Question

In: Chemistry

finishing this table.

 

finishing this table.

Hint: The column “i” applies to electrolyte (ionic) solutions and represents the ratio of moles of particles in solution to moles of formula units dissolved. In this case, glycerol has a value of 1 (it does not dissociate into separate units), NaCl has a value of 2 (it separates into 2 units—1 Na+ and 1 Cl-), and CaCl2 has a value of 3 (it separates into 3 units—1 Ca2+ and 2 Cl-). The molality column is experimentally determined by solving the equation Δt = iKfm for m. Note: Kf = 1.86 oC•kg/mol; Δt = iKfm, therefore m = Δt/iKf;

Table 1: Freezing Data Point

Solution

Freezing Point (OC)

Δt (Ti – Tf)

i

Molality (m)

Solute Mass (g)

Solvent Mass (kg)

H2O

-1.3OC

         

Glycerol

- 4.4OC

3.1

   

6.3

0.025

NaCl

-8.6OC

7.3

   

2.0

0.025

CaCl2

-5.6OC

4.3

   

2.0

0.025

Solutions

Expert Solution

Ans 1) Let us first calculate the molality and vant hoff factor(i) for glycerol

We all know Vant Hoff factor (i) is the ratio of observed number of particles ( after dissociation / association ) to the original number of particles (before dissociation /association) only in case of electrolyte.

i.e. i= obserbed number of particles / original number of particle

Now we know glycerol is a non-electrolyte so there is no chance of association or dissociation of particles and in case of non electrolyte ,vant hoff factor (i) = 1

therefore for glycerol , i= 1

Now , we know

where m is the molality

Therefore

where Kf = molal depression constant

Given

Kf = 1.86 0C Kg/mol

therefore molality

      = 3.1 / 1x1.86

       = 1.666 m

Ans 2) Let us calculate the molality and vant hoff factor for NaCl

We Know, NaCl is a electrolyte which dissociates

i.e NaCl -> Na+ + Cl-

Here we can see after dissociation,

observed number of particle = 1+1 = 2

and before dissociation

original number of particle = 1

Therefore , i=2/1

                 = 2

Now, we know

Given ,

Therefore

      = 7.3 / 2 x 1.86

      = 1.962 m

Ans 3) Let us calculate the molality and vant hoff factor for CaCl2

We know , CaCl2 is a electrolyte which dissociates as

CaCl2 -> Ca2+ + 2Cl-

Here we can see after dissociation

observed number of particle = 1+2=3

and before dissociation

original number of particle = 1

therefore i= 3/1

              = 3

we Know

Given ,

      = 4.3 / 3 x 1.86

      = 0.770 m

Now , Together we can conclude our answer as

For glycerol ,

i= 1 , molality m = 1.666

For NaCl

i=2 ,molality ,m=1.962

For CaCl2

i=3 , molality , m= 0.770 m


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