A 1.02 % solution of glycerine is isotopic with 2 % solution of glucose. What will be the molecular mass of glycerine?

Question

A 1.02 % solution of glycerine is isotopic with 2 % solution of glucose. What will be the molecular mass of glycerine? (A) 91.8 (B) 93 .0 (C) 90.2 (D) 96.4

Tardigrade Admin · Accepted Answer

Since the two solution are isotonic, thus ( W 2/ M 2 . V 2) (glycerine) =( W 2/ M 2 . V 2) (glucose) (1.02/ M 2 × 0.1) =(2/180 × 0.1) or M 2 =(1.02 × 180 × 0.1/0.1 × 2)=91.8

Q. A $1.02%$ solution of glycerine is isotopic with $2%$ solution of glucose. What will be the molecular mass of glycerine?

91.8

93 .0

90.2

96.4

Since the two solution are isotonic, thus
$\frac{W _{2}}{M _{2} . V _{2}}$ (glycerine) $= \frac{W _{2}}{M _{2} . V _{2}}$ (glucose)
$\frac{1.02}{M _{2} \times 0.1} = \frac{2}{180 \times 0.1}$
or $M_{2} = \frac{1.02 \times 180 \times 0.1}{0.1 \times 2} = 91.8$

Q. A 1.02% solution of glycerine is isotopic with 2% solution of glucose. What will be the molecular mass of glycerine?