Molar mass and acid dissociation constant of aspirin can be determined in a titration experiment. A 1.00g sample of aspirin is dissolved to make 500 mL of solution. 50.0 mL of this solution is titrated with .02450 M NaOH and the endpoint is determined to occur at 22.66 mL. The titration curve shows only one endpoint with a ph of 7.37.
(a)calculate the molar mass of monoprotic aspirin molecule.
(b)calculate the concentration of the sodium salt of aspirin at the endpoint and then calculate Ka for aspirin
(c) Using the Ka from part (b) for what pH range can aspirin and it's sodium salt be used as a buffer?
(d)If the sodium salt of aspirin is written as NaA write the hydrolysis reaction for the sodium salt and determine it's equilibrium constant
2007-05-30 11:56:06 · 1 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
a) 172.34
b) 2.34 , 7.85
c) 6.9 - 9.56
d) use the data above.
2007-05-31 06:20:23 · answer #1 · answered by ag_iitkgp 7 · 0⤊ 0⤋