how to find mass of aspirin if I used 0.2845g of the powder(crushed apririn) with 1mL of 6.0 mol/L of Nacl? Does the dilution(the above chemicals are diluted in a 500mL volumetric flask) matter ,and does adding the HCL/Fe^3+ stock solution in the end matter (1.00 mL of the the above diluted solution is put into a 10 mL volumetric flsk. Then, the rest is filled using HCL/Fe3+ stock solution which is made of 0.020 mol/L FeCl3 and 0.12 mol/ L KCL. If it's does, please help me calculate the mass percent and the of aspirin in the tablet.
(0.2845 g of aspirin tablet used ,and
0.3723 g of crushed aspirin tablet used)
To calculate the mass percent of aspirin in the tablet, we need to determine the mass of aspirin used and the total mass of the tablet.
First, let's calculate the mass of aspirin used:
Mass of crushed aspirin = 0.3723 g
Next, we need to calculate the total mass of the tablet. Since you only provided the mass of the crushed aspirin, we'll assume that the entire tablet was crushed and used. Therefore, the total mass of the tablet is:
Total mass of tablet = 0.2845 g
Now, we can calculate the mass percent of aspirin in the tablet:
Mass percent = (mass of aspirin used / total mass of tablet) x 100
Mass percent = (0.3723 g / 0.2845 g) x 100
Mass percent ≈ 130.83 %
Regarding the dilution with NaCl and the addition of HCl/Fe^3+ stock solution, these steps can affect the final mass percent calculation if they involve any chemical reactions with the aspirin. It's important to know the specific purpose of these steps to accurately determine their impact on the analysis.
If the dilution with NaCl and the addition of HCl/Fe^3+ stock solution do not react with the aspirin, they may not directly affect the mass percent calculation. However, they might still impact the overall experiment's accuracy and reliability depending on the specific analytical method being used.
To calculate the mass percent of aspirin in the tablet, you'll need to know the mass of the crushed aspirin and the total mass of the tablet.
To find the mass of aspirin, we need to calculate the amount of aspirin in the 0.2845g powder and the 0.3723g crushed tablet used.
First, we need to calculate the moles of NaCl diluted in the 1mL solution:
Moles of NaCl = concentration (mol/L) x volume (L) = 6.0 mol/L x 0.001 L = 0.006 mol
Since NaCl is not relevant for finding the mass of aspirin, we can ignore this information and move on.
Next, let's consider the dilution. Dilution does not affect the mass of the substance but affects the concentration. In this case, we have diluted the NaCl solution into a 500mL volumetric flask, but we need to calculate the mass percent and mass of aspirin, which are not affected by the dilution. Therefore, we can ignore the dilution for now.
Moving on to the addition of HCl/Fe^3+ stock solution, we need to calculate the moles of FeCl3 diluted in the 10mL solution:
Moles of FeCl3 = concentration (mol/L) x volume (L) = 0.020 mol/L x 0.01 L = 0.0002 mol
Now, we can calculate the mass percent of aspirin in the tablet.
Mass percent of aspirin = (mass of aspirin / mass of tablet) x 100
For the 0.2845g powder:
Mass percent of aspirin = (0.2845g / 0.2845g) x 100 = 100%
For the 0.3723g crushed tablet:
Mass percent of aspirin = (0.3723g / 0.3723g) x 100 = 100%
Note that both calculations result in 100% because we are assuming that all the mass used was pure aspirin.
Lastly, we need to find the mass of aspirin in the tablet. Since both calculations resulted in 100% mass percent, we can conclude that the mass of the tablet is equal to the mass of aspirin used:
Mass of aspirin in the tablet = 0.2845g and 0.3723g for the powder and crushed tablet, respectively.