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Darya [45]
2 years ago
9

What is the expected freezing-point depression for a solution that contains 2.0 mol of KCI

Chemistry
1 answer:
larisa86 [58]2 years ago
8 0

Answer:

a. -7.44 °C

Explanation:

Hello there!

In this case, since the freezing point depression formula is:

\Delta T_f=-i*m*Kf

Thus, since the Van't Hoff's factor is 2 for KCl as it ionizes in K⁺ and Cl⁻, the molarity is 2.0 m (2.0mol/1.0kg) and the freezing point depression constant is 1.86 °C/m, we calculate the freezing point depression as follows:

\Delta T_f=-2*2.0m*1.86\°C /m\\\\\Delta T_f=-7.44\°C

Therefore, the answer is a. -7.44 °C.

Regards!

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The majority of reactions take place in solutions, making it crucial to comprehend how the substance's concentration is expressed in a solution when it is present. The number of chemicals in a solution can be stated in a variety of ways, including.

The symbol for it is M, and it serves as one of the most often used concentration units. Its definition states how many moles of solute there are in a liter of solution.

Given data:

V_{1} =57.3 L\\V_{2} = 39.5 L\\M_{1} = 0.497 m\\\\M_{2} = ?

Molarity can be determined by the formula:

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