An ethylene glycol solution contains 28.3 g of ethylene glycol, C 2 H 6 O 2 in 97.2 mL of water. Calculate the freezing point of the solution. The density of water 1.00 g/mL.

An ethylene glycol solution contains 28.3 grams of ethylene glycol, which is c c 2 h six zero two, in 97.2 ml of water. Calculate the freezing point of the solution, where total the density of water is 1 gram per milliliter. Alright. So here we need to calculate the freezing point. So we need to figure out change in freezing point. So delta t f equals I times k f times m. Ethylene glycol is a covalent solute, so it doesn't break up into ions. Therefore, the van't Hoff factor is 1. The solvent here is water, so its k f is 1.86 degrees Celsius over molality. Then what we need to do is we need to figure out the moles of ethylene glycol. K. So here we're gonna figure out the moles of ethylene glycol. For every 1 mole, the mass is 62.068 grams. So plug that here. And then we need to figure out the kilograms of water, so we have 97.2 ml's. We're told that the density of water is 1 gram per 1 ml. And then remember 1 kilogram is 10 to the 3 grams. Okay. So this comes out to 0.0972 kilograms. So we plug that here. So when we do that we get 8.72 degrees Celsius, and freezing point of our new solution equals freezing point of our pure solvent water minus delta t f. Remember, pure water freezes at 0 degrees Celsius minus 8.72 degrees Celsius, so our answer here is negative 8.72 degrees Celsius. So this will be the new freezing point of our created solution.

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14. Solutions

Freezing Point Depression

General Chemistry

14. Solutions

Freezing Point Depression

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Multiple Choice

An ethylene glycol solution contains 28.3 g of ethylene glycol, C₂H₆O₂ in 97.2 mL of water. Calculate the freezing point of the solution. The density of water 1.00 g/mL.

–8.72°C

–0.848°C

–0.541°C

–17.4°C

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Verified step by step guidance

Determine the molar mass of ethylene glycol (C₂H₆O₂) by adding the atomic masses of its constituent elements: carbon (C), hydrogen (H), and oxygen (O). Use the periodic table to find these values.

Calculate the number of moles of ethylene glycol using the formula: \( \text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \). Substitute the given mass of ethylene glycol and the molar mass you calculated.

Find the mass of water in grams using the density formula: \( \text{mass} = \text{density} \times \text{volume} \). Given the density of water is 1.00 g/mL and the volume is 97.2 mL, calculate the mass of water.

Calculate the molality of the solution using the formula: \( \text{molality} = \frac{\text{moles of solute}}{\text{kilograms of solvent}} \). Convert the mass of water from grams to kilograms and use the moles of ethylene glycol calculated earlier.

Use the freezing point depression formula: \( \Delta T_f = i \cdot K_f \cdot m \), where \( i \) is the van't Hoff factor (which is 1 for ethylene glycol), \( K_f \) is the freezing point depression constant for water (1.86 °C/m), and \( m \) is the molality. Calculate the change in freezing point and subtract it from the normal freezing point of water (0°C) to find the freezing point of the solution.