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Byju's Answer

Standard XII

Chemistry

Types of Redox Reactions

21.6 g of sil...

Question

21.6 g of silver coin is dissolved in $H N O_{3}$ . When $N a C l$ is added to this solution, all silver is precipitated as $A g C l$ . The weight of $A g C l$ is found to be 14.35 g, then % of silver in coin is:

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Solution

Given when $N a C l$ is added, all the silver are precipitated as $A g C l$

Again weight of $A g C l$ given = $14.35 g$
Molar mass of $A g C l$ = $(103 + 35.5) g$
= $143.5 g$
So moles of $A g C l = \frac{14.35}{143.5}$ mol
$= 0.1 m o l$
Applying POAC on $A g$ ,
moles of $A g^{+}$ ion present = $0.1 m o l$
We have molar mass of $A g$ = $108 g$
$∴ 0.1 m o l A g = 108 \times 0.1 g A g = 10.8 g A g$
Given, mass of the silver coin = $21.6 g$
$∴$ $% A g$ in the coin $= \frac{10.8}{21.6} \times 100 = 50 %$

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