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Posted by on Sunday, January 5, 2014 at 12:40pm.

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?

  • Grade 12 Chemistry - , Sunday, January 5, 2014 at 1:04pm

    first, the H+ in solution.

    pH=-log[H]
    2.62=-logH
    H=antilog-2.62= 0.00239883292

    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

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