In titration 1, to determine M ASA , you weigh out 269.1 mg of pure aspirin (ASA

Question

In titration 1, to determine MASA, you weigh out 269.1 mg of pure aspirin (ASA) on the analytical balance. After dissolving this mass in ethanol and water, you titrate the solution with the KOH to the phenolpthaline equilvalence point. Subtracting the initial buret reading from the final one, you find that the amount of KOH consumed is equal to 24.58 mL.

Based on this titration, what is the value of MASA   (mg / mmol ) ?

While you are doing the above titration your partner is doing titration 2, to determine MSA. They weigh out 214.8 mg of pure saliclyic acid (SA) on the analytical balance. After dissolving the mass in ethanol and water, they titrate the solution to the phenolphtalein equivalence point. By subtracting the initial buret reading from the final one, they find that the amount of KOH consumed is equal to 25.84 mL.

What value of MSA ( mg / mmol ) did your partner give to you ?

In titration 3, to determine the effective molar mass (EMM) of your product, you weigh out 198.3 mg of your aspirin product on the analytical balance. After dissolving this mass in ethanol and water, you titrate the solution with KOH to the phenolphthalein endpoint. By subtracting the initial buret reading from the final one, you find the amount of KOH consumed is equal to 18.48 mL.

Based on the above titration what is the EMM (mg / mmol) of your aspirin product ?

Explanation / Answer

HC9H7O4    + KOH ----> KC9H7O4 + H2O

in the reaction above you can see that 1 mol of ASA reacts with 1mol of KOH, so in 1 mol of ASA are presents 180.15gr then, 269.1mg are content in 1.49mmol, so 1.49mmol of KOH reacts with that quantity of ASA.

269.1mg/1.49mmol = 180.60mg/mmol.

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