Aspirin is a weak acid with a pk, of 3.5. It is absorbed into the blood through the cells lining thestomach and the small intestine. Absorption requires passage through the plasma membrane, therate of which is determined by the polarity of the molecule, charged and polar molecules tend to passmore slowly, whereas neutral hydrophobic molecules pass rapidly. The pH of the stomach contents isabout 1.5, and the pH of the contents of the small intestine is about 6. Is the aspirin absorbed into thebloodstream from the stomach or the small intestine? Clearly justify your choice.ОНAcetylsalicylic Acid(Aspirin)

Acid is a compound that donates proton and base is a compound that accepts proton. The strength of…

Answered: Aspirin is a weak acid with a pk, of…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 58P

See similar textbooks

Similar questions

. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
Consider a weak organic base (nonelectrolyte) with molar mass 281 g/mol. An aqueous solution of the base has a pH of 8.73 and an osmotic pressure of SS mm Hg at 25C. What is Kb for the weak base?
In humans, blood pH is maintained within a narrow range:acidosis occurs if the blood pH is below 7.35, and alkalosis oc-curs if the pH is above 7.45. Given that the pKᵥᵥ of blood is 13.63 at 37°C (body temperature), what is the normal range of [H₃O⁺]and of [OH⁻] in blood?
A chemist takes 8.579 mL of liquid acetic acid, CH₃COOH (molar mass: 60.052 g/mol) with 1.05 g/mL density and mix it with 12.305 g of solid sodium acetate, CH₃COONa (molar mass: 82.0343g/mol) and prepare an aqueous solution of 1.0 L by adding required amount of water. (Acidity constant of CH₃COOH is 1.8x10⁻⁵) What would the pH of the solution be if 0.020 mol HCl added to the solution in a? What would the pH of the solution be if 0.15 mol HCl added to the solution in a? What would the pH of the solution be if 0.17 mol HCl added to the solution in a?.
Rain with a pH below 5.6 is considered acid rain. The principal cause of acid rain is coal-burning electrical power plants (sulfurous and sulfuric acids are formed in the atmosphere from this). Any combustion reaction that produces high temperature can also produce acid rain (nitrous and nitric acid are produced in the atmosphere from this). Thus, automotive engines are also an important contributor to acid rain. Acid rain harms both living and nonliving things in a variety of ways. What solution/s can you propose to combat acid rain?
Due to the pandemic Covid-19, the uses of hand sanitizers are very important among us. Predict and explain the colour of the solution and pH value when red cabbage indicator was added to the hand sanitizers.
Normally, the volume of gastric acid in the human stomach ranges from 20. mL to 100. mL and a pH between 1.5 and 3.5 Using the information above, what is the minimum concentration (in M) of HCl for the normal human stomach? Please provide all the work so I can fully understand the arrical of the solution, thank you.
when chlorine gas is added to water during the disinfection of drinking water, it hydrolyzes with the water to form HOCL. The disinfection power of the acid HOCL is 88 times better than its conjugate base, OCl-. The pKa for HOCl is 7.5. (a) what percentage of the total disinfection power exists in the acid form at pH of 6?
Let's say a weak acid A has ph of 4.56, its molar conductivity is 5.32x10^7 microsiemens/Molarity times cm and conductivity at infinite dilution is 6.12x10^8 microsiemens/Molarity times cm. Find the initial concentration, ionization constant, and fraction ionized of A.
A chemist takes 8.579 mL of liquid acetic acid, CH₃COOH (molar mass: 60.052 g/mol) with 1.05 g/mL density and mix it with 12.305 g of solid sodium acetate, CH₃COONa (molar mass: 82.0343g/mol) and prepare an aqueous solution of 1.0 L by adding required amount of water. (Acidity constant of CH₃COOH is 1.8x10⁻⁵) a) What is the pH of such solution?b) What would the pH of the solution be if 0.020 mol NaOH added?c) What would the pH of the solution be if 0.15 mol NaOH added to the solution in a?d) What would the pH of the solution be if 0.17 mol NaOH added to the solution in a? e) What would the pH of the solution be if 0.020 mol HCl added to the solution in a? f) What would the pH of the solution be if 0.15 mol HCl added to the solution in a?g) What would the pH of the solution be if 0.17 mol HCl added to the solution in a?
A chemist takes 8.579 mL of liquid acetic acid, CH₃COOH (molar mass: 60.052 g/mol) with 1.05 g/mL density and mix it with 12.305 g of solid sodium acetate, CH₃COONa (molar mass: 82.0343g/mol) and prepare an aqueous solution of 1.0 L by adding required amount of water. (Acidity constant of CH₃COOH is 1.8x10⁻⁵) a) What is the pH of such solution?. Single line text.
What is the pH of a solution that is prepared by dissolving 7.50 grams of pyruvic acid (formula weight = 88.06 grams/mol) and 8.95 grams of sodium pyruvate (formula weight = 90.04 grams/mole) in water and diluting to 500.00 mL? The Ka for pyruvic acid is 0.00324.

SEE MORE QUESTIONS

Recommended textbooks for you

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS