Questions: Sulfuric acid is normally purchased at a concentration of 18.0 M. What is the volume of the sulfuric acid solution is required to prepare 206.7 mL of 0.225 M aqueous H2SO4? (Remember to add acid to water rather than water to acid.)

Solution Steps

We need to determine the volume of a concentrated sulfuric acid solution (18.0 M) required to prepare 206.7 mL of a diluted sulfuric acid solution with a concentration of 0.225 M.

The dilution formula is given by:

\[ C_1V_1 = C_2V_2 \]

where:

• \(C_1\) is the concentration of the concentrated solution (18.0 M),
• \(V_1\) is the volume of the concentrated solution we need to find,
• \(C_2\) is the concentration of the diluted solution (0.225 M),
• \(V_2\) is the volume of the diluted solution (206.7 mL).

Rearrange the dilution formula to solve for \(V_1\):

\[ V_1 = \frac{C_2V_2}{C_1} \]

Substitute the known values into the equation:

\[ V_1 = \frac{0.225 \, \text{M} \times 206.7 \, \text{mL}}{18.0 \, \text{M}} \]

Perform the calculation:

\[ V_1 = \frac{0.225 \times 206.7}{18.0} = \frac{46.5075}{18.0} \approx 2.5838 \, \text{mL} \]

Final Answer