Question

a student prepare for 0.1 molal aqueous solution is containing one of the solution give below with solution has the lowest freezing point​

Answer 1

Answer:

NH4NO3 is the answer

Explanation:

this is the answer

Answer 2

Answer:

Correct answer is Option D

Explanation:

• Freezing point of a solution will decrease with  the increase of solute  in the solution
• The melting point is the same as the freezing point of the solution. The addition solute decreases the freezing point of a solvent.
• The depression in the freezing of a solvent (ΔTf) depends on the concentration and type of solute added.
• ΔTf depends on van’t Hoff factor (i), the value of i for strong electrolytes is equal to the number of ions produced by the solute.
• For non-electrolytes like glucose which remain as the whole molecule in solution without any association, the value of i is 1. The relation of ΔTf with concentration (m) and i value of solute is given as follows:
• Freezing point  depression can be calculated by using formula  :
•  $\ Tf = i * Kf* m$  
• where ∆Tf  is the change in freezing point. i is the van't Hoff factor. Kf is the cryogenic constant. m is the molality of the solution.

       Option A

• $\mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$
• = $0.1*11= 1.1$
• Option B
• $\mathrm{KOH} \\0.1 * 2=0.2$
• Option C
• $\mathrm{CH}_{3} \mathrm{COOH} \\=0.1*5=0.5$
• Option D
• $\mathrm{NH}_{4} \mathrm{NO}_{3}$
• $0.1*7=0.7$