Topic 11: Measurement and Data Processing Honors Chemistry Mrs. Peters Fall 2014

11.1 Uncertainty and Error in Measurement Measurement is important in chemistry. Many different measurement apparatus are used, some are more appropriate than others. Have out each of the different types of measurement devices, have students walk around and record what they notice about the increments and measurements of each item.

11.1 Uncertainty and Error in Measurement Example: You want to measure 25 cm3 (25 ml) of water, what can you use? Beaker, volumetric flask, graduated cylinder, pipette, buret, or a balance All of these can be used, but will have different levels of uncertainty. Which will be the best? Have out each of the different types of measurement devices, have students walk around and record what they notice about the increments and measurements of each item.

A & S 1. Systematic Errors Systematic Error: occur as a result of poor experimental design or procedure. Cannot be reduced by repeating experiment Can be reduced by careful experimental design

A & S 1. Systematic Errors Systematic Error Example: measuring the volume of water using the top of the meniscus rather than the bottom Measurement will be off every time, repeated trials will not change the error

A & S 1. Random Error Random Error: imprecision of measurements, leads to value being above or below the “true” value. Causes: Readability of measuring instrument Effects of changes in surroundings (temperature, air currents) Insufficient data Observer misinterpreting the reading Can be reduced by repeating measurements

A & S 1: Random and Systematic Error Systematic and Random Error Example Random: estimating the mass of Magnesium ribbon rather than measuring it several times (then report average and uncertainty) 0.1234 g, 0.1232 g, 0.1235 g, 0.1234 g, 0.1235 g, 0.1236 g Avg Mass= 0.1234 + 0.0002 g

A & S 1: Random and Systematic Error Systematic and Random Error Example Systematic: The balance was zeroed incorrectly with each measurement, all previous measurements are off by 0.0002 g 0.1236 g, 0.1234 g, 0.1237 g, 0.1236 g, 0.1237 g, 0.1238g Avg Mass = 0.1236

A & S 8. Distinguish between precision and accuracy in evaluating results Precision: how close several experimental measurements of the same quantity are to each other how many sig figs are in the measurement. Smaller random error = greater precision

Accuracy: how close a measured value is to the correct value A & S 8. Distinguish between precision and accuracy in evaluating results Accuracy: how close a measured value is to the correct value Smaller systematic error = greater accuracy Example: masses of Mg had same precision, 1st set was more accurate.

U 5. Reduction of Random Error Random errors can be reduced by Use more precise measuring equipment Repeat trials and measurements (at least 3, usually more)

A & S 2. Uncertainty Range (±) Random uncertainty can be estimated as half of the smallest division on a scale Always state uncertainty as a ± number

A & S 2. Uncertainty Range (±) Example: A graduated cylinder has increments of 1 mL The uncertainty or random error is 1mL / 2 = ± 0.5 mL

A & S 2. Uncertainty Range (±) Uncertainty of Electronic Devises On an electronic devices the last digit is rounded up or down by the instrument and will have a random error of ± the last digit. Example: Our balances measure ± 0.01 g Digital Thermometers measure ± 0.1 oC

State uncertainties as absolute and percentage uncertainties Absolute uncertainty The uncertainty of the apparatus Most instruments will provide the uncertainty If it is not given, the uncertainty is half of a measurement Ex: a glass thermometer measures in 1oC increments, uncertainty is ±0.5oC; absolute uncertainty is 0.5oC

State uncertainties as absolute and percentage uncertainties Percentage uncertainty = (absolute uncertainty/measured value) x 100%

Determine the uncertainties in results Calculate uncertainty Using a 50cm3 (mL) pipette, measure 25.0cm3. The pipette uncertainty is ± 0.1cm3. What is the absolute uncertainty? 0.1cm3 What is the percent uncertainty? 0.1/25.0 x 100= 0.4%

Determine the uncertainties in results Calculate uncertainty Using a 150 mL (cm3) beaker, measure 75.0 ml (cm3). The beaker uncertainty is ± 5 ml (cm3). What is the absolute uncertainty? 5 ml (cm3) What is the percent uncertainty? 5/75.0 x 100= 6.66%  7%

Determine the uncertainties in results Percent error = I error l x 100 accepted When… Percent error > Uncertainty Systematic errors are the problem Uncertainty > Percent error Random error is causing the inaccurate data

Determine the uncertainties in results Error Propagation: If the measurement is added or subtracted, then absolute uncertainty in multiple measurements is added together.

Determine the uncertainties in results Example: If you are trying to find the temperature of a reaction, find the uncertainty of the initial temperature and the uncertainty of the final temperature and add the absolute uncertainty values together.

Determine the uncertainties in results Example: Find the change in temperature Initial Temp: 22.1 ± 0 .1oC Final Temp: 43.0 ± 0.1oC Change in temp: 43.1-22.1 = 20.9 Uncertainty: 0.1 + 0.1 = 0.2 Final Answer: Change in Temp is 20.9 ± 0.2 oC

Determine the uncertainties in results Error Propagation: If the measurement requires multiplying or dividing: percent uncertainty in multiple measurements is added together.

Determine the uncertainties in results Example: If you are trying to find the density of an object, find the uncertainty of the mass, the uncertainty of the volume, you add the percent uncertainty for each to get the uncertainty of the density.

Determine the uncertainties in results Example: Find the Density given: Mass: 25.45 ± 0.01 g and Volume: 10.3 ± 0.05 mL Density: 25.45/10.3 = 2.47 g/mL % uncertainty Mass: (0.01/25.45) x 100 = 0.04% % uncertainty Volume: (0.05/10.3) x 100 = .5% 0.04 + .5 = .54% Final Answer: Density is 2.47 ± .54%

Determine the uncertainty in results Uncertainty in Results (Error Propagation) 1. Calculate the uncertainty a. From the smallest division (on a graduated cylinder or glassware) b. From the last significant figure in a measurement (a balance or digital thermometer) c. From data provided by the manufacturer (printed on the apparatus) 2. Calculate the percent error 3. Comment on the error a. Is the uncertainty greater or less than the % error? b. Is the error random or systematic? Explain.