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Need help with titrations, spectroscopy, or chromatography? Analytical chemistry concepts are simplified to support labs and problem sets.

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1. Chemical Measurements

2. Tools of the Trade

3. Experimental Error

4 & 5. Statistics, Quality Assurance and Calibration Methods

6. Chemical Equilibrium

7. Activity and the Systematic Treatment of Equilibrium

8. Monoprotic Acid-Base Equilibria

9. Polyprotic Acid-Base Equilibria

10. Acid-Base Titrations

11. EDTA Titrations

12. Advanced Topics in Equilibrium

13. Fundamentals of Electrochemistry

14. Electrodes and Potentiometry

15. Redox Titrations

16. Electroanalytical Techniques

17. Fundamentals of Spectrophotometry

[BOOK ANALCHEM] CLUTCH - 1e

Le Chatelier's Principle

Chemical Thermodynamics: Enthalpy

Chemical Thermodynamics: Entropy

Chemical Thermodynamics: Gibbs Free Energy

Solubilty Product Constant

Protic Acids and Bases

The pH Scale

Acid Strength

Ionic Strength of Soluble Salts

Activity Coefficients

pH Revisited

Arrhenius Acids and Bases

Bronsted-Lowry Acids and Bases

Lewis Acids and Bases

Auto-Ionization

Ka and Kb of compounds

Weak Acid-Base Equilibria

Ionic Salts of Weak Acids and Bases

Buffers

Diprotic Acids and Bases

Polyprotic Acids and Bases

Diprotic Buffers 

Polyprotic Buffers

Principal Species

Isoelectric and Isoionic pH

Analytical Chemistry Midterm - Part 2 of 2

Using the Henderson-Hasselbalch equation, calculate the pH of a buffer solution containing 0.2 M formic acid (pKa = 3.75) and 0.1 M sodium formate.

Using the Henderson-Hasselbalch equation, calculate the pH of a buffer solution containing 0.2 M formic acid (pK_a = 3.75) and 0.1 M sodium formate.