Question
In: Chemistry
An aspirin tablet (acetylsalicylic acid, pKa = 3.49, molecular weight = 180.15) was taken orally with...
- An aspirin tablet (acetylsalicylic acid, pKa = 3.49, molecular weight = 180.15) was taken orally with cold water to make a solution of aspirin in the stomach fluids of 0.00167 M. The cold water produced a temperature in the stomach temporarily of 25 °C. What is the percentage of aspirin in the ionized form in the stomach in which the pH of the fluid is 3.2?
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queen_honey_blossom answered 1 year agoRelated Solutions
A Doctor prescribes a aspirin 134 mg tablet to be taken orally, 0.8 mg of sublingual...
A Doctor prescribes a aspirin 134 mg tablet to be taken
orally, 0.8 mg of sublingual nitroglycerin should be taken after.
What should be some monitoring parameters that someone can follow
to ensure efficacy and safety of the medication use?
A typical aspirin tablet contains 319 mg acetylsalicylic acid. Calculate the pH of a solution that...
A typical aspirin tablet contains 319 mg acetylsalicylic acid.
Calculate the pH of a solution that is prepared by dissolving two
aspirin tablets in enough water to make one cup (249 mL) of
solution. Assume the aspirin tablets are pure acetylsalicylic acid,
Ka=3.3x10^-4.
The lab experiment is the synthesis of aspirin. The product will be acetylsalicylic acid (aspirin) and...
The lab experiment is the synthesis of aspirin. The product will
be acetylsalicylic acid (aspirin) and the by-product will be acetic
acid. How will you separate the by-product from the desired
product? is it from recrystallization and then vacuum
filtration?
Acetylsalicylic acid, also known as Aspirin, has a formula of C9H8O4 and is a weak acid...
Acetylsalicylic acid, also known as Aspirin, has a formula of
C9H8O4 and is a weak acid with a Ka of 3.0 x 10-4. It has been
suggested that a regular low-dose regimen of “baby aspirin”,
approximately 81 mg, may help reduce the risk of a heart
attack.
a. Determine the molarity of acetylsalicylic acid in a solution
of “baby aspirin” if a tablet containing 81.0 mg of acetylsalicylic
acid is dissolved in a cup of water (8.0 fluid ounces). Note:...
A typical aspirin tablet contains 424 mg of aspirin (C9O4H8), a monoprotic acid with a Ka=...
A typical aspirin tablet contains 424 mg of aspirin (C9O4H8), a
monoprotic acid with a Ka= 2.8x10^-4. A monoprotic acid donates a
single proton. If you dissolve two aspirin tablets in a 300 mL
glass of water, what is the pH of the solution?
Part A Aspirin (acetylsalicylic acid, C9H8O4) is a weak monoprotic acid. To determine its acid-dissociation constant,...
Part A
Aspirin (acetylsalicylic acid, C9H8O4) 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 2.60?
Express your answer numerically using two significant
figures.
Part B
A 0.100 M solution of ethylamine (C2H5NH2) has a pH of
11.87. Calculate the Kb for ethylamine.
Express your answer numerically...
Part A Aspirin (acetylsalicylic acid, C9H8O4) is a weak monoprotic acid. To determine its acid-dissociation constant,...
Part A
Aspirin (acetylsalicylic acid, C9H8O4) 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 2.62?
Express your answer numerically using two significant
figures.
Answer I got: 3.16 x 10^-4 (incorrect) this is the reason why:
You used the initial concentration of aspirin in the Ka expression....
Part A Aspirin (acetylsalicylic acid, C9H8O4) is a weak monoprotic acid. To determine its acid-dissociation constant,...
Part A
Aspirin (acetylsalicylic acid, C9H8O4) 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
pHof the solution was 2.62?
Express your answer numerically using two significant
figures.
Ka=
Part B
A 0.100 M solution of ethylamine (C2H5NH2) has a pH of
11.87. Calculate the Kb for ethylamine.
Express your answer numerically...
Part A Aspirin (acetylsalicylic acid, C9H8O4) is a weak monoprotic acid. To determine its acid-dissociation constant,...
Part A
Aspirin (acetylsalicylic acid, C9H8O4) 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 2.62?
Part B
A 0.100 M solution of ethylamine (C2H5NH2) has a pH of
11.87. Calculate the Kb for ethylamine.
The active ingredient in aspirin is acetylsalicylic acid (HC9H7O4) , a monoprotic acid with Ka=3.3×10−4 at...
The active ingredient in aspirin is acetylsalicylic acid
(HC9H7O4) , a monoprotic acid with Ka=3.3×10−4 at
25 ∘C .
What is the pH of a solution obtained by dissolving two
extra-strength aspirin tablets, containing 510 mg of
acetylsalicylic acid each, in 300 mL of water?
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