Osmosis and Osmotic Pressure of the Solution

A solution containing $5 \%$  urea  solution (molecular mass = 60 g mol^-1) is isotonic with a 20 % solution of a nonvolatile solute. The molar mass of non volatile solute is-

Select the incorrect statements about the following solutions.
I: $1 \mathrm{M}$ aqueous glucose solution
II$:1 \mathrm{M}$ aqueous sodium chloride solution
II!: $1 \mathrm{M}$ aqueous ammonium phosphate solution
IV: $1 \mathrm{M}$ benzoic acid in benzene

According to Boyle -Van't Hoff law for solutions the osmotic pressure of a dilute solution is

Which of the following is Boyle-Van't Hoff law?

A $0.6\%$ solution of urea (molecular mass $=60$ ) would be isotonic with $\_\_\_$

A $25\%$ solution of cane-sugar $\left(\mathrm{mol}\right.$mass $\left.=342 \mathrm{g}{ \mathrm{mol}}^{-1}\right)$ is isotonic with $5\%$ solution of a substance $\mathrm{A}.$ Then find the molecular weight of $\mathrm{A} ?$

A living cell contains a solution which is isotonic with $0.3 \mathrm{M}$ sugar solution. What osmotic pressure develops when the cell is placed in $0.1 \mathrm{M} \mathrm{NaCl}$ solution at body temperature$\left(37°\mathrm{C}\right)$?

Which of the following $0.1 \mathrm{M}$ aqueous solutions will exert the highest osmotic pressure?

$0.05 \mathrm{M}$ solution of ${\mathrm{K}}_4\left[\mathrm{Fe}{\left(\mathrm{CN}\right)}_6\right]$ at $300\mathrm{K}$ is $92\%$ dissociated. Calculate the osmotic pressure of the solution.$(\mathrm{R}=0.0821 \mathrm{atm} {\mathrm{LK}}^{–1}{\mathrm{mol}}^{–1})$

Osmosis is defined as

Calculate the osmotic pressure of $0.01 \mathrm{M}$ solution of urea at $27 °\mathrm{C}$ temperature in atmospheres. $(\mathrm{R} = 0.0821 \mathrm{L} \mathrm{atm} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1})$.

The measured osmotic pressure of a solution prepared by dissolving $17.4\mathrm{mg}$ of ${\mathrm{K}}_2{\mathrm{SO}}_4$ in $2 \mathrm{L}$ of water at $27°\mathrm{C}$ is $3.735\times {10}^{-3}$ bar. The Van't Hoff factor is $\left(\mathrm{R}=0.083 \mathrm{L}\right.$ bar ${\mathrm{K}}^{-1} {\mathrm{mol}}^{-1};$ atomic weights $\left.\mathrm{K}=39;\mathrm{S}=32;\mathrm{O}=16\right)$

At $300 \mathrm{K}$, a decimolar solution of ${\mathrm{K}}_4\left[\mathrm{Fe}(\mathrm{CN}{)}_6\right]$ dissociates to $50\%$. The osmotic pressure of the solution is __________

If the $\mathrm{pH}$ of a monobasic acid is $2.0$ at $25{}^o\mathrm{C}$, the osmotic pressure of its $0.1 \mathrm{M}$ solution will nearly be equal to

$7.6\mathrm{gm} \mathrm{KBr}$ in $1250 \mathrm{ml}$ solution was found to have an osmotic pressure of $1.804 \mathrm{atm}$ at $27°\mathrm{C}$. Calculate degree of dissociation in $\%$ $($Atomic weight $\mathrm{K}=39, \mathrm{Br}=80)$

A solution has osmotic pressure of $0.821 \mathrm{atm}$ at $300\mathrm{K}$.

Its concentration would be :

Osmotic pressure of naphthalene solution at $27°\mathrm{C}$ is $500 \mathrm{mm} \mathrm{Hg}$. When the solution is diluted and temperature is raised to $47°\mathrm{C}$, osmotic pressure of the solution becomes $105 \mathrm{mm} \mathrm{Hg}$. The extent of dilution approximately is :-