A 3% aqueous solution of urea is isotonic to 5% aqueous solution of another solute. Considering van't Hoff factor of the other solute to be 1.0, determine its molecular mass.

Question

A 3% aqueous solution of urea is isotonic to 5% aqueous solution of another solute. Considering van't Hoff factor of the other solute to be 1.0, determine its molecular mass. (A) 50 (B) 60 (C) 90 (D) 100

Tardigrade Admin · Accepted Answer

π = C1RT π = C2RT ∴ C1 = C2 or n1 = n2 ⇒ (3/60) = (5/Mol. mass) ⇒ Mol. mass = 100

Q. A 3% aqueous solution of urea is isotonic to 5% aqueous solution of another solute. Considering van't Hoff factor of the other solute to be 1.0, determine its molecular mass.

50

60

90

100

$π = C_{1} RT$
$π = C_{2} RT$
$∴ C_{1} = C_{2}$ or $n_{1} = n_{2}$
$\Rightarrow \frac{3}{60} = \frac{5}{M o l . ma ss} \Rightarrow$ Mol. mass $= 100$

Q. A 3% aqueous solution of urea is isotonic to 5% aqueous solution of another solute. Considering van't Hoff factor of the other solute to be 1.0, determine its molecular mass.

50

60

90

100

π=C1​RT π=C2​RT ∴C1​=C2​ or n1​=n2​ ⇒603​=Mol.mass5​⇒ Mol. mass =100

$π = C_{1} RT$
$π = C_{2} RT$
$∴ C_{1} = C_{2}$ or $n_{1} = n_{2}$
$\Rightarrow \frac{3}{60} = \frac{5}{M o l . ma ss} \Rightarrow$ Mol. mass $= 100$