Concept explainers
Videos
(a)
Interpretation:
Conjugate base of
Concept Information:
Conjugate acid-base pair:
By gain or loss of
Consider acid
Conjugate base of strong acid is a weak base.
Conjugate acid of strong base is a weak acid.
Bronsted-Lowry acid and bases:
The chemical species which is able to donate hydrogen ion to other substance known as B-L acid and the species which is able to accept hydrogen ion from another species known as B-L base.
(b)
Interpretation:
Conjugate base of
Concept Information:
Conjugate acid-base pair:
By gain or loss of
Consider acid
Conjugate base of strong acid is a weak base.
Conjugate acid of strong base is a weak acid.
Bronsted-Lowry acid and bases:
The chemical species which is able to donate hydrogen ion to other substance known as B-L acid and the species which is able to accept hydrogen ion from another species known as B-L base.
(c)
Interpretation:
Conjugate base of
Concept Information:
Conjugate acid-base pair:
By gain or loss of
Consider acid
Conjugate base of strong acid is a weak base.
Conjugate acid of strong base is a weak acid.
Bronsted-Lowry acid and bases:
The chemical species which is able to donate hydrogen ion to other substance known as B-L acid and the species which is able to accept hydrogen ion from another species known as B-L base.
(d)
Interpretation:
Conjugate base of
Concept Information:
Conjugate acid-base pair:
By gain or loss of
Consider acid
Conjugate base of strong acid is a weak base.
Conjugate acid of strong base is a weak acid.
Bronsted-Lowry acid and bases:
The chemical species which is able to donate hydrogen ion to other substance known as B-L acid and the species which is able to accept hydrogen ion from another species known as B-L base.
(e)
Interpretation:
Conjugate base of
Concept Information:
Conjugate acid-base pair:
By gain or loss of
Consider acid
Conjugate base of strong acid is a weak base.
Conjugate acid of strong base is a weak acid.
Bronsted-Lowry acid and bases:
The chemical species which is able to donate hydrogen ion to other substance known as B-L acid and the species which is able to accept hydrogen ion from another species known as B-L base.
(f)
Interpretation:
Conjugate base of
Concept Information:
Conjugate acid-base pair:
By gain or loss of
Consider acid
Conjugate base of strong acid is a weak base.
Conjugate acid of strong base is a weak acid.
Bronsted-Lowry acid and bases:
The chemical species which is able to donate hydrogen ion to other substance known as B-L acid and the species which is able to accept hydrogen ion from another species known as B-L base.
Want to see the full answer?
Check out a sample textbook solution
Chapter 14 Solutions
General Chemistry: Atoms First
- . In each of the following chemical equations, identify the conjugate acid-base pairs. a. NH3(aq)+H2O(l)NH4+(aq)+OH(aq) b. PO43(aq)+H2O(1)HPO42(aq)+OH(aq) c. C2H3O2(aq)+H2O(l)HC2H3O2(aq)+OH(aq)arrow_forwardThe 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_forwardUsing the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?arrow_forward
- 12.62 Write the formula of the conjugate acid of each of the following bases, (a) OH-, (b) NHj, (c) CHjNHt, (d) HPO/-, (e) CO.,2’arrow_forwardFor 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_forwardHydrazine, N2H4 (having the structure H2NNH2), and its derivatives have been used as rocket fuels. Draw the Lewis electron-dot formula for the hydrazine molecule. Describe the geometries expected about the nitrogen atoms in this molecule. Why would you expect hydrazine to be basic? Which substance, NH3 or N2H4, would you expect to be more basic? Why? Write the chemical equation in which hydrazine reacts with hydrochloric acids to form the salt N2H5Cl. Consider the positive ion of this salt. How does its basic character compare with that of NH3 and N2H4? Explain.arrow_forward
- Write the Lewis structures of the reactants and product of each of the following equations, and identify the Lewis acid and the Lewis base in each: (a) CS2+SHHCS3 (b) BF3+FBF4 (c) I+SnI2SnI3 (d) Al(OH)3+OHAl(OH)4 (e) F+SO3SFO3arrow_forwardWrite two BrnstedLowry acid-base reactions and show how they represent proton-transfer reactions.arrow_forwardWrite the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ionarrow_forward
- . Write the conjugate base for each of the following acids. a. HBrO b. HNO2 c. HSO3 d. CH3NH3+arrow_forwardIn the following net ionic reaction, identify each species as either a Brnsted-Lowry acid or a Brnsted -Lowry base: CH3COO(aq)+HS(aq)CH3COOH(aq)+S2(aq). Identify the conjugate of each reactant and state whether it is a conjugate acid or a conjugate base.arrow_forwardConsider a 0.33 M solution of the diprotic acid H2X. H2X H+(aq)+ HX(aq)Ka1=3.3 10 4 HX H+(aq)+ X2(aq)Ka2=9.7 10 8 Calculate the pH of the solution and estimate [HX-] and [X2-].arrow_forward
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning