writing a lab report about separation of a mixture of solids

EXPERIMENT #2: SEPARATION OF AMIXTURE OF SOLIDS
Purpose:
The purpose of this experiment is to learn methods of separating a mixture of
substances and to perform calculations involving mass percentages.
Special Apparatus and Chemicals:
Bunsen burner
Tongs
2 Evaporating dishes
Watch glass
Iron ring and stand
Clay triangle
Electric hot plate
2-3g of unknown mixture
Discussion:
Since chemistry is the scientific study of the composition, structure, and
properties of matter and the transformations that it undergoes, chemists are
often called upon to determine the composition of a material. If the material is a
mixture, the components of the mixture may have to first be separated in order
to quantitatively determine the composition. Materials may be classified as
either pure substances or a mixtures. Pure substances are those materials
defined by a fixed composition and a set of characteristic properties. A pure
substance may be either an element or a compound. Mixtures are combinations
of two or more pure substances in a variable ratio. Mixtures may be classified
as heterogenous or homogenous. Homogenous mixtures (often called solutions)
have a uniform composition throughout; heterogenous mixtures have a variable
composition in different regions of the material.
Mixtures may be separated into pure substances based on differences in the
physical properties of its component pure substances. Physical properties are
those properties that can be measured without changing the basic nature of the
substance. Some examples of physical properties are melting and boiling
points, color, odor, density, solubility, and hardness. In this experiment we will
use differences in the properties of sublimation and solubility to separate a
heterogenous mixture of solid NH4C1, NaC1, and Si02.
Because ammonium chloride (NH4Cl) undergoes sublimation at 340°C and NaC1 and
Si02 do not, the NH4C1 may therefore be separated from a mixture containing NaCl
and Si02 by heating the mixture containing all three above 340°C. A substance is said
to undergo sublimation when it goes from the solid phase directly to the gas phase
without passing through the liquid state. Some common substances that undergo
sublimation under normal conditions are CO2 (dry ice), iodine, naphthalene (moth
balls), and ice (below the freezing point, 0°C). Upon heating the mixture containing
NH4Cl, the ammonium chloride will be seen leaving the sample as a white smoke. As
soon as the ammonium chloride leaves the dish, the sublimed NH4C1 condenses back
to a solid which is seen as white smoke.
Both NH4C1 and NaCl are soluble in water but SiO2 is not. NH4C1 and/or NaC1 could
be extracted from a mixture with SiO2 by adding water to preferentially dissolve the
NH4C1 and/or NaC1. The aqueous solution of NH4C1 and/or NaC1 that forms could
be removed from the still solid SiO2 by decantation or filtration. Decantation is the
process of carefully pouring a liquid from a solid. Filtration is the process of using a
porous membrane (i.e. filter paper), allowing a liquid to pass through leaving the solid
behind on the filter.
Once you have determined the mass of the components in a mixture, and the total
mass of the sample is known, the percent by mass of the components in the mixture
may be determined. The composition of mixtures is often reported as a mass percent.
“Percent” means per centuin the amount out of 100. Percents are calculated by taking
a fraction or ratio and multiplying by 100. To calculate a mass percent take the mass
fraction and multiply by 100. For example if a mixture contains two components A
and B with a total sample mass of 2.454g and there is 1 .002g of A in the mixture then
the mass percent of A in the mixture may be calculated as follows:
Concept:
The unknown mixture that you will separate contains 3 components, NaCl (sodium
chloride, “table salt”), SiO2, (silicon dioxide, “sand” or “silica”) and NH4Cl
(ammonium chloride). The separation of these three compounds will be accomplished
by first heating the mixture to remove NH4Cl by sublimation. Next, extracting the
NaCl from the mixture with water, and finally removing the remaining water from the
NaCl and SiO2. See scheme above:
Procedure:
Weigh a clean, dry evaporating dish. Add between 2 to 3 grams of your unknown
mixture and weigh the dish and the sample and determine the sample mass to the full
limit of precision of your balance. Put the evaporating dish with the mixture on a
ring stand IN THE FUME HOOD and heat the mixture over a Bunsen burner until
white smoke stops forming.
CAUTION: Sublimation
must be done in the hood because a large amount of NH4Cl
smoke is produced. Be careful to make sure that all of the NH4Cl has been removed
from the dish, check to make sure none has recondensed on the side of the dish.
Crucible tongs may be used to move the dish and a wire gauze pad should be used as a
hot pad. Cool the evaporating dish to room temperature and weigh the dish and
sample after heating. (NEVER WEIGH HOT OBJECTS). The mass difference before
and after heating is the amount of NH4Cl sublimed. Calculate the mass percent of
NH4Cl in the original sample.
Alternative Heating Method. If Bunsen burners are unavailable, the sublimation
step
may be carried out by placing the sample in a evaporating dish or Petri dish
bottom and
heating on an electric hot plate turned on high. Remember to do this step in the
HOOD.
Add 20 mL of distilled water to the solid remaining in the evaporating dish and stir to
dissolve the NaCl. Weigh the second evaporating dish and watch glass empty. After
letting any SiO2 present settle to the bottom, decant (pour off) the liquid from the first
dish to the second. Be careful not to transfer any of the SiO2, sediment to the second
dish. Add 10 more mL of water to the first dish, stir, and then again decant liquid to
the second dish. Repeat with a second 10 mL portion of water. Now the first dish
contains wet SiO2 and the second an aqueous solution of NaCl.
Heat both dishes carefully on a hot plate until all of the water evaporates. When the
dish containing NaCl is near to dryness, cover with the watch glass to prevent
splattering as the last of the water evaporates. After all the water has evaporated from
both dishes (make sure the watch glass is completely dry also), cool to room
temperature, and weigh both dishes. Calculate the amount of NaCl and SiO2, that you
have recovered from the sample. Calculate the mass percentage of NaCl and SiO2 that
were in the original sample.
DISPOSAL: The NaCl left in the evaporating dish may be washed down
the sink since it is non-toxic and water soluble. The leftover SiO2 should
be dumped in the trash can.
Add the masss of NH4Cl, NaCl, and SiO2 that you determined to be in your sample.
Calculate the percent of matter that you recovered. If your combined total is not
between 99.0% and 100.0%, explain what mistakes may have occurred in your
experiment. Some common mistakes include not completely drying the NaCl or SiO2,
letting some of the NaCl solution splash out of the dish during evaporation, and
material popping out of the dish during sublimation or evaporation. Consult your
instructor to find out if you should repeat the procedure.
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Running head: DENSITY
1
Introduction to laboratory techniques:
Experiment 2 Density
Name: Omar Alardhawy
Chem 110L.002
Dr.Haynes
Morgan state university
DENSITY
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Introduction
Density
In chemistry, density is defined as mass per unit volume of matter. It is used to calculate the
solidity in the molecular arrangement in a particular substance, therefore, determining how
weighty or light it measures. It is easier to identify a substance by measuring its density in the lab
and comparing the densities list (Craesmeyer & Schadschneider, 2015). However, this can only
be achieved if the substances used are pure. Below is a compilation of a lab report done to
identify unknown solid through measurement of density. Density measurement is applied in
many fields. This paper also explains how the experiment can be applied in the engineering
world.
Density formula= mass/volume
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Typed data and observation
Calibration of the Balance
Limit of
0.01g
Precision
Accuracy
10g
100g
9.99g
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Standard
4
10.01g
weight
Standard
100.01g
weight
99.99g
Measured
9.87g
Weight
Measured
99.87g
Weight
Temperature of 19 degrees Celsius.
Precision Using
Trial 1
Trial 2
Trial 3
Trial 4
48.79g
58.79g
68.70g
78.62g
40.46g
48.79g
58.78g
68.71g
Pipet
Mass of the flask
after addition of
water
Mass of the flask
before addition
of water
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Mass of water
8.33g
10.00g
9.92g
9.91g
Temperature of water used in pipet is 19 degrees Celsius.
Density of water is 0.9989g/ml (See table 1)
Volume of water delivered (Show Calculations)
Volume=mass/density
Mass of
8.33g
10.00g
9.92g
9.91g
Volume
8.33/0.9989
10/0.9989
9.92/0.9989
9.91/0.9989
Volume =
8.34ml
10.02ml
9.93ml
9.94ml
water
Average volume delivered (Show calculations)
V (av) = (V1+V2+V3+V4)/4
= (8.34+10.02+9.93+9.94)/4
=9.56ml
Standard deviation of Volume
S= (d12+d22+d32+d42)/ (4-1)
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Volume =
d
8.34ml
10.02ml
9.93ml
9.94ml
(8.34-
(10.02-
(9.93-
(9.94-
9.56)
9.56)
9.56)
9.56)
Standard deviation of Volume= (8.34-9.56)2+ (10.02-9.56)2+ (9.93-9.56)2+ (9.949.56)2)/3
= 0.057
Density of Unknown Solid
This is the second part of the experiment which is calculating the density of three unknown solids.
First, three random objects were picked. They have these shapes.
Mass of metal
9.49g
7.71g
8.75g
Volume of cylinder
680ml
680ml
660ml
610ml
610ml
605ml
70ml
70ml
55ml
after adding metal
Volume of cylinder
before adding metal
Volume of metal
sample
Density formula= mass/volume
DENSITY
Density of metal
Density
7
9.49g/70ml
7.71g/70ml
8.75g/55ml
0.13g/ml
0.11g/ml
0.15g/ml
Average density= (D1+D2+D3)/3
= (0.13+0.11+0.15)/3
= 0.13g/ml
Standard deviation of density
S= (d12+d22+d32)/ (3-1)
Density
0.13g/ml
0.11g/ml
0.15g/ml
d
(0.13-0.13)
(0.11-0.13)
(0.15-0.13)
Standard deviation of density= ((0.13-0.13)2+ (0.11-0.13)2+ (0.15-0.13)2)/2
=0.0004
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Report Sheet Questions
1. What is the calculated precision for your measurement of the volume delivered by the
pipet and what is the suggested limit of precision for a 10ml volume pipet? How do these
two values compare? The two values are similar.
Calculated Precision
±0.01
Suggested limit of precision
±0.01
2. What other properties besides density could you use to identify unknown solid?
There are several physical colors that one could use to identify the unknown solid such as
color, solubility or odor. Additionally, the physical state at room temperature such as being solid,
liquid or gas. Other properties include melting and boiling points, as well as refractive index.
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Application of Density in Engineering World
Density measurement is a critical concept for Engineers. While density helps in determining the
mass of a substance, it is also essential in the determination of the ability of an object to float or
sink while placed on a fluid. The density of a substance can be changed by either compression or
increase in mass for the same volume. An object floats on fluid when the overall weight it
displaces from the surface area of contact is equal to the weight of the object otherwise it will
just sink. Engineers use density knowledge in designing ships, boats, and all other water
constructions (Kitchin & Dodge, 2011).
Conclusion
In conclusion, density is described as mass per unit volume. With the known value of density,
the mass of an object can easily be calculated using its volume. Additionally, it is easy to identify
a substance using its measured density and comparing it to the list of densities. Finally, density
can be applied in many fields in the real world including engineering.
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References
Craesmeyer, M., & Schadschneider, A. (2015). Simulation of Merging Pedestrian Streams at TJunctions: Comparison of Density Definitions. In Traffic and Granular Flow’13 (pp. 291298). Springer, Cham.
Kitchin, R., & Dodge, M. (2011). Code/space: Software and everyday life. Mit Press.