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Limiting Reagent or Reactant

A mixture con...

Question

A mixture containing $K C l$ and $N a C l$ was dissolved and total halide was determined by titration with silver nitrate. A sample weighing $0.3250 g$ required $51 m L$ of $0.1 N$ solution. Calculate the percentage of each salt in the sample.

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Solution

In the mixture of $K C l a n d N a C l$ :

74.5 g of $K C l$ requires 170 g of $A g N O_{3}$ and

58.5 g of $N a C l$ requires 170 g of $A g N O_{3}$

And in $51 m L o f 0.1 N$ solution :
weight of $A g N O_{3}$ = $\frac{0.1 \times 170 \times 51}{1000} = 0.867 g$

In solution weighing $0.3250 g$ let us consider $x$ gm $K C l$ and the remaining $0.325 - x$ gm is $N a C l$ .

$∴ m o l e s_{N a C l} + m o l e s_{K C l} = m o l e s_{A g N O_{3}}$

$∴ \frac{x}{74.5} + \frac{0.325 - x}{58.5} = \frac{0.867}{170}$

$∴ x = 0.1240 g m = w e i g h t o f K C l i n s a m p l e$

$∴ 0.201 g m = w e i g h t o f N a C l i n s a m p l e$

$p e r c e n t a g e o f K C l = \frac{0.124 \times 100}{0.325} = 38.19 %$

$p e r c e n t a g e o f N a C l = \frac{0.201 \times 100}{0.325} = 61.81 %$

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