🏷️ LIMITED TIME OFFER: GET 20% OFF GRADE+ YEARLY SUBSCRIPTION →
Log in
HomeClass Notes1,200,000US530,000

CH 302 Lecture Notes - Lecture 1: Conjugate Acid, Amphoterism, Acid Strength

26 views7 pages
School
UT-Austin
Department
Chemistry
Course
CH 302
Professor
Fakhreddine Fatima

For unlimited access to Class Notes, a Class+ subscription is required.

Document Summary

The strength of an acid is determined by its degree of ionization. A strong acid completely ionizes and a weak acid ionizes slightly. In an aqueous solution, the ionization reaction of a weak acid, ha, is represented by the following equation: The equilibrium constant for this reaction is ka = A strong acid completely ionizes in water and therefore, its ka. The conjugate base of a strong acid is very weak to the point where it is not interested in accepting a proton! Therefore, the ionization of a strong acid in water is not reversible. The conjugate base of a weak acid is not very weak and easily accepts a proton. Therefore, the ionization of a weak acid in water is reversible. The conjugate base of the acid ha is a-. A stronger acid has a -------- conjugate base. Question: compare the strength of the conjugate bases of hf, hcl and.

Get access

Grade+20% off
$8 USD/m$10 USD/m
Billed $96 USD annually
Grade+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
40 Verified Answers
Class+
$8 USD/m
Billed $96 USD annually
Class+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
30 Verified Answers

Related Documents

CH 302 Lecture Notes - Lecture 1: Weak Base, Ionic Compound, Sodium Chloride
periwinklepug717
CH 302 Lecture Notes - Lecture 1: Houghton Mifflin Harcourt, Titration Curve, Bromothymol Blue
periwinklepug717
CH 302 Lecture Notes - Lecture 1: Solubility Equilibrium, Magnesium Fluoride, Ionic Compound
periwinklepug717

Related Questions

Which of the follow statements is FALSE?

a Group 1A and Heavy Group 2A metal hydroxides are classified as strong bases.
b When a strong acid dissolves in water it ionizes completely.
c When a weak acid dissolves in water it ionizes completely.
d The conjugate of a strong base is a negligible conjugate acid.
e When a strong base dissolves in water it ionizes completely.

For conjugate acid-base pairs, how are Ka and Kb related?

Consider the reaction of acetic acid in water.

 

where  

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 1x106, 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 acid 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.)

For conjugate acid-base 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 × 10−5

  1. Which two bases are competing for the proton?
  2. Which is the stronger base?
  3. 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.
  4. 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 the 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.)