Aspirin tablet, mass of tablet= 0.4149 g concentration of iron III salicylate complex = 3.997E-4, What is the concentration of ASA in the original solution? What is the mass of ASA in the original solution?

The procedure was as follows: accurately weigh by difference a tablet and transfer it into a 125ml erlnemyer flask, add 20 ml of 0.5 M NaOH and gently heat the mixture to boiling, Transfer the solution to a 100 ml volumetric flask and dilute the solution with water to the 100ml mark, pipet 2ml of the solution into a 100 ml volumetric flask and dilute to 100ml mark with 0.02 M iron III chloride Solution.

To determine the concentration of ASA (acetylsalicylic acid) in the original solution, we can use the reaction between ASA and iron III chloride. The reaction is as follows:

FeCl3 + ASA -> iron III salicylate complex

Given:
Mass of aspirin tablet = 0.4149 g
Concentration of iron III salicylate complex = 3.997E-4

Step 1:
Calculate the moles of iron III salicylate complex:
Moles = concentration * volume

From the given information:
Concentration of iron III salicylate complex = 3.997E-4
Volume of iron III chloride solution used = 2 ml (or 0.002 L)

Moles of iron III salicylate complex = 3.997E-4 * 0.002 L = 7.994E-7 moles

Step 2:
Determine the number of moles of FeCl3 required for the above reaction. The balanced chemical equation shows that 1 mole of ASA reacts with 1 mole of FeCl3.

Therefore, the number of moles of FeCl3 = Moles of iron III salicylate complex = 7.994E-7 moles

Step 3:
Calculate the volume of 0.02 M FeCl3 solution required to react with the FeCl3:
Moles = concentration * volume

From the given information:
Concentration of FeCl3 = 0.02 M

Volume of 0.02 M FeCl3 solution required = Moles / concentration
Volume = 7.994E-7 moles / 0.02 M = 3.997E-5 L or 39.97 µL

Step 4:
Calculate the volume of the original solution in the 100 ml volumetric flask:
Volume of original solution = 100 ml

Step 5:
The dilution factor can be calculated by dividing the volume of the 100 ml volumetric flask to the volume of the original solution taken (2 ml):
Dilution factor = Volume of original solution / Volume of taken solution

Dilution factor = 100 ml / 2 ml = 50

Step 6:
Calculate the volume of the original solution using the dilution factor and the volume of the solution taken:
Volume of original solution = Dilution factor * Volume of taken solution

Volume of original solution = 50 * 2 ml = 100 ml

Step 7:
Finalize the calculations:
Concentration of ASA in the original solution = Moles of ASA / Volume of original solution

From Step 2, we know that the number of moles of ASA is equal to the number of moles of FeCl3, which is 7.994E-7 moles.

Concentration of ASA in the original solution = 7.994E-7 moles / 0.1 L = 7.994E-6 M

To calculate the mass of ASA in the original solution, we can use the molar mass of ASA:
Molar mass of ASA = 180.16 g/mol (approximately)

Mass of ASA in the original solution = Concentration of ASA * Volume of original solution * Molar mass of ASA

Mass of ASA in the original solution = 7.994E-6 M * 0.1 L * 180.16 g/mol = 14.39 µg

So, the concentration of ASA in the original solution is approximately 7.994E-6 M, and the mass of ASA in the original solution is approximately 14.39 µg.

To find the concentration of ASA (acetylsalicylic acid) in the original solution, we need to use the information provided.

1. Calculate the concentration of ASA:
- We know that the concentration of the iron III salicylate complex is 3.997E-4.
- According to the procedure, 2ml of the solution was pipetted into a 100ml flask and diluted to the mark with 0.02 M iron III chloride solution.
- This means that the volume of the pipetted solution was 2ml / 100ml = 0.02.
- The final concentration of ASA can be calculated using the dilution formula: C1V1 = C2V2.
- C1 = concentration of ASA in original solution.
- V1 = volume of ASA-containing solution (unknown).
- C2 = concentration of iron III salicylate complex = 3.997E-4.
- V2 = volume of the final diluted solution = 0.02.
- Rearranging the formula, we get C1 = (C2V2) / V1.

2. Calculate the mass of ASA:
- We know the mass of the aspirin tablet is 0.4149g.
- ASA is the main ingredient in the tablet, so the mass of ASA in the tablet is equal to the mass of the tablet.
- Therefore, the mass of ASA in the original solution is also 0.4149g.

Note: This calculation assumes that all the ASA present in the tablet is dissolved and converted to the iron III salicylate complex.

Would you like step-by-step calculations for finding the concentration of ASA in the original solution?