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?

1. 👍 0
2. 👎 0
3. 👁 182
1. 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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2. 👎 0

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