The volume of the solution I am making is 2.5 L. To measure this volume I will use a large graduated cylinder that can measure volume to ± 10 mL. What is the absolute uncertainty in my concentration?
Table of contents
- 1. Chemical Measurements1h 50m
- 2. Tools of the Trade1h 17m
- 3. Experimental Error1h 52m
- 4 & 5. Statistics, Quality Assurance and Calibration Methods1h 57m
- 6. Chemical Equilibrium3h 41m
- 7. Activity and the Systematic Treatment of Equilibrium1h 0m
- 8. Monoprotic Acid-Base Equilibria1h 53m
- 9. Polyprotic Acid-Base Equilibria2h 17m
- 10. Acid-Base Titrations2h 37m
- 11. EDTA Titrations1h 34m
- 12. Advanced Topics in Equilibrium1h 16m
- 13. Fundamentals of Electrochemistry2h 19m
- 14. Electrodes and Potentiometry41m
- 15. Redox Titrations1h 14m
- 16. Electroanalytical Techniques57m
- 17. Fundamentals of Spectrophotometry50m
3. Experimental Error
Uncertainty
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Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Based on the previous example calculate the molarity value for each student if they dissolve 0.300 (± 0.03) moles of analyte.
A
1.5 ± 0.2 M for both
B
1.5 ± 0.2 M for student A and 1.5 ± 0.1 M for student B
C
1.5 ± 0.1 M for student A and 1.5 ± 0.2 M for student B
D
1.5 ± 0.04 M for student A and 1.5 ± 0.01 M for student B

1
Identify the formula for molarity, which is M = \frac{n}{V}, where M is the molarity, n is the number of moles, and V is the volume in liters.
Determine the number of moles of the analyte, which is given as 0.300 moles with an uncertainty of ± 0.03 moles.
Assume a volume for the solution based on the context or previous example, as it is not provided in the problem. This volume should be in liters.
Calculate the molarity by dividing the number of moles by the volume in liters. Consider the uncertainty in the number of moles when calculating the uncertainty in molarity.
Compare the calculated molarity and its uncertainty with the given options to determine which matches the calculated values for each student.
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