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1. Chemical Measurements(0)

SI Units
(0)

Metric Prefixes
(0)

Chemical Concentrations
(0)

Volumetric Analysis
(0)

Volumetric Titrations
(0)

2. Tools of the Trade(0)

Safety & Labels
(0)

Buoyancy
(0)

Thermal Dependency
(0)

Volumetric Instruments
(0)

Filtration & Evaporation
(0)

3. Experimental Error(0)

Significant Figures
(0)

Addition and Subtraction Operations
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Multiplication and Division Operations
(0)

Logarithm and Anti-Logarithm Operations
(0)

Precision and Accuracy
(0)

Types of Errors
(0)

Uncertainty
(0)

4 & 5. Statistics, Quality Assurance and Calibration Methods(0)

Mean Evaluation
(0)

The Gaussian Distribution
(0)

Confidence Intervals
(0)

Hypothesis Testing (t-Test)
(0)

Analysis of Variance (f-Test)
(0)

Detection of Gross Errors
(0)

6. Chemical Equilibrium(0)

The Equilibrium State
(0)

The Reaction Quotient
(0)

Le Chatelier's Principle
(0)

Chemical Thermodynamics: Enthalpy
(0)

Chemical Thermodynamics: Entropy
(0)

Chemical Thermodynamics: Gibbs Free Energy
(0)

Solubilty Product Constant
(0)

Protic Acids and Bases
(0)

The pH Scale
(0)

Acid Strength
(0)

7. Activity and the Systematic Treatment of Equilibrium(0)

Ionic Strength of Soluble Salts
(0)

Activity Coefficients
(0)

pH Revisited
(0)

8. Monoprotic Acid-Base Equilibria(0)

Arrhenius Acids and Bases
(0)

Bronsted-Lowry Acids and Bases
(0)

Lewis Acids and Bases
(0)

Auto-Ionization
(0)

Ka and Kb of compounds
(0)

Weak Acid-Base Equilibria
(0)

Ionic Salts of Weak Acids and Bases
(0)

Buffers
(0)

9. Polyprotic Acid-Base Equilibria(0)

Diprotic Acids and Bases
(0)

Polyprotic Acids and Bases
(0)

Diprotic Buffers
(0)

Polyprotic Buffers
(0)

Principal Species
(0)

Isoelectric and Isoionic pH
(0)

10. Acid-Base Titrations(0)

Strong Acid-Strong Base Titrations
(0)

Weak Acid-Strong Base Titrations
(0)

Weak Base-Strong Acid Titrations
(0)

Diprotic Acid Titrations
(0)

Polyprotic Titrations
(0)

11. EDTA Titrations(0)

Metal Chelate Complexes
(0)

EDTA
(0)

EDTA Titration Curves
(0)

12. Advanced Topics in Equilibrium(0)

General Approach to Acid-Base Systems
(0)

Fractional Compositions and Concentrations
(0)

Dependence of Solubility on pH
(0)

13. Fundamentals of Electrochemistry(0)

Basic Concepts
(0)

Electrochemical Cells
(0)

Standard Potentials
(0)

Nernst Equation
(0)

Standard Cell Potential & the Equilibrium Constant
(0)

14. Electrodes and Potentiometry(0)

Potentiometry
(0)

Reference Electrodes
(0)

Junction Potential
(0)

Glass Electrodes and pH Measurements
(0)

15. Redox Titrations(0)

Titrations and Titration Curves
(0)

The End Point
(0)

Analyte Oxidation State
(0)

Oxidizing Agents
(0)

16. Electroanalytical Techniques(0)

Fundamentals of Electrolysis
(0)

Gravimetric Analysis
(0)

Coulometry
(0)

Voltammetry
(0)

17. Fundamentals of Spectrophotometry(0)

Properties of Light
(0)

Absorption of Light
(0)

Measuring Absorbance
(0)

Beer's Law
(0)

Instrument Components
(0)

8. Monoprotic Acid-Base Equilibria

Ka and Kb of compounds

8. Monoprotic Acid-Base Equilibria

Ka and Kb of compounds: Videos & Practice Problems

Video Lessons Practice Worksheet

Ka and Kb of compounds Practice Problems

19 problems

Problem 1Multiple Choice

What does the term K_a represent in the context of weak acids?

Problem 2Multiple Choice

Which of the following statements is true about K_b?

Problem 3Multiple Choice

How does a higher K_a value affect the strength of a weak acid?

Problem 4Multiple Choice

What does a low K_b value suggest about the strength of a weak base?

Problem 5Multiple Choice

Given a K_a value of 1.8 x 10^-5 for a weak acid, calculate its pK_a.

Problem 6Multiple Choice

If the K_a of a weak acid is 3.2 x 10^-7, what is its pK_a?

Problem 7Multiple Choice

Which component is ignored in the equilibrium expression for weak acids and bases?

Problem 8Multiple Choice

What is the equilibrium expression for a weak acid HA in water?

Problem 9Multiple Choice

According to Bronsted-Lowry theory, what role does water play when a weak acid donates an H⁺ ion?

Problem 10Multiple Choice

In the Bronsted-Lowry theory, what happens when a weak base accepts an H⁺ ion from water?

Problem 11Multiple Choice

Using an ICE chart, calculate the equilibrium concentration of H₃O⁺ for a weak acid HA with initial concentration 0.1 M and K_a = 1.0 x 10^-5.

Problem 12Multiple Choice

If the K_a of a weak acid is 4.0 x 10^-6, what is the K_b of its conjugate base at 25°C?

Problem 13Multiple Choice

Given a K_b value of 1.5 x 10^-5 for a weak base, calculate the K_a of its conjugate acid at 25°C.

Problem 14Multiple Choice

Which acid is stronger: Acid A with K_a = 1.0 x 10^-3 or Acid B with K_a = 5.0 x 10^-5?

Problem 15Multiple Choice

Given two acids, Acid X with K_a = 2.0 x 10^-4 and Acid Y with K_a = 8.0 x 10^-6, which produces more H⁺ ions in solution?

Problem 16Multiple Choice

Why do weak acids and bases establish equilibrium in solution?

Problem 17Multiple Choice

What is the implication of equilibrium establishment for product formation in weak acid solutions?

Problem 18Multiple Choice

Given the K_a values of two acids, Acid C (K_a = 3.0 x 10^-4) and Acid D (K_a = 1.0 x 10^-6), determine which acid is stronger and explain why.

Problem 19Multiple Choice

If the K_a of Acid E is 2.5 x 10^-5 and the K_a of Acid F is 7.5 x 10^-7, which acid is weaker and why?

Auto-Ionization Practice Problems Weak Acid-Base Equilibria Practice Problems

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