Suppose you need 2.0 L of 6.0 M sulphuric acid, and you have a bottle of concentrated acid of 18.0 M sulphuric acid. a). How much of this would be needed to a 2 L, 6.0 sulphuric acid solution? a). Describe how you would prepare this solution.

To determine how much of the concentrated 18.0 M sulphuric acid is needed to prepare a 2.0 L, 6.0 M sulphuric acid solution, we can use the equation:

C1V1 = C2V2

Where:
C1 = Initial concentration of the concentrated acid (18.0 M)
V1 = Volume of the concentrated acid needed
C2 = Desired concentration of the resulting solution (6.0 M)
V2 = Final volume of the resulting solution (2.0 L)

Rearranging the equation to solve for V1, we have:
V1 = (C2 * V2) / C1

Substituting the values, we get:
V1 = (6.0 M * 2.0 L) / 18.0 M

Calculating this, we find:
V1 ≈ 0.67 L

So, approximately 0.67 L of the concentrated 18.0 M sulphuric acid is needed to prepare 2.0 L of a 6.0 M sulphuric acid solution.

To prepare the solution, follow these steps:

1. Measure out approximately 0.67 L of the concentrated 18.0 M sulphuric acid using a graduated cylinder or a pipette.
2. Carefully pour the measured acid into a suitable container.
3. Add distilled water to the container to bring the total volume up to 2.0 L, ensuring thorough mixing to achieve a homogeneous solution.
4. Once the solution is prepared, use caution as concentrated sulphuric acid is highly corrosive and can cause severe chemical burns. It is recommended to wear appropriate personal protective equipment, such as gloves and goggles, when handling the acid.

It's always best to double-check calculations and take safety precautions when working with chemicals.