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natta225 [31]
2 years ago
9

describe in general terms an experiment to determine the molal freezing point depression constant kf of water. Assume the availa

bility of deionized water and solid NaNO3
Chemistry
1 answer:
Dvinal [7]2 years ago
6 0
A solution (in this experiment solution of NaNO₃) freezes at a lower temperature than does the pure solvent (deionized water). The higher the solute concentration (sodium nitrate), freezing point depression of the solution will be greater.
Equation describing the change in freezing point: 
ΔT = Kf · b · i.
ΔT - temperature change from pure solvent to solution.
Kf - the molal freezing point depression constant.
b -  molality (moles of solute per kilogram of solvent).
i - Van’t Hoff Factor.
First measure freezing point of pure solvent (deionized water). Than make solutions of NaNO₃ with different molality and measure separately their freezing points. Use equation to calculate Kf.

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where,

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C = concentration

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Now put all the given values in the above formula, we get:

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Therefore, the molar mass of catalase is, 2.40\times 10^5g/mol

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