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If the quantity of electricity required ...

If the quantity of electricity required to liberate 2.6267 g of gold from a solution of gold salt is used for the the electrolysis of `CuSO_(4)` solution in presence of copper anode, then 1.26 g of copper gets dissolved. Find the oxidation number of gold in the gold salt.
`[Cu=63, Au=197]`

Text Solution

Verified by Experts

Equivalent weight Cu in `CuSO_(4)=(63)/(2)=31.5.`
Quantity of electricity required to dissolve 31.5 g of copper from the copper anode = 96500 C.
So, electricity required to dissolve 1.26 of copper `=(96500xx1.26)/(31.5)=3860C.`
Since, 3860 C electricity is required to deposit 2.6276 g of gold from the solution, 96500 C of electricity will deposit `(2.6267xx96500)/(3860)=65.6677" g of gold."`
Therefore, the equivalent weight of gold in the gold salt = 65.6675 and its valency in the salt `=(197)/(65.6675)~~3`. Thus, the oxidation state of gold in the gold salt `=+3`.
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