Question

Which of the following pairs of solutions can we expect to be isotonic at the same temperature?
(1) 0.1 M NaCl and 0.1 M Na2so4
(2) 0.1 M urea and 0.1 M NACI
(3) 0.1 M urea and 0.2 M MgCl2
(4) 0.1 M Ca(NO3)2 and 0.1 M NaSO4​

Answer 1

Answer : 0.1MCa(NO3)2and0.1MNa2SO4

Isotonic solution have the same osmotic pressures.

The same osmotic pressures implies the same concentrations, 0.1MCa(NO3)2 produces 0.3M species (0.1MCa2++0.2MNO−3) and also 0.1MNa2SO4 produces 0.3M species (0.2MNa+ and 0.1MSO2−4)

Answer 2

The pairs of solutions are 0.1 M $Ca(NO_3)_2$ and 0.1 M $Na_2SO_4$  that are isotonic at the same temperature.

Explanation:

Isotonic solutions are those solutions which have the same osmotic pressure.  If osmotic pressures are equal at the same temperature, concentrations must also be equal.

$\pi=iCRT$   (for non electrolytes)

$\pi$ = osmotic pressure

i= vant hoff factor

C= concentration

R= solution constant

T= temperature

0.1 M $Ca(NO_3)_2$ and 0.1 M $Na_2SO_4$

i= 3 For $Ca(NO_3)_2$ as it dissociate to give 3 ions.

$Ca(NO_3)_2\rightarrow Ca^{2+}+2NO_3^{-}$

$C=3\times 0.1=0.3M$

i = 3 for 0.1 M $Na_2SO_4$

$Na_2SO_4\rightarrow 2Na^++SO_4^{2-}$

$C=3\times 0.1=0.3M$

Thus as the concentrations are same, the solutions are isotonic.

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