Transfer the tablet to a clean 125-mL Erlenmeyer flask. Add 10-mL of 1M NaOH and heat the mixture to a gentle boil. Once the solution has cooled to room temperature, transfer it to a 100-mL vol. flask. Using the diluted solution from the 100-mL volumetric flask, rinse a 1-mL vol. pipet with a few

drops and then pipet exactly 1.00-mL into a 50-mL volumetric flask. Fill the 50-mL volumetric flask to the mark with acidic FeCl3 solution. then fill the cuvette about 2/3 full with the solution.
aspirin weighs .300g and the concentration is .250mol/mL. How do i use the concentration to go back to find exact mass of ASA in unknown aspirin

To use the concentration to find the exact mass of acetylsalicylic acid (ASA) in the unknown aspirin, you'll need to follow these steps:

1. Calculate the number of moles of ASA in the known solution by using the molarity (concentration) and volume of the solution. In this case, the concentration is 0.250 mol/mL, and the volume is 1.00 mL. To convert the volume to liters, divide it by 1000:
Moles of ASA = Concentration * Volume (L)
Moles of ASA = 0.250 mol/mL * (1.00 mL / 1000) = 0.000250 mol

2. Use the molar mass of ASA to convert the moles of ASA to grams. The molar mass of ASA is 180.16 g/mol:
Mass of ASA = Moles of ASA * Molar mass of ASA
Mass of ASA = 0.000250 mol * 180.16 g/mol = 0.04504 g

Therefore, the exact mass of ASA in the known solution is approximately 0.04504 grams.