Colligative Properties - Boiling Point Elevation, Freezing Point Depression & Osmotic Pressure

This chemistry video tutorial provides a basic introduction into colligative properties such as boiling point elevation, freezing point depression, osmotic pressure, and vapor pressure. It explains how to calculate the boiling point and freezing point of a solution as well as how to calculate the molar mass of a solute using osmotic pressure and freezing point depression.
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molality*'

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Is the melting point depressed equally as much as the freezing point by colligative forces?

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What is the relation b/w i(von't half) , boiling point and freezing point?

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If 10.00 g of NH4NO3 (M.W. = 80.043 g/mole) are dissolved in 75.00 mL of ethanol, what is the vapor pressure of the solution? I need complete explanation for this.

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0:31 - boiling point elevation 3:44 - freezing point depression 8:37 - vapor pressure 10:46 - osmotic pressure 13:44 - sample questions

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You take 20.0 g of a sucrose (C12H22O11) and NaCl mixture and dissolve it in 1.0 L of water. The freezing point of this solution is found to be "-0.426°C." Assuming ideal behavior, calculate the mass percent composition of the original mixture, and the mole fraction of sucrose in the original mixture. how can i solve this?? there are 2 solvents its mixture

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How do we know that we actually can dissolve the amount of chemical for water? As you know solubility of chemicals are limited for every chemical in every solvent. In other words how do we know that we can have a 5m solution of AlCl3 in water at the calculated freezing temperature?

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Where did you get the i=4?