compared to osmotic pressure of 0.1M urea, the osmotic pressure of 0.01 M KCl will be (assume 100% dissosiation) aprrox?

Dear student,
The osmotic pressure of urea${\pi }_{urea}$ = MRT 
where 'M' is molarity , 'T' is the temperature 
so ${\pi }_{urea}=0.1RT$
Since KCl is strong electrolyte i=2
so ${\pi }_{KCl}=iMRT$
${\pi }_{KCl}=2\times 0.01\times RT$
Putting the values of RT from equation of urea into equation of osmotic pressure
we get
${\pi }_{KCl}=0.02\times \frac{{\pi }_{urea}}{0.1}$
${\pi }_{KCl}= 0.2{\pi }_{urea}$
Therefore the osmotic pressure of KCl is 0.2 times the osmotic pressure of urea
Regards!