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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

Strong Acid-Strong Base Titrations

Weak Acid-Strong Base Titrations

Weak Base-Strong Acid Titrations

Diprotic Acid Titrations

Polyprotic Titrations

Metal Chelate Complexes

EDTA

EDTA Titration Curves

General Approach to Acid-Base Systems

Fractional Compositions and Concentrations

Dependence of Solubility on pH

Basic Concepts

Electrochemical Cells

Standard Potentials

Nernst Equation

Standard Cell Potential & the Equilibrium Constant

Potentiometry

Analytical Chemistry Final - Part 1 of 2

After adding 310 mL of 0.050 M HNO3 to 150 mL of 0.100 M NaOH, what is the pH of the solution?

After adding 310 mL of 0.050 M HNO₃ to 150 mL of 0.100 M NaOH, what is the pH of the solution?