Determine the boiling points of 1 m solution of suger, glucose, urea, sodium chloride, barium chloride, aluminium chloride.

What do you mean by m millimeter?

Also there is not boiling point When sugar is melted, it becomes caramelized.

Note that m stands for molality.

delta T = i*Kb*m
i is the van't hoff factor and is 1 for sugar, glucose and urea. i for NaCl is 2, for BaCl2 it is 3 and for AlCl3 it is 4.
Plug in m, Kb (look up Kb in your text or Google it) and the appropriate i value, then add delta T to the normal boiling point of water (100 C).
Post your work if you get stuck.

To determine the boiling points of these solutions, we need to consider the concept of boiling point elevation. Boiling point elevation occurs when a non-volatile solute, such as sugar, glucose, urea, sodium chloride, barium chloride, or aluminium chloride, is added to a solvent, typically water. The presence of the solute increases the boiling point of the solvent.

To calculate the boiling point elevation, we can use the following formula:

ΔTb = Kb * m

Where:
- ΔTb represents the boiling point elevation,
- Kb is the molal boiling point elevation constant specific to the solvent (for water, Kb = 0.512 °C/mol/kg),
- m is the molality of the solution, which is the number of moles of solute divided by the mass of the solvent in kilograms.

Let's calculate the boiling points for each solution using this information:

1. Sugar (C12H22O11):
The molecular weight of sugar is approximately 342.3 g/mol.
Let's assume we have 1 mole of sugar added to 1 kg of water.
Therefore, the molality (m) of the solution is 1 mol/kg.

Using the formula, ΔTb = Kb * m, we can calculate the boiling point elevation:
ΔTb = 0.512 °C/mol/kg * 1 mol/kg = 0.512 °C

Therefore, the boiling point of a 1 m sugar solution would be the boiling point of pure water (100 °C) plus the boiling point elevation (0.512 °C), which is approximately 100.512 °C.

Repeat this process for the other solutes:
2. Glucose (C6H12O6):
- Molecular weight: 180.16 g/mol
- Assume 1 mole of glucose and 1 kg of water
- Calculate molality (m) and ΔTb similarly

3. Urea (CH4N2O):
- Molecular weight: 60.06 g/mol
- Assume 1 mole of urea and 1 kg of water
- Calculate molality (m) and ΔTb similarly

4. Sodium chloride (NaCl):
- Molecular weight: 58.44 g/mol
- Assume 1 mole of sodium chloride and 1 kg of water
- Calculate molality (m) and ΔTb similarly

5. Barium chloride (BaCl2):
- Molecular weight: 208.23 g/mol
- Assume 1 mole of barium chloride and 1 kg of water
- Calculate molality (m) and ΔTb similarly

6. Aluminium chloride (AlCl3):
- Molecular weight: 133.34 g/mol
- Assume 1 mole of aluminium chloride and 1 kg of water
- Calculate molality (m) and ΔTb similarly

By performing these calculations, you will be able to determine the boiling points of 1 m solutions of each of these solutes in water. Remember to add the calculated boiling point elevation to the boiling point of pure water (100 °C) to obtain the boiling point of the solutions.