What about 100cm³ of 0.1 mol/dm³

We use the dilution formula: $M_1V_1 = M_2V_2$
Where:
$M_1 = 1 \text{ mol/dm}^3$ (initial concentration of stock solution)
$V_1 = ?$ (volume of stock solution needed)
$M_2 = 0.1 \text{ mol/dm}^3$ (final desired concentration)
$V_2 = 100 \text{ cm}^3$ (final desired volume)

Substitute the values into the formula:

$$(1 \text{ mol/dm}^3) \times V_1 = (0.1 \text{ mol/dm}^3) \times (100 \text{ cm}^3)$$ $$V_1 = \frac{(0.1 \text{ mol/dm}^3) \times (100 \text{ cm}^3)}{1 \text{ mol/dm}^3}$$ $$V_1 = \boxed{10 \text{ cm}^3}$$

So, you will need 10 cm³ of the 1 mol/dm³ sulfuric acid.

• Using a 10 cm³ pipette, accurately measure 10 cm³ of the 1 mol/dm³ sulfuric acid.
• Transfer this 10 cm³ of acid into a 100 cm³ volumetric flask.
• Carefully add distilled water to the volumetric flask, swirling gently to mix.
• Continue adding distilled water until the bottom of the meniscus reaches the 100 cm³ calibration mark on the neck of the volumetric flask. Use a dropping pipette for the final few drops to ensure accuracy.

You will then have 100 cm³ of 0.1 mol/dm³ sulfuric acid.