Question

Osmotic pressure of 0.1 M aqueous solution of NaCl is how many times does motive pressure of 0.1 M aqueous solution of glucose?

Answer 1

Answer:- two times.

Explanations:- Osmotic pressure is a colligative property means it depends on the number of solute particles that are present in the solution. The equation for osmotic pressure is:

$\pi =icRT$

where, $\pi$ stands for osmotic pressure, i stands for Van't Hoff factor, R is universal gas constant and T is kelvin temperature.

Both the solutions must be at same temperature, R is a constant so it is also same. The given concentrations are also same. So, the only deciding factor is the Van't Hoff factor"i".

Glucose is a covalently bonded molecule and so it does not dissociate to give the ions in the solution where as NaCl is an ionic compound and dissociate to give sodium and chloride ions.

$NaCl(aq)\rightarrow Na^+(aq)+Cl^-(aq)$

As is clear from the equation, one NaCl gives two ions, the value of i is 2. So, the osmotic pressure of aqueous solution of NaCl would be two times to the osmotic pressure of aqueous glucose solution.