What is the correct procedure to prepare 100.0 ml of 3.00 M HCl solution from an 18.0 M HCl stock solution?

To prepare a diluted solution from a concentrated stock solution, the solution's molarity and volume are important. The process involves the dilution equation, which states that the product of the concentration and volume of the concentrated solution is equal to the product of the concentration and volume of the diluted solution. This can be represented with the formula:

[ C_1V_1 = C_2V_2 ]

Where:

• ( C_1 ) is the concentration of the stock solution (18.0 M),

• ( V_1 ) is the volume of the stock solution needed,

• ( C_2 ) is the concentration of the diluted solution (3.00 M),

• ( V_2 ) is the volume of the diluted solution (100.0 ml or 0.1 L).

Substituting the values into the equation gives:

[ (18.0 , M)(V_1) = (3.00 , M)(100.0 , ml) ]

Solving for ( V_1 ):

[ V_1 = \frac{(3.00 , M)(100.0 , ml)}{18.0 , M} = \frac