The problem asks to calculate the mass of the solution the student should use, given:

• The student needs 40.0 g of acetyl bromide.
• A solution is available with a 10.1% w/w (weight/weight) concentration of acetyl bromide in chloroform.
• The total available solution is 220.0 g.

To solve this:

1. The concentration means that 10.1 g of acetyl bromide is present in every 100 g of solution.

The formula for calculating the mass of solution needed is:

$\text{mass of solution} = \frac{\text{desired mass of solute}}{\text{mass fraction of solute in solution}}$

Where:

• The desired mass of solute (acetyl bromide) = 40.0 g.
• The mass fraction of solute = 10.1% = 0.101.

$\text{mass of solution} = \frac{40.0 \, \text{g}}{0.101} = 396.04 \, \text{g}$

However, only 220.0 g of solution is available, which is not enough to get the required 40.0 g of acetyl bromide.

Thus, the answer is "No solution".

Would you like further details or have any other questions?

Here are 5 related questions to expand on this topic:

1. What does w/w (weight/weight) percentage mean in chemistry?
2. How do you calculate the mass of a solution when given a solute concentration?
3. What is the significance of using significant digits in chemical calculations?
4. How can concentration percentages affect experimental outcomes in chemistry?
5. How do you dilute a solution if more solute is needed but less solution is available?

Tip: Always verify the available amount of solution before performing calculations, as it may limit your ability to meet experimental requirements.