0-01 N solution of KCl and BaCl2 are prepared in water- The freezing point of KCl is found to be -2-C- What is the freezing point of BaCl2 solution assuming both KCl and BaCl2 to be completely ionized-

The correct option is A 3^∘C The concentrations of the two solutions are same. #160;The depression in the freezing point will be proportional to the nu ...

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Byju's Answer

Standard XII

Chemistry

Depression in Freezing Point

0.01 N soluti...

Question

$0.01 N$ solution of $K C l$ and $B a C l_{2}$ are prepared in water. The freezing point of $K C l$ is found to be $- 2^{\circ} C$ . What is the freezing point of $B a C l_{2}$ solution assuming both $K C l$ and $B a C l_{2}$ to be completely ionized?

- 3^{\circ} C

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+ 3^{\circ} C

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- 2^{\circ} C

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- 4^{\circ} C

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Solution

The correct option is A $- 3^{\circ} C$
The concentrations of the two solutions are same.

The depression in the freezing point will be proportional to the number of particles obtained on the dissociation of each solute molecule.

$K C l \to K^{+} + C l^{-}$ ..... 2 ions

$B a C l_{2} \to B a^{2 +} + 2 C l^{-}$ ..... 3 ions
$\frac{Δ T_{f} B a C l_{2}}{Δ T_{f} K C l} = \frac{3}{2}$

$\frac{Δ T_{f} B a C l_{2}}{- 2} = \frac{3}{2}$

$Δ T_{f} B a C l_{2} = - 3^{o} C$

The freezing point of water is 0 deg C.

The freezing point of $B a C l_{2}$ solution is $- 3^{o} C$ .

Hence, option A is correct.

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0.01 N solution of KCl and BaCl2 are prepared in water. The freezing point of KCl is found to be −2∘C. What is the freezing point of BaCl2 solution assuming both KCl and BaCl2 to be completely ionized?

$0.01 N$ solution of $K C l$ and $B a C l_{2}$ are prepared in water. The freezing point of $K C l$ is found to be $- 2^{\circ} C$ . What is the freezing point of $B a C l_{2}$ solution assuming both $K C l$ and $B a C l_{2}$ to be completely ionized?