Question
When silver chloride is dissolved in a large excess of ammonia, practically all silver ion can be assumed to exist in form of a single ionic species [Agx(NH3)y]x+. Compute the values of x and y using the two following cells:
Cell I: Ag|4.0 × 10−4 M – AgCl, 1 M – NH3||4 × 10−2 M – AgCl, 1 M – NH3|Ag; Ecell = 0.118 V at 298 K.
Cell II: Ag|3 × 10−3 M – AgCl, 1 M – NH3 ||3 × 10−3 M – AgCl, 0.1 M – NH3|Ag; Ecell = 0.118 V at 298 K.
Options
Solution
$xAg^{+} + yNH_{3} \rightleftharpoons Ag\left( NH_{3} \right)_{y}^{x +} $$${a\text{ Mb M}0\text{b>>a} }{\text{Eqn.}?\text{b M}\frac{a}{x}\text{ M}}$$
$K_{f} = \frac{a/x}{\left\lbrack Ag^{+} \right\rbrack^{x}.b^{y}} \Rightarrow \left\lbrack Ag^{+} \right\rbrack = \left( \frac{a}{K_{f}.x.b^{y}} \right)^{1/x}$
Cell reaction: Ag+ (Right) ? Ag+ (Left)
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