Grade 12 Chemistry
posted by Anonymous on .
This is my question:
AspirinTM (acetylsalicylic acid) is a monoprotic acid with molar mass of 180g/mol. An aqueous solution containing 3.3 g/L has a pH of 2.62. What percentage of acetylsalicylic acid molecules ionizes
in the solution?
first, the H+ in solution.
Now the H in the aspirin: molesH=3.3/180= you do it.
Now divide the H in solution by the H in the aspirin, and forpercent, multiply by 100