Aspirin (acetylsalicylic acid) is a weak monoprotic acid. To determine its acid-dissociation constant, a student dissolved 2.00 g of aspirin in 0.600 L of water and measured the ph . What was the ka value calculated by the student if the ph of the solution was 2.61?

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Elin HesselLv2

28 Sep 2019

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cetylsalicylic acid, a monoprotic weak acid, is the active ingredient in aspirin. Two aspirin tablets, each containing 500.0 mg of acetylsalicylic acid, are dissolved in 25.0 mL water. a. Calculate the pH of the solution. b. Calculate the percent ionization of acetylsalicylic acid in the solution. (2 pts)

Aspirin is acetylsalicylic acid, a monoprotic acid whose K_a value is . Does a solution of the sodium salt of aspirin in water test acidic, basic, or neutral?

Acidic, because aspirin is a weak acid.
Basic, because the anion produced from aspirin is a weak acid.
Basic, because the anion produced from aspirin is a weak base.
Neutral, because the acid was neutralized to form the sodium salt.
None of these.

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The active ingredient in aspirin is acetylsalicylic acid (HC₉H₇O₄), a monoprotic acid with K_a = 3.3 × 10^-4 at 25 °C. What is the pH of a solution obtained by dissolving two extra-strength aspirin tablets, containing 500 mg of acetylsalicylic acid each, in 250 mL of water?