A certain sample of cuprous sulphide is found to have composition `Cu_(1.8)S,`, because of imcroporation of `Cu^(2+)` ion in the lattice, What is the mole % of `Cu^(2+)` in total content in this crystal?
A
0.998
B
0.1111
C
0.8888
D
none of these
Text Solution
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The correct Answer is:
B
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Ammonia is used in detection of Cu^(2+) ion because
The equilibrium constant at 278K for Cu(s)+2Ag^(o+)(aq) hArr Cu^(2+)(aq)+2Ag(s) is 2.0xx10^(15) . In a solution in which copper has displaced, some silver ions from the solution, the concentration of Cu^(2+) ions from the solution, the concentration of Cu^(2+) ions is 1.8xx10^(-2) mol L^(-1) and the concentration of Ag^(o+) ions is 3.0xx10^(-9) mol L^(-1) . Is the system at equilibrium?
How much charge in faraday is required for the reduction of 1 mole of Cu^(2+) ions to Cu ?
How does ammonia react with blue solution having Cu^(2+) ions ?
Assertion : Cuprous ion (Cu^(+)) has unpaired electrons while cupric ion (Cu^(++)) does not. Reason : Cuprous ion (Cu^(+)) is colourless where as cupric ion (Cu^(+2)) is blue in the aqueous solution.
