(F) = 0.059 ]

MnO_(4)^(-)+8H^(+)+n e^(-)rarrMn^(2+)+4H_(2)O The value of n is

How much is the oxidising power of the MnO_4^(-) (1M)|Mn^(2+) (1M) couple decreased if the H^+ concentration is decreased from 1M to 10^-4 M at 25^@C

In acidic medium " MnO"_(4)^(-) is an oxidising agent as " MnO"_(4)^(-) +8H^(+)+5e^(-) rarr Mn^(2+)+4H_(2) O . If H^(+) concentration is doubled, electrode potential of the half-cell " MnO"_(4)^(-)// " Mn"^(2+), Pt will :