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Alex_Xolod [135]
3 years ago
7

A solution that contains 55.0 g of ascorbic acid (Vitamin C) in 250. g of water freezes at –2.34°C. Calculate the molar mass (in

units of g/mol) of the solute. K f of water is 1.86°C/m
Chemistry
1 answer:
Vaselesa [24]3 years ago
3 0

Answer:

M=174.87g/mol

Explanation:

Hello,

In this case, we consider the depression in the freezing point as:

\Delta T=-i*m*Kf

Whereas the van't hoff factor for ascorbic acid is 1 since it is covalent, thus, we solve for the molality as shown below:

(-2.34-0)\°C=-m*1.86\°C/m\\\\m=\frac{-2.34\°C}{-1.86\°C/m} =1.26m

Next, since molal units are mol/kg, we can compute the present moles of ascorbic acid in the 250 g (0.25kg) of water:

n=1.26mol/kg*0.25kg=0.315mol

Finally, the molar mass with the given 55.0 g of ascorbic acid:

M=\frac{55.0g}{0.315mol}\\ \\M=174.87g/mol

Regards.

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When 3.66 g of KOH (∆Hsol = -57.6 kJ/mol) is dissolved in 150.0 mL of solution, it causes a temperature change of 5.87 °C.

The enthalpy of solution of KOH is -57.6 kJ/mol. We can calculate the heat released by the solution (Qr) of 3.66 g of KOH considering that the molar mass of KOH is 56.11 g/mol.

3.66g \times \frac{1mol}{56.11g} \times \frac{(-57.6kJ)}{mol} = -3.76 kJ

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150.0 mL of solution with a density of 1.02 g/mL were prepared. The mass (m) of the solution is:

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Qa = c \times m \times \Delta T\\\\\Delta T = \frac{Qa}{c \times m} = \frac{3.76 \times 10^{3}J  }{\frac{4.184J}{g.\° C }  \times 153g} = 5.87 \° C

When 3.66 g of KOH (∆Hsol = -57.6 kJ/mol) is dissolved in 150.0 mL of solution, it causes a temperature change of 5.87 °C.

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