Practice: Calculate the absolute uncertainty from the given problem.
6.77 (± 5.6%)
Uncertainty can be thought of as the range (+/-) that is associated with any given value.
Types of Uncertainty
Concept #1: With any given value there is some level of uncertainty, which can be classified as absolute, relative or percent.
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Example #1: Calculate the relative and percent relative uncertainty from the given problem.
3.25 (± 0.03)
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Propagation of Uncertainty from Random Error
Concept #2: With any calculations dealing with uncertainty we will have to take into account the Real Rule.
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Concept #3: For addition and subtraction, the uncertainty in our final answer is determined from each individual absolute uncertainty.
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Example #2: For multiplication and division, we must first convert the absolute uncertainties into percent relative uncertainties.
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Example #3: Determine the absolute and relative uncertainty to the following addition problem.
1.511 (± 0.02) + 2.53 (± 0.01) + 0.987 (± 0.01)
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Practice: Determine the absolute and relative uncertainty to the following addition and subtraction problem.
8.88 (± 0.03) - 3.29 (± 0.10) + 6.43 (± 0.001)
Example #4: Determine the absolute and relative uncertainty to the following multiplication and division problem.
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Practice: Determine the absolute and relative uncertainty to the following multiplication and division problem.
1.12(±0.01) x 0.546 (±0.01) / 3.12(±0.02) x 1.12 (0.03)
Example #5: Two students wish to prepare a stock solution for their lab experiment. Student A uses an un-calibrated pipet that delivers 50.00 (± 0.02) mL to deliver 200 mL to a container. Student B uses a calibrated pipet that delivers 40.00 (± 0.01) mL to deliver 200 mL to a container.
a) Calculate the absolute uncertainty in each of their deliveries.
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Practice: Based on the previous example calculate the molarity value for each student if they dissolve 0.300 (± 0.03) moles of analyte.
Example #6: A “Class A” 50-mL buret is certified by the manufacturer to deliver volumes within a “tolerance” (i.e. uncertainty) of ± 0.05 mL. The smallest graduations on the buret are 0.1 mL. You use the buret to titrate a solution, adding 5 successive volumes to the solution. The following volumes were added:
Addition Volume (mL)
1 6.73
2 8.92
3 7.52
4 2.48
5 5.15
What is the total volume added, and what is the uncertainty associated with this final volume?
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Example #7: A Class A 250 mL volumetric flask has an uncertainty of ± 0.15 mL, and a 50 mL volumetric pipet has an uncertainty of ± 0.05 mL. If I fill a 250 mL volumetric flask to the line and remove four 50 mL aliquots with my volumetric pipet, I should have 50 mL of solution remaining in the flask. What is the absolute and relative uncertainty in the remaining volume?
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Practice: I am making a 0.1 M KCl (molar mass 74.551) solution for an experiment. To measure the mass of the KCl, I will use an analytical balance that is only accurate to ± 0.01 g. I place a piece of paper on the balance and set the tare to read 0.00. I then put the KCl on the balance until it reads 6.79 g. What is the uncertainty in this mass?
Practice: 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?
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