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Tpy6a [65]
3 years ago
9

If the freezing point of the solution had been incorrectly read 0.3 °C lower than the true freezing point, would the calculated

molar mass of the solute have been too high or too low? Explain.
Chemistry
1 answer:
Dovator [93]3 years ago
6 0

Answer : The molar mass of the solute would be low.

Explanation :

Formula used for depression in freezing point is:  

\Delta T_f=i\times K_f\times m\\\\T^o-T_s=i\times K_f\times\frac{w_b}{M_b}\times w_a}

where,

\Delta T_f = change in freezing point

\Delta T_s = freezing point of solution

\Delta T^o = freezing point of water

i = Van't Hoff factor

K_f = freezing point constant

m = molality

w_b = mass of solute

w_a = mass of solvent

M_b = molar mass of solute

From the formula we conclude that, when the freezing point of the solution read incorrectly that is freezing point of the solution is lower than the true freezing point then this means that change in freezing point would be high and the molar mass of the solute would be low.

Hence, the molar mass of the solute would be low.

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