Identify lab equipment and calculate the mass of NaCl needed for a solution.

Volume of solution ($V$) = $100 \text{ cm}^3 = 0.1 \text{ dm}^3$
Concentration ($C$) = $1.0 \text{ mol/dm}^3$
Molar mass of NaCl ($M$) = $58.5 \text{ g/mol}$

2 (d) Describe how 100 cm$^3$ of the 1.0 mol dm$^{-3}$ solution of sodium chloride is prepared using the materials provided.

1. Weigh out 5.85 g of sodium chloride (NaCl) into beaker C.
2. Add a small amount of distilled water from measuring cylinder B to beaker C and stir with the stirring rod until the NaCl is completely dissolved.
3. Carefully transfer the dissolved NaCl solution from beaker C into the 100 cm$^3$ volumetric flask A.
4. Rinse beaker C and the stirring rod with small portions of distilled water from B and add the washings to volumetric flask A to ensure all solute is transferred.
5. Add distilled water from B to volumetric flask A until the solution level is close to the calibration mark.
6. Add distilled water drop by drop until the bottom of the meniscus exactly touches the 100 cm$^3$ mark.
7. Stopper the volumetric flask and invert it several times to ensure the solution is thoroughly mixed.

2 (e) Determine the approximate volume of distilled water that will remain in B after the preparation.

Initial volume of distilled water in B = $100 \text{ cm}^3$ (from part b).
Volume of solution to be prepared = $100 \text{ cm}^3$.

When preparing a solution in a volumetric flask, the volume of the solid solute is considered negligible. Therefore, approximately $100 \text{ cm}^3$ of distilled water will be used to prepare the $100 \text{ cm}^3$ solution.