The standard electrode potential for the following reaction is `+1.33` V. What is the potential at pH=2.0?
`Cr_(2)O_(7)^(2-)(aq,1M)+14H^(+)(aq)+6e^(-)to2Cr^(3+)(aq,1M)+7H_(2)O(l)`

Options

A. `+1.820V`
B. `+1.990V`
C. `+1.608V`
D. `+1.0542V`

Answer

4

Explanation

`E_(Cr_(2)O_(7)^(2-)|Cr^(3+))=E_(Cr_(2)O_(7)^(2-)|Cr^(3+))^(@)-(0.0591)/(6)xx(log.([Cr^(3+)]^(2))/([Cr_(2)O_(7)^(2-)])xx(1)/([H^(+)]^(14)))`
`E_(Cr_(2)O_(7)^(2+)|Cr^(3+))=1.33-(0.0591)/(6)log.(1)/((0.01)^(14))" "rArr" "1.0542V`