Asolution is prepared by dissolving 4.66 g of kcl in enough distilled water to give 250 ml of solution. kcl is a strong electrolyte. how will the freezing point of the solution be different from that of pure water?

Answer : The solution will be  lower than water.

Explanation :  Given,

Molal-freezing-point-depression constant for water =

Mass of KCl (solute) = 4.66 g

Volume of water = 250 mL

Density of water = 1.00 g/mL

So,

Mass of water (solvent) =

Molar mass of KCl = 74.5 g/mole

Formula used :  

where,

= change in freezing point

i = Van't Hoff factor = 2  (for KCl electrolyte)

= freezing point constant for water =

m = molality

Now put all the given values in this formula, we get

From this we conclude that, the solution will be  lower than water.

Therefore, the solution will be  lower than water.

the atomic mass is the bottom number on the element.

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