Ch.3 - Experimental ErrorWorksheetSee all chapters
All Chapters
Ch.1 - Chemical Measurements
Ch.2 - Tools of the Trade
Ch.3 - Experimental Error
Ch.4 + 5 - Statistics, Quality Assurance and Calibration Methods
Ch.6 - Chemical Equilibrium
Ch.7 - Activity and the Systematic Treatment of Equilibrium
Ch.8 - Monoprotic Acid-Base Equilibria
Ch.9 - Polyprotic Acid-Base Equilibria
Ch.10 - Acid-Base Titrations
Ch.11 - EDTA Titrations
Ch.12 - Advanced Topics in Equilibrium
Ch.13 - Fundamentals of Electrochemistry
Ch.14 - Electrodes and Potentiometry
Ch.15 - Redox Titrations
Ch.16 - Electroanalytical Techniques
Ch.17 - Fundamentals of Spectrophotometry
BONUS: Chemical Kinetics
Sections
Significant Figures
Addition and Subtraction Operations
Multiplication and Division Operations
Logarithm and Anti-Logarithm Operations
Precision and Accuracy
Types of Errors
Uncertainty
Propagation of Uncertainty: Triangular Distribution

The efficacy of any calculation or experiment is based on the principles of precision and accuracy

Precision, Accuracy and Error

Example #1: The principles of precision and accuracy are essential in the minimization of error in all experimental calculations.  

Example #2: A student must measure the weight of a sodium bicarbonate compound and obtains the following measurements: 23.12 g, 23.26 g, 23.08 g and 23.17g. If the true weight of the compound is 18.01 g what can be said about the student’s results?

a) They are accurate and precise.

b) They are accurate, but not precise.

c) They are not accurate, but precise.

d) They are neither accurate or precise. 

As the number and complexity of calculations increases it will become more essential to rely on standard deviation to determine their precision.