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Using Raoult's Law explain how the total...

Using Raoult's Law explain how the total vapour pressure over the solution is related to mole fraction of components in the following solution.
`CHCl_(3)" "(l)and CH_(2)Cl_(2)(l)" "(b)NaCl(s)and H_(2)O(l)`

Text Solution

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In this case, both the components are volatile liquids, Accoding to Raoult's law,
`P_(A)=P_(A)^(@)x_(A),P_(B)=P_(B)^(@)x_(B),P=P_(A)+P_(B)`
`P=P_(A)^(@)x_(B)=P_(A)^(@)x_(A)+P_(B)^(@)(1-x_(A))`
Here, A and B are volatile components
`P_(A)^(@)` and `P_(B)^(@)` are the partial pressures while P is the total pressure.
`x_(A) and x_(B)` are the mole fraction of the compnents in the binary solution.
In this case, NaCI(s) is non-volatile and Raoult's law is applicable only to water wich is of volaltile nature According to the law `P=P_(A)^(@)x_(A)`.
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