Concept explainers
There is a buffer system in blood
(a) Calculate the
(b) What percentage of the
(c) What percentage of the
(a)
Interpretation:
The ratio
Concept introduction:
Henderson-Hasselbalch equation is an equation useful to determine the pH of any solution when any acid’s aqueous solution is related to its acid dissociation constant.
Buffer equation is considered as an equation when ionization of a weak acid in the water occurs resulted into the hydronium ion and the conjugate base of that acid.
Answer to Problem 36QAP
The ratio
Explanation of Solution
For
For acid-dissociation constant of the given
For
Now, we need to determine the concentration of
In equation (1), we are substituting the value of
(b)
Interpretation:
The percentage
Concept introduction:
Henderson-Hasselbalch equation is an equation useful to determine the pH of any solution when any acid’s aqueous solution is related to its acid dissociation constant.
Buffer equation is considered as an equation when ionization of a weak acid in the water occurs resulted in the hydronium ion and the conjugate base of that acid.
Answer to Problem 36QAP
Explanation of Solution
The pH of the buffer system as 6.80and the ratio of the concentration of
Now, let us take the concentration of
We have the dissociation equation of
As per the Henderson-Hasselbalch equation,
Now, the percentage of
(c)
Interpretation:
The percentage
Concept introduction:
Henderson-Hasselbalch equation is an equation useful to determine the pH of any solution when any acid’s aqueous solution is related to its acid dissociation constant.
Buffer equation is considered as an equation when ionization of a weak acid in the water occurs resulted in the hydronium ion and the conjugated base of that acid.
Answer to Problem 36QAP
Explanation of Solution
We have the pH of the buffer system as 7.80 and the ratio of the concentration of
Now, let us take the concentration of
We have the dissociation equation of
As per the Henderson-Hasselbalch equation,
Now, the percentage of
Want to see more full solutions like this?
Chapter 14 Solutions
CHEMISTRY:PRIN.+REACTIONS-OWLV2 ACCESS
- For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)arrow_forwardA chemist wanted to determine the concentration of a solution of lactic acid, HC3H5O3. She found that the pH of the solution was 2.60. What was the concentration of the solution? The Kd of lactic acid is 1.4 104.arrow_forward8-53 Write equations to show what happens when, to a buffer solution containing equimolar amounts of CH3COOH and CH3COO-, we add: (a) H3O (b) OH-arrow_forward
- The pH of a 0.10-M solution of propanoic acid, CH3CH2COOH, a weak organic acid, is measured at equilibrium and found to be 2.93 at 25 °C. Calculate the Ka of propanoic acid.arrow_forwardA solution of acetic acid, HC2H3O2, on a laboratory shelf was of undetermined concentration. If the pH of the solution was found to be 2.57, what was the concentration of the acetic acid? The Ka of acetic acid is 1.7 105.arrow_forwardMethylammonium chloride is a salt of methylamine, CH3NH2. A 0.10 M solution of this salt has a pH of 5.82. a Calculate the value for the equilibrium constant for the reaction CH3NH3++H2OCH3NH2+H3O+ b What is the Kb value for methylamine? c What is the pH of a solution in which 0.450 mol of solid methylammonium chloride is added to 1.00 L of a 0.250 M solution of methylamine? Assume no volume change.arrow_forward
- Barbituric acid, HC4H3N2O3, is used to prepare barbiturates, a class of drugs used as sedatives. A 325-mL aqueous solution of barbituric acid has a pH of 2.34 and contains 9.00 g of the acid. What is Ka for barbituric acid?arrow_forwardExplain why the pH does not change significantly when a small amount of an acid or a base is added to a solution that contains equal amounts of the base NH3 and a salt of its conjugate acid NH4CI.arrow_forwardThe base ethylamine (CH3CH2NH2) has a Kb of. A closely related base, ethanolamine(HOCH2CH2NH2), has a Kb of 3.2105. (a) Which of the two bases is stronger? (b) Calculate the pH of a 0.10M solution of the strong base?arrow_forward
- Calculate the maximum concentration of Mg2+ (molarity) that can exist in a solution of pH 12.00.arrow_forwardTartaric acid is a weak diprotic fruit acid with Ka1 = 1.0 103 and Ka2 = 4.6 105. a Letting the symbol H2A represent tartaric acid, write the chemical equations that represent Ka1 and Ka2. Write the chemical equation that represents Ka1 Ka2. b Qualitatively describe the relative concentrations of H2A, HA, A2, and H3O+ in a solution that is about 0.5 M in tartaric acid. c Calculate the pH of a 0 0250 M tartaric acid solution and the equilibrium concentration of [H2A]. d What is the A2 concentration in solutions b and c?arrow_forwardIonization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid-ionization constant for the second proton is 1.1 102. a What would be the approximate hydronium-ion concentration in 0.100 M H2SO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.100 M H2SO4, accounting for the ionization of both protons.arrow_forward
- General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning