1. Uncertainty/Error in Measurment
Year 11 DP Chemistry
R. Slider

2. Uncertainty and Error
All experimental measurements contain some amount of uncertainty because we are limited by the precision of the instruments that we are using. Error in measurement is introduced when instruments are calibrated incorrectly or used incorrectly.

3. Random vs. Systematic
Random Uncertainties
Systematic Error
Random uncertainty comes from fluctuations in measurements that can be greater or less than the actual result. These often stem from the limitations of the equipment being used or limitations of the experimenter (e.g. how precisely you can read a scale) These errors can never be eliminated completely, but can be reduced by using repeats
Systematic error always affects the measurement in one direction only These are due to either flaws in an instrument that is calibrated incorrectly (giving readings that are too high for example) or from experimenter error such as in parallax error where, for example, the readings are consistently too low These are reduced by good experimental design
Have students brainstorm/list other examples of these. More in Brown, Ford HL Chemistry text, p. 424.

4. Reporting Uncertainty
Analogue instruments
Digital instruments
Instruments such as thermometers and measuring cylinders have various divisions The uncertainty of an analogue scale is +/- half of the smallest division
Digital readouts such as electronic balances have various precision levels The uncertainty of a digital scale is +/- the smallest scale division

5. Precision and Accuracy
Precision refers to how close repeated measurements are to one another (has the least uncertainty/random errors)
Accuracy refers to how close a value is to an accepted (true) value. Small systematic errors lead to accurate measurements.

6. Precision and Accuracy
Example: Two groups are determining the gas constant value (8.314 J/mol K). Results are: Group A: 8.537; 8.487; 8.598; 8.492; (Avg=8.517) Group B: 8.13; 7.94; 8.44; 8.54; 8.22 (Avg =8.25) Which group is more precise? Group A (less variation/uncertainty) Which group is more accurate? Group B (closer to accepted value)
See Green, Damji Chemistry text, p 291 for complete “Extension” example and introduction to “consistency” and std deviation calculation

7. Significant Figures
Significant figures (s.f.) establish the precision of a number.
The rules:
All non-zero numbers are ALWAYS significant (e.g. 1, 2, 3...)
Zeroes between 2 non-zero or 2 significant numbers are ALWAYS significant.
Zeros used to locate a decimal point (placeholders) are NOT significant
Zeroes which are SIMULTANEOUSLY to the right of the decimal point AND at the end of the number are ALWAYS significant
The last significant figure on the right is the one which is somewhat uncertain
For operations:
When adding/subtracting, the number of digits to the right of the decimal is the same as the number with the fewest digits to the right
When multiplying/dividing, the number of s.f. in the answer is the same as the least number of s.f. in any of the original numbers.

8. Significant Figures Examples
Determine the number of s.f. in each of these numbers and the rule # that led you to that conclusion. Tabulate results.
48,923
3.967
900.06
0.0004
8.1000
3,000,000
10.0

9. Significant Figures Examples
Number
# Significant figures
Rule
48,923 5 1
3.967 4
900.06
1,2
0.0004
1,3
8.1000
1,4 6
1,2,4
3,000,000
unspecified
10.0 3

10. Absolute and % Uncertainty
Once you have determined the uncertainty of a single measurement (as a ± value) you can easily determine % uncertainty. %unc = abs unc/value x 100 For example: You determine the mass of a sample to be ±0.01g. Your absolute uncertainty is 0.01g and % uncertainty = (o.o1÷24.56) x 100 = o.04%

11. Propagating Uncertainty
When multiple readings are combined, the following rules apply:
Addition/subtraction – add the absolute uncertainties
Multiplication/division – add the % uncertainties
See example in Green, Damji textbook, p. 292

12. Propagating Uncertainty Problem
X = A(B-C) If : A=123±0.5 B=12.7±0.2 C=4.3±0.1 Determine the value, absolute uncertainty and %uncertainty of X. State the final answer with the correct significant figures.
From Green, Damji, pp

13. Propagating Uncertainty Solution
X = A(B-C)
If :
A=123±0.5 B=12.7±0.2 C=4.3±0.1
X = 123 x (12.7 – 4.3) = (not rounded yet)
Step 1: For B-C, uncertainties are added: = 0.3
Step 2: % unc (A) = 0.5/123 x 100 = 0.407%
Step 3: % unc (B-C) = 0.3/8.4 x 100 = 3.571%
Step 4: % unc (X) = 3.571% % = 3.978%
Step 5: abs unc = x 3.978/100 = 41.1
So,
X = 1030 ± 40