The standard reduction potential of a silver chloride electrode (metal-sparingly soluble salt electrode) is 0.029 V and for silver electrode is 0.80V. If the moles of AgCl that can dissolve in 10 L of a 0.01 M NaCl solution is represted as `10^(-z)` find the value of Z.
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`E_(Cl^(-))^(o)//AgCl//Ag=E_(Ag^(+)//Ag)^(o)+(0.0591)/1log K_(sp)` `=0.209=0.80+(0.0591)/1logK_(sp)` `K_(sp)=10^(-10)`, Let solubility of `AgCl` in `0.01M` solution is `x` `10^(-10)=x(x+0.01)` `x=10^(-6)` Moles of `AgCl` dissolved in `10L=10^(-8)xx10=10^(-7)`
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