An aspirin tablet weighing 0.502 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved

the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL
of the solution was pipetted into a 100 mL volumetric flask and diluted to the mark with FeCl3 solution.
The concentration of the diluted solution is

68.2% of .502 g is 0.3424 g of ASA (acetylsalicylic acid). Divide that by 180.16 g/mole to get the number of moles of ASA. You end up with that many moles of ASA in the 250 ml flask.

3/250 of that number of moles of ASA ends up in the 100 ml flask, where it remains as the sample is further diluted. Divide that number by 0.100 liters for the molar concentration of ASA in the final solution.

To find the concentration of the diluted solution, we need to determine the number of moles of ASA (Acetylsalicylic acid) present in the 3.00 mL solution, and then calculate its concentration.

Step 1: Calculate the mass of ASA in the tablet.
Given:
- Mass of the tablet = 0.502 g
- Percentage of ASA in the tablet = 68.2%
- Molar mass of ASA = 180.16 g/mol

The mass of ASA in the tablet can be found by multiplying the mass of the tablet by the percentage of ASA:
Mass of ASA = (0.502 g) x (68.2%)
Mass of ASA = 0.502 g x 0.682
Mass of ASA = 0.342164 g

Step 2: Calculate the number of moles of ASA in the tablet.
The number of moles can be calculated by dividing the mass of ASA by its molar mass:
Number of moles of ASA = Mass of ASA / Molar mass of ASA
Number of moles of ASA = 0.342164 g / 180.16 g/mol
Number of moles of ASA = 0.001898 mol

Step 3: Calculate the concentration of ASA in the 3.00 mL solution.
The concentration can be calculated by dividing the number of moles of ASA by the volume of the solution in liters:
Concentration = Number of moles / Volume (in liters)
Volume of the solution = 3.00 mL = 3.00 x 10^-3 L
Concentration = 0.001898 mol / 3.00 x 10^-3 L
Concentration = 632.67 mol/L

Therefore, the concentration of the diluted solution is 632.67 mol/L.

To calculate the concentration of the diluted solution, we need to follow the steps outlined in the question. Let's break it down:

1. We start with an aspirin tablet weighing 0.502 g that contains 68.2% ASA by mass.
2. Convert the percentage mass of ASA to a decimal:

ASA mass = 68.2% x 0.502 g = 0.342 g

3. Calculate the number of moles of ASA using the molar mass of ASA:

Number of moles = ASA mass / molar mass of ASA
Number of moles = 0.342 g / 180.16 g/mol

4. The student dissolves the tablet in hot NaOH and dilutes it with DI water to the mark in a 250 mL volumetric flask. This step involves dilution, so the number of moles of ASA remains the same.

5. Exactly 3.00 mL of the solution is pipetted into a 100 mL volumetric flask and diluted to the mark with FeCl3 solution. Again, this step involves dilution, so the number of moles of ASA remains the same.

6. Calculate the concentration of the diluted solution:

Concentration = (Number of moles / Volume of solution) x 1000

The volume of the diluted solution is 100 mL.

Concentration = (Number of moles / 100 mL) x 1000

Now, you can substitute the calculated number of moles of ASA into the equation to find the concentration of the diluted solution.