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natta225 [31]
3 years ago
6

A certain substance X has a normal freezing point of -10.1 degree C and a molal freezing point depression constant K_f = 5.32 de

gree C middot kg middot mol^-1. Calculate the freezing point of a solution made of 29.82 g of urea ((NH_2)_CO) dissolved in 500. g of X. Be sure your answer has the correct number of significant digits.
Chemistry
1 answer:
kirill115 [55]3 years ago
7 0

Answer: -15.4^00C

Explanation:

T^0_f-T_f=i\times k_f\times \frac{w_2\times 1000}{M_2\times w_1}

where,

T_f = boiling point of solution = ?

T^o_f = boiling point of solvent (X) = -10.1^oC

k_f = freezing point constant  = 5.32^oC/kgmol

m = molality

i = Van't Hoff factor = 1 (for non-electrolyte like urea)

= mass of solute (urea) = 29.82 g

= mass of solvent (X) = 500.0 g

M_2 = molar mass of solute (urea) = 60 g/mol

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

(-10.1-(T_f))^oC=1\times (5.32^oC/m)\times \frac{(29.82g)\times 1000}{60\times (500.0g)}

T_f=-15.4^0C

Therefore, the freezing point of  solution is -15.4^0C

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