The chlorate ion can disproportinate in basic solution according to reaction,
`2ClO_3^(-)iffClO_2^(-)+ClO_4^-)`
what is the equilibrium concentration of perchlorate ions from a solution initially at 0.1 M in chlorate ions at 298 K?
Given: `E_(Cl_4^(-)|ClO_3^(-))^(@)=0.36V "and" E_(Cl_3^(-)|ClO_2^(-))^(@)=0.33V "at"298 K`

Options

A. `0.019` M
B. `0.024` M
C. `0.1` M
D. `0.19` M

Answer

A

Explanation

`E_(cell)^(@)=0.33-0.36=-0.03E_(cell)^(@)=(RT)/(2F)"In K"`
`-0.03=(0.06)/(2)"log K or K"=0.1`
`{:(2ClO_(3)^(-)hArrClO_(4)^(-)+ClO_(2)^(-)(x^(2))/((0.1-2x)^(2))=(1)/(10),),(0.1-2x" x x , "3.16x=0.1-2x):}`
`5.16x=0.1rArrx=0.1//5.16=0.0193~=1.9xx10^(-2)`