There are two solutions each at `27^(@)C`
Solution `A`: contains `6g` urea in `200mL` solution
Solution `B`: contains `6g` acetic acid in `100mL` solution.
(i) Are they equimolar ? (ii) Are they isotonic ?

Answer

solution A and B are equimolar but not isotonic.

Explanation

For A: Urea is non-electolyte and exists without asociation or dissociation.
`6g` urea`//100mL` solution
`60g` urea//L` solution
`thereofer 1` mol urea`//L` solution
`thererfore 1` Molarity of urea solution `=1M`
Osmotic pressure `pi_(A)=MST`
`=1xx0.0821xx300=24.63` atm
For B: Molarity of acetic acid solution `=1M`
`CJ_(3)COOH` ionises in aqueous solution:
`CH_(3)COOH+hArrCH_(3)COO^(-)+H_(3)O^(+)`
`i`(van't Hoff factor)`=(1+x),xgt0`,*Where `x` is degree of dissociation)
`therefore pi_(B)=MST)1+x)`
`=1xx0.0821xx300(1+x)`
`=24.63(1+x)` atm.
Thus, `24.63(1+x)gt24.63`
`pi_(B)pi_(A)`
Thus, solutions A and B are equimolar but not isotonic.