Out of 0.1 molal aqueous solution of glucose and 0.1 molal aqueous solution of $K C l$ , which one will have higher boiling point and why?

Open in App

Solution

In the same value of water, $0.1$ molar of $K C l$ will have a greater boiling point elevation, as boiling point elevation is a colligative property which depends on the relative amount of the constituent.
Since more ions will be produced by $K C l$ than glucose as $K C l$ is an ionic compound while glucose is a covalent compound, and thus $K C l$ will have more boiling point.

Suggest Corrections

Similar questions

Q. Out of two

0.1

molal solutions of glucose and of potassium chloride, which one will have a higher boiling point and why?

Q. The molal elevation constant of water is

0.51

. The boiling point of

0.1

molal aqueous NaCl solution is nearly:

Q. The molal elevation constant of water

= 0.52 K m^{- 1}

. The boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of

K C l

) should be:

The molal elevation constant of water = 0.52⁰C. The boiling point of 1.0 molal aqueous KCl solution (assuming complete dissociation of KCl), therefore, should be

Q. Elevation of boiling point of a

1 M

aqueous glucose solution (density

= 1.2 g/ml

) is:
(

K_{b}

is molal boiling point elevation constant)

Join BYJU'S Learning Program

Out of 0.1 molal aqueous solution of glucose and 0.1 molal aqueous solution of KCl, which one will have higher boiling point and why?

Out of 0.1 molal aqueous solution of glucose and 0.1 molal aqueous solution of $K C l$ , which one will have higher boiling point and why?