determine the concentration of the HCl solution from the data for the standardization of the HCl with the Na2CO3. B.)calculate the moles and mass of acetylsalicylic acid in each tablet (molar mass = 180.16 g/mol). C.)calculate the % by mass of aspirin in the tablet.
Moles of HCl titrant = Excess Moles of NaOH analyte in solution
(Moles NaOH added to acetylsalicylic acid) – (Excess Moles NaOH analyte in solution) = Moles NaOH reacted
Moles NaOH reacted / 2 = Moles of acetylsalicylic acid
The titration of the excess NaOH with HCl is a neutralization reaction:
HCl (aq) + NaOH (aq) -> NaCl (aq)) + H2O (l)
2HCl (aq) + Na2CO3 (s) -> H2O (l) + CO2 (g) + 2NaCl (aq)
Knowing the mass of sodium bicarbonate used, one can calculate the moles
of sodium bicarbonate and the moles of HCl. With the volume readings from the burette and the moles of HCl
calculated, the molarity of the HCl solution can be found.
Na2CO3 is mixed with 25 mL of water in the titrated flask. final reading - Initial of HCl in burette is amount used. Show work
A.) determine the concentration of the HCl solution from the data for the standardization of the HCl with the Na2CO3.
B.)calculate the moles and mass of acetylsalicylic acid in each tablet (molar mass = 180.16 g/mol).
C.)calculate the % by mass of aspirin in the tablet.
Trending now
This is a popular solution!
Step by step
Solved in 9 steps with 3 images
