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`A. `0.019` MB. `0.024` MC. `0.1` MD. `0.19` M

The chlorate ion can disproportinate in basic solution according to re

1.	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`A. `0.019` MB. `0.024` MC. `0.1` MD. `0.19` M
Answer» Correct Answer - A `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)`

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