Lab Notebook

• See pages 10-11

• Required Headings for each lab:

o Title

o Purpose (2-3 sentences briefly stating main concepts, reactions and techniques)

o Theory (1-2 pages outlining relevant theory of concepts, reactions and techniques.

Chemical structure, figures and schematic diagrams are highly recommended.)

o Procedure (A point form version of experimental procedure. Tables for data collection

are required.)

o Chemical Hazards (Toxicological properties, preventative measures, first aid measures)

• Write in pen

• Write on the original page and insert divider under

copy sheet before wiring

• Put your name on the front and leave room for a Table

of Contents

Determinate and

Indeterminate Errors

• Determinate errors: systematic, experimental

o i.e. inaccurate equipment, impure reagents

• Indeterminate errors: operator, random

o i.e. Losses from transfers, differences in judgement

Precision versus Accuracy

Precision:

agreement

between various

measurements

Accuracy:

agreement

between the

average result and

the actual value

http://celebrating200years.noaa.gov/magazine/tct/accuracy_vs_precision.html 2010-09-14

Uncertainty

• There is always some uncertainty in measurement

• Equipment in this lab has typical uncertainty

o See page 43

Instrument

Typical Uncertainty

Graduated cylinder, 10 mL

± 0.1 mL

Graduated cylinder, 100 mL

± 0.2 mL

Pipette, 5 mL

± 0.01 mL

Pipette, 10 mL

± 0.02 mL

Pipette, 25 mL

± 0.03 mL

Balance: Electronic top loader

± 0.01 g

Balance: analytical, Mettler

AE160/AE200

± 0.0001 g

Significant Figures

• Significant figures help to identify the precision of a

measurement

o Zeros to denote position of decimal are not sig figs

Number of sig figs

Number of sig figs

0.0301 g

3

0.001030 g

4

4.290 hours

4

5000 miles

1 (but ambiguous)

1.030 mg

4

5.000 x103

miles

4

• Example: using a 10 mL graduated cylinder, measured

6.2 mL

o According to the typical uncertainty in equipment, the data would be

recorded as 6.2 ± 0.1 mL

o 2 sig figs in the measurement

o 6 is certain, 2 is uncertain

Significant Figures in

Calculations

• Addition and Subtraction:

o Significant figures should be reported to the precision of the term of lowest

precision

24.35

- 9.575

+11.2

+0.46

26.435 -> 26.4 (3 significant figures)

Note: Keep the least decimal places

o Perform the calculation and then round off the digits

Significant Figures in

Calculations

• Multiplication and Division

o Significant figures are reported to the precision of the term of lowest

relative precision

•

ସଷ.଼ଽ ×ହ.ଶ

ସ.ଷ

= 5.648 × 10ଶ → 5.6 × 10ଶ

Note: Keep the least sig.fig.

(2 sig figs)

Significant Figures in

Calculations

• Logarithms and Antilogarithms

o The number of sig fig. in the number = The number of decimal places in

the logarithm

o For example:

log 1.21

3 sig. figs

=

0.083

- 3 decimal places

o In pH calculations

if [H+] = 0.047M, pH = -log 0.047 (2 sig. figs)

= -log 4.7x10-2

= 2.00 - log 4.7

= 2.00 - 0.67(2)

= 1.33 (2 decimal places)

Significant Figures in

Calculations

• Multistep calculations:

o Calculate intermediate results beyond the necessary precision and round

off at the end

• Rounding:

o If the figure next to the last retained digit is 5 or more round up

o If the If the figure next to the last retained digit is lee than 5 round down

o 4.6349

o 4.6349

4.635 (to 4 sig figs)

4.63 (to 3 sig figs)

Uncertainty in

Calculations

• Addition and Subtraction

o Uncertainty is the sum of the uncertainties of each component

measurement

• Length measurement

o Between 1.38 ± 0.02 cm and 13.85 ± 0.02 cm

13.85

- 1.38

12.47

± 0.02

± 0.02

± 0.04 cm

• Uncertainty of the Average

o Three trials of a length measurement:(1)18.50 ± 0.04 cm; (2)18.40 ± 0.04

cm; (3)18.60 ± 0.04 cm

o Average : (18.50 +18.40…