The preparation of 0.1M NaCl in100ml of NaCl solution write laboratory report and answer the following questions molarity molarity normality mole fraction %w/w %w/v?

Title: Preparation of 0.1M NaCl Solution

Objective: To prepare a 0.1M NaCl solution in the laboratory.

Materials and Methods:
- 100ml of distilled water
- 0.585g of NaCl
- Weighing balance
- Beaker
- Stirring rod
- Volumetric flask

Procedure:
1. Weigh out 0.585g of NaCl using a weighing balance.
2. Add the NaCl to a beaker containing 100ml of distilled water.
3. Stir the solution until the NaCl is completely dissolved.
4. Transfer the solution to a 100ml volumetric flask and fill it up to the mark with distilled water.
5. Mix the solution thoroughly to ensure homogeneity.

Results:
- Molarity of NaCl solution = 0.1M
- Normality of NaCl solution = 0.1N
- Mole fraction of NaCl = 0.0016
- %w/w of NaCl = 0.585%
- %w/v of NaCl = 0.585%

Discussion:
- The molarity of a solution is defined as the number of moles of solute per liter of solution. In this case, the molarity of the NaCl solution is 0.1M.
- The normality of a solution is defined as the number of equivalents of solute per liter of solution. Since NaCl dissociates into Na+ and Cl- ions, the normality of the NaCl solution is also 0.1N.
- The mole fraction of NaCl is calculated by dividing the moles of NaCl by the total moles of solute and solvent. In this case, the mole fraction of NaCl is 0.0016.
- The %w/w of NaCl is calculated by dividing the mass of NaCl by the total mass of the solution and multiplying by 100. The %w/w of NaCl in this solution is 0.585%.
- The %w/v of NaCl is calculated by dividing the mass of NaCl by the volume of the solution and multiplying by 100. The %w/v of NaCl in this solution is also 0.585%.

Conclusion:
A 0.1M NaCl solution was successfully prepared in the laboratory, with the molarity, normality, mole fraction, %w/w, and %w/v of NaCl calculated and determined.