A solution of citric acid C6H8O7 in 50 g of acetic acid has a boiling point elevation of 1.76 K. If Kb for acetic acid is 3.07 K kg mol-1, what is the molality of solution? - Chemistry

Exercise | Q 11 | Page 46

A solution of citric acid C6H8O7 in 50 g of acetic acid has a boiling point elevation of 1.76 K. If Kb for acetic acid is 3.07 K kg mol-1, what is the molality of solution?

Solution:


Given: Boiling point elevation =ΔTb = 1.76 K

Kb of acetic acid = 3.07 K kg mol-1

Mass of acetic acid = 50 g

To find: Molality of the solution

Formula: ΔTb =  Kb m

Calculation: Using formula and rearranging, we get,

m=TbKb=1.76K3.07K kg mol-1=0.573 mol kg-1 = 0.573 m

The molality of the solution is 0.573 m.