This document provides information on various laboratory techniques and concepts related to experimental design and chemical analysis. It discusses the following key topics in 3 sentences or less each:
- Basic laboratory equipment used for carrying out reactions and storing liquids such as flasks, beakers, test tubes, and boiling tubes.
- Units and methods for measuring time, temperature, mass, and volume including the SI units. Instruments like measuring cylinders and burettes used to measure volume are described.
- Different methods for collecting and drying gases depending on their properties like solubility, density, and whether they are lighter or denser than air.
- The difference between mixtures and solutions, and concepts like solvents, saturated solutions, and
5. Learning outcomes
• know and understand how to
measure time, temperature, mass
and volume
• know and understand the
concept of each method of
separating mixtures
• know and understand the use of
suitable solvent, filtration,
crystallisation and distillation
7. Basic Laboratory
apparatus
• Flask are used for carrying out reactions
where fairly small amounts of liquid are
used
• Beakers are used to store liquids
temporarily or sometimes for carrying
out reactions
• Test tubes are used to carry out
reactions where small amounts of liquid
are used and not heated
• Boiling tubes are used to heat small
amounts of liquids
9. Measuring volumes and units
The SI unit dm3.
Beaker
• Used to estimate the volume of a
liquid, e.g. approximately 100 cm3.
Measuring cylinder
• More accurate than a beaker
• Measures up to the nearest cm3,
e.g. 99 cm3
Burette
• Accurately measures out the volume
of a liquid to the nearest ±0.1 cm3
• Scale marked (graduated) in 0.1 cm3
divisions
• Used to deliver different volumes of
liquids, e.g. 24.0 cm3 or 38.9 cm3.
Pipette
• Accurately measures out fixed
volumes of liquids, e.g. 20.0 cm3
or 25.0 cm3
10.
11.
12.
13. Seatwork
Open your google classroom.
Read the measurement tools on the
worksheet.
Plot the data into graph
15. How we collect a gas depends on the
physical properties of the gas, namely:
•solubility — whether a gas is soluble in water
•density — how dense the gas is compared to air
16. Gas Solubility in water Density compared to
air
Ammonia Extremely soluble Less dense
Carbon dioxide Slightly soluble Denser
Chlorine Soluble Denser
Hydrogen Not soluble Less dense
Hydrogen chloride Very soluble Denser
Oxygen Very slightly soluble Slightly denser
Sulphur dioxide Very soluble Denser
The solubility and density of some common
gases
17. Collecting Gases –
Method 1
Displacement of water
This method is used to
collect insoluble gases.
Examples of insoluble
gases:
Hydrogen, oxygen,
carbon dioxide.
18. Collecting Gases – Method 2
Downward delivery This method is used to
collect gases that are
denser than air (and
soluble in water).
Examples of such
gases:
Chlorine, hydrogen
chloride.
19. Collecting Gases – Method 3
Upward delivery
Examples of such gases:
ammonia.
This method is used to
collect gases that are less
dense than air (and soluble
in water).
20. Learning check
Determine the method of collecting gases .
Question 2: collecting a gas that is lighter than
air
Answer 2:
Question 3: collecting a gas that is soluble
heavier than air
Answer 3:
Question 1: Measuring the volume of a gas that
is sparingly soluble in water?
Answer 1:
22. Drying a gas – method 1
Concentrated sulphuric
acid is used dry many
gases except for ammonia
Notice the positions of
the delivery tubes
23. Drying a gas – method 2
We use quicklime to
dry ammonia gas.
quicklime (calcium oxide)
24. Drying a gas – method 3
Fused calcium chloride can
be used to dry most gases.
fused calcium chloride
25. How do we measure the volume of a gas
accurately?
A gas syringe is used to measure the volume of
a gas. The gas syringe measures a maximum
volume of 100 cm3.
barrel
plunger
29. Pure substances and impurities
A pure substance is made up of only one substance.
30. Does purity matter?
An unwanted substance, mixed with the substance you want, is called
an impurity.
Impurities must be detected as they may cause side effects.
Impurities can be checked by its melting and boiling points.
31. A pure substance has a definite, sharp, melting point and boiling point.
When a substance contains an impurity:
– its melting point falls and its boiling point rises
– it melts and boils over a range of temperatures, not sharply.
The more impurity there is:
– the bigger the change in melting and boiling points
– the wider the temperature range over which melting and boiling occur .
37. 2 By crystallisation
It works because soluble solids tend to be less soluble at lower temperatures.
38. 3 By evaporating all the solvent
For some substances, the solubility changes very little as the temperature falls.
So crystallisation does not work for these. Salt is an example.
39. Now you try!
Calcium carbonate is insoluble in water.
Sodium sulfate is soluble in water.
Describe how you could separate a mixture
to obtain a sample of each pure solid.
40. 4 Simple distillation
This is a way to obtain the solvent
from a solution.
Example
Water from salt solutions
41. 5 Fractional distillation
This is used to separate a mixture of liquids from each other.
Example mixture of water and ethanol
43. 6 Paper chromatography
This method can be used to separate a mixture of substances. For example, you could use it to
find out how many different dyes there are in black ink:
The dyes in the ink have different solubilities in water. So they travel across the paper
at different rates. (The most soluble one travels fastest.)
That is why they separate into rings. The filter paper with the coloured rings is called a
chromatogram. (Chroma means colour.)
44. 6 Paper chromatography
Paper chromotography can also be used to identify substances
The more soluble a substance is in the solvent, the further it will
travel up the chromatography paper.
45. What are the uses of chromatography?
Chromatography is used to
• separate the components in a sample,
• identify the number of components in a sample,
• identify the components present in a sample,
• determine the purity of a sample.