CHEM115 LAB 1 DENSITY
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Dec 6, 2023
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Brianna Krzyminski
CHEM115 Lab 1
TITLE
: Density Determination: Quantitative Measurement
BACKGROUND INFORMATION
: The study of chemistry involves not only observing, but
also measuring. Careful attention should be given to the degree of uncertainty in your
measurements. Record only those digits which are significant and use only those digits in
your calculations.
The accuracy of your methods can be reported with your results in terms of percent of
error. The percent error in calculations and measurements is a comparison of differences
between experimental results and theoretical values, expressed as a percentage.
Percentage error can be determined as follows:
% error = experimental value – theoretical value
X 100
theoretical value
A useful way of comparing two substances is to compare their densities. By carefully
measuring the mass and volume of two substances, their densities can be calculated as
follows: Density = Mass/Volume
OBJECTIVES
: In this experiment, you will
*Determine the density of different substances
*Calculate the percentage error in your results
EQUIPMENT
: 10 ml graduated cylinder
50 ml graduated cylinder
Test tube brush
PROCEDURE
:
1.)
Prepare a data table as directed in the analysis.
A.
Density of an unknown Liquid
.
1.)
Measure the Mass of a 10 ml graduated cylinder.
2.)
Pour approximately 9 ml of the liquid into the graduated cylinder. Record, to the
nearest .01 ml, the
exact
amount of liquid you use.
3.)
Measure and record the mass of the graduated cylinder and the liquid.
B.
Density of solids
.
1.)
Obtain two different metals, measure and record their masses.
2.)
Put about 25 ml of water into the 50 ml graduated cylinder. Accurately read the
volume of water you use, and record.
3.)
Carefully immerse one metal into the water in the graduated cylinder. Carefully read
the new volume and record.
4.)
Repeat steps 2&3 with the other metal.
ANALYSIS
:
1.)
Prepare a data table to record your observations. Follow the sample format for your
table. Calculate the density for the unknown liquid, and the metals.
Mass Calculation:
48.1925 g – 39.8673 g
=
8.3252 g
Density Calculation:
8.3252 g
=
0.888 g/mL
9.38 mL
Volume Calculation:
67.0 mL – 73.4 mL
=
6.4 mL
Density Calculation:
57.9824 g
=
9.1 g/mL
6.4 mL
Volume Calculation:
96.8 mL – 75.6 mL
=
21.2 mL
Density Calculation:
57.9747 g
=
9.1 g/mL
21.2 mL
2.)
Once you have completed your measurements, use your chemistry book to
determine the unknown metals true density.
True Density Mineral Oil
: 0.89 g/mL
True Density Metal #1 (Copper Cu)
: 8.96 g/mL
True Density Metal #2 (Aluminum Al)
: 2.7 g/mL
QUESTIONS
:
1.)
Calculate the percentage error for the unknown liquid, and two metals.
Use significant digits and show set-ups for your calculations.
% error
= | true density
-
experimental value |
X 100
true density
Material
Mass
Volume
Density
Graduated Cylinder
39.8673 g
Graduated Cylinder & Liquid
48.1925 g
Liquid (Mineral Oil)
8.3252 g
9.38 mL
0.888 g/mL
Material
Mass
Volume
Density
Water
67.0 mL
Water & Solid #1
73.4 mL
Solid #1 (Copper Cu)
57.9824 g
6.4 mL
9.1 g/mL
Material
Mass
Volume
Density
Water
75.6 mL
Water & Solid #2
96.8 mL
Solid #2 (Aluminum Al)
57.9747 g
21.2 mL
2.73 g/mL
Mineral Oil
:
| 0.89
-
0.888 |
x
100
=
0.22 %
0.89
Copper (Cu)
:
| 9.1
-
8.96 |
x
100
=
1.6 %
8.96
Aluminum (Al)
:
| 2.73
-
2.7 |
x
100
=
1.1 %
2.7
2.)
What were at least two likely sources of error?
Two of the most likely sources of error are related to human error and/or equipment
error. Values recorded off the graduated cylinders to obtain volumes weren’t likely to
be perfectly accurate due to volumes falling between measurement lines and having to
guesstimate the exact volume. Equipment error could be a variable when considering
the possibility of the scales utilized to obtain mass not being perfectly calibrated.
3.)
The method used to find the densities of the metals will not work for all solids.
Why not? Suggest a method of determining the density of these solids.
Water displacement was utilized to determine volumes in this experiment. Water
displacement may not be appropriate for finding the volumes of other objects due to
the type of material and or shape / size and the ability to accommodate those variables
while still remaining accurate. A pycnometer is another means to calculate density that
could be utilized in these types of scenarios.
4.)
Water is often used as a standard in making comparisons between densities of
substances. Based on your data of waters density, suggest a reason for using
water as a standard.
Water is a great standard to use because it has a true density of 1 g/mL, additionally
water is an extremely abundant/available substance.
5.)
Is density an intensive or extensive physical property? Explain why density can
be used to determine the identity of an unknown substance.
Density is an intensive physical property. The values used to find density (volume /
mass) however, are extensive because they can vary / change depending on sample
size. The calculation of density utilizing those values however should not change; this
property of density is what makes it a great way to determine the identity of an
unknown substance as it is a constant. The story of Archimedes and the gold crown is a
great example for why/how density can be used to identify an unknown substance.
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Part 3: Calculate density of a metal an unknown metal.
1. Using the pictures below, record the displayed data in the data table in the report sheet. Make sure to include the right
number of significant figures in the measurements and calculations.
Mass measurement
7.1 g
Volume of water
measurement. There's
only one measurement
here – the larger image
is for magnification
only.
-20
15 m
Volume of water and
metal measurement.
There's only one
measurement here – the
larger image is for
magnification only.
20 m
15
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sample whose density is 7.639 g/mL and the only other component
is copper? The density for pure copper is 8.96 g/cm³ and the density
of pure zinc is 7.13 g/cm³. Report your answer to one decimal place.
NOTE: This question is meant to give you practice before your data.
The density value generated is random within a certain realistic
constraint. It will not be representative of your data in the
experiment.
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Use the References to access important values if needed for this question.
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First he measured the mass of the metal to be 311.2 grams. Then he dropped the metal into a measuring cup and found that it displaced 15.9 mL of
water.
Calculate the density of the metal.
Density =
g/ mL
Use the table below to decide the identity of the metal. This metal is most likely
Densities of Some Common Substances
Substance Density (g/mL)
Water
1.00
Aluminum 2.72
Chromium 7.25
Nickel
8.91
Сopper
8.94
Silver
10.50
Lead
11.34
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Please answer this question as fast as you can please and tahnk you. I will afterwards write an wonderful review on solving the question. Thank you.
For each piece of glassware measure the density of water in triplicate (three times). Why repeat the procedure multiple times for each piece of glassware?
Running the measurement in triplicate increases the precision of our results and reduces the impact of a single outlier result.
The experiment would be too short if you only ran each trial once
The first two trials act as practice, and the final trial will give you the true result.
Running the measurement in triplicate increases the accuracy of our results and reduces the impact of a single outlier result.
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Use the References to access important values if needed for this question.
A general chemistry student found a chunk of metal in the basement of a friend's house. To figure out what it was, she used the ideas just developed in class about
density.
She measured the mass of the metal to be 323.0 grams. Then she dropped the metal into a measuring cup and found that it displaced 16.5 mL of water.
Calculate the density of the metal.
Density=
g/mL
Densities of Some Common
Substances
Substance Density (g/mL)
Water
Aluminum 2.72
Chromium 7.25
Nickel
Copper
Silver
Lead
Mercury
1.00
Gold
Tungsten
Platinum
8.91
8.94
10.50
11.34
13.60
19.28
19.38
21.46
Previous
Next>
?
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Scientific method may never prove a theory to be wrong.
Repeat measurements that fall close to the true value are both accurate and precise.
There is only energy in the Universe and no matter.
The number in the quantity '30 miles' is inexact.
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Liquid
Dichloromethane
Methanol
0
Density
mL
g
mL
1.3340
0.791
Volume (mL)
9.28
Determine the density of the object. Be sure your answer has the correct number of significant digits.
6.15
0
X
S
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hexane for the unknown sample. You must also follow all the instructions given throughout this
handout.
% hexane
100.0
(SECTION 2) TO BE DONE BY HAND AND TURNED IN
80.0
60.0
40.0
20.0
unknown
Density (g/mL)
0.642
0.684
0.724
0.766
0.806
0.699
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Using his observations of the properties of the ink, the student can classify it as a
heterogeneous mixture.
solution.
compound.
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PART 3
A Volumetric Flask
+ A
С —
ALI50
SOA
A 50-mL volumetric flask measures a volume of 50.00 mL. In this experiment, we want to show that
this is true. 50.00 mL is the actual volume measured by this volumetric flask.
EXPERIMENT:
The mass of an empty volumetric flask is measured.
Then water is added to the volumetric flask and the meniscus is adjusted to be at the correct
level.
Then the mass of the volumetric flask and the water is measured.
Finally, the temperature of the water in the volumetric flask is measured.
RESULTS:
Mass of empty volumetric flask = 37.04 g
Mass of volumetric flask and water = 86.83 g
Temperature of the water in the volumetric flask = 23°C
4
Densities of water at different temperatures:
Density of Water at Different Temperatures
(g/cm)
Temp, °C
Density
Temp, °C
Density
Temp, °C
Density
18
0.99862
21
0.99802
24
0.99733
19
0.99844
22
0.99780
25
0.99708
20
0.99823
23
0.99757
26
0.99681
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Use weighing paper, a watch glass, a beaker, or some other container to measure mass of your solid samples.
For different trials of an experiment, use multiple balances for your measurements.
Do not return the mass settings to zero mark; let the next user tare it for you.
Place chemicals directly on the balance pan.
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4. The accepted value for the density of a certain metal is 6.81 g/cm³ . Calculate the percent
error in a laboratory measurement that gives a density value of 6.6 g/cm³ . Express this result
in the proper number of significant figures.
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