Question

Which of the following solution has highest boiling point (with explanation)
a. 0.1 M KNO3 b. 0.1 BaCl2 c.0.1Na3PO4 d. 0.1M K2SO4

Answer 1

The solution having highest boiling point is 0.1 m $Na_3PO_4$

Explanation:

The expression of elevation in boiling point is given as:

$\Delta T_b=i\times k_b\times m$

where,

$\Delta T_b$ = Elevation in boiling point

i = Van't Hoff factor  

$T_b$ = change in boiling point

$k_b$ = boiling point constant

m = molality

For the given options:

• Option a:  0.1 m $KNO_3$

Value of i = 2

So, molal concentration will be = $(0.1)\times 2=0.2m$

• Option b:  0.1 m $BaCl_2$

Value of i = 3

So, molal concentration will be = $(0.1)\times 3=0.3m$

• Option c:  0.1 m $Na_3PO_4$

Value of i = 4

So, molal concentration will be = $(0.1)\times 4=0.4m$

• Option d:  0.1 m $K_2SO_4$

Value of i = 3

So, molal concentration will be = $(0.1)\times 3=0.3m$

As, the molal concentration of is the highest, so its boiling point will be the highest.

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