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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
(0)

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)

6. Chemical Equilibrium

The Equilibrium State

6. Chemical Equilibrium

The Equilibrium State: Videos & Practice Problems

Video Lessons Practice Worksheet

Back to all problems

Back to all problems

3 of 0

Problem 3Multiple Choice

Given the reaction: 2 NO₂(g) ⇌ N₂O₄(g), with equilibrium concentrations [NO₂] = 0.5 M and [N₂O₄] = 0.2 M, calculate the equilibrium constant K.

A

K = 0.8

B

K = 0.4

C

K = 0.8

D

K = 0.8

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