NaCl has higher boiling point than C₂H₆O₂ in H₂O.
<h3>What is molality?</h3>
- The number of moles of solute in a solution equal to 1 kg or 1000 g of solvent is referred to as its molality.
- The definition of molarity, on the other hand, is based on a certain volume of solution.
- Mol/kg is a typical molality measurement unit in chemistry.
<h3>Calculation of boiling point:</h3>
When the non-volatile solute is dissolved in a solvent, the boiling point rises along with the molality (concentration) of the solute.
Given,
Mass of C₂H₆O₂ (solute) = 15.0 g
Mass of solvent (H₂O) = 0.50 kg
Molar mass of C₂H₆O₂ = 62 g/mol
Thus, the moles of solute = 15.0 g x 1.0 mol solute/62 g/mol
= 0.2419 mol
Therefore, molality(m) of C₂H₆O₂ (solute) = Amount of solute (mol)/ Mass of solvent
= 0.2419/0.50
= 0.4838 m
Similarly,
Given ,
Mass of NaCl (solute) = 15 g
Mass of solvent (H₂O) = 0.50 kg
Molar mass of NaCl (solute) = 58.44 g/mol
Thus, the moles of NaCl (solute) = 15.0 g x 1.0 mol solute/58.44
= 0.2566 mol
Therefore, molality(m) of NaCl (solute) = Amount of solute (mol)/ Mass of solvent
= 0.2566 mol/0.50 kg
= 0.51 m
Hence, the molality of NaCl (solute) is more than the molality of C₂H₆O₂(solute).
So, with an increase in the solute's concentration (molality), the boiling point rises.
Therefore, NaCl has higher boiling point than C₂H₆O₂ in H₂O.
Learn more about boiling point here:
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