Mole fraction is a way to express the concentration of a solution. It is a dimensionless quantity used in Class 12 Chemistry (Solutions chapter).
Mole fraction is temperature-independent, unlike molarity which changes with temperature.
Mole fraction of solute is the ratio of the number of moles of solute to the total number of moles of all components in the solution.
χ(solute) = n(solute) / [n(solute) + n(solvent)]
Where:
If 2 moles of NaCl are dissolved in 8 moles of water:
In a very dilute solution, n(solute) << n(solvent), so mole fraction of solute approaches 0 and mole fraction of solvent approaches 1.
Molecular Mass of NaOH
Molecular mass of NaOH (sodium hydroxide) = 40 g/mol. Calculation: Na (23) + O (16) + H (1) = 40. Uses of NaOH and related Class 10 Chemistry concepts explained.
Molecular Weight of Calcium Carbonate (CaCO₃)
Calculate the molecular weight of CaCO₃ (Calcium Carbonate). Step-by-step solution gives 100 g/mol — the easiest molar mass to remember.
Molecular Weight of HNO₃ (Nitric Acid)
Learn the molecular weight of HNO₃ (Nitric Acid). Step-by-step calculation gives 63 g/mol with atomic masses of H, N, and O.
Molecular Weight of NaOH (Sodium Hydroxide)
Molecular weight of NaOH (sodium hydroxide) = 40 g/mol. Step-by-step calculation: Na (23) + O (16) + H (1) = 40. Uses and properties of NaOH.
Difference Between Molecule and Compound
What is the difference between a molecule and a compound? Learn why all compounds are molecules, but not all molecules are compounds.
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