Leader : Beejay C. Oanes
Members :
Carl Jensen delos Santos
Bermhel Organte
Robert Jeremiah Reyes
Ivan Roberto
Yanni Young
Hershey Genovania
Emma Pauline Perdiguerra
Chrisette Perez
Hannah Joy Serrano
SCORING RUBRICS FOR FORMAL REPORTS
The question to be answered during the laboratory is stated
The hypothesis clearly shows it is based on research
Research references to prepare the lab are listed
Results of the procedure are clearly stated
Summarize the essential laboratory data
State how the essential data answers the lab questions
Report is neatly printed with ink, no visible correction
The lab report is written in such a way others could accurately duplicate the
experiment
TOTAL
Points
5
5
5
60
10
5
5
5
100
Score
Activity 1
Physical Properties of Organic Compounds
I.OBJECTIVE



To know how to measure the physical properties of organic compounds.
To know the melting and boiling point of different solvents.
To know the density of different solvents.
ii.Science concept/theoretical background:
In general chemistry, the most common solvent is water. In organic chemistry, however, we
use a variety of organic liquids as solvents that you will need to become familiar with. A solvent is
any liquid which can be used to dissolve solids, other liquids, or gases. This first part of this lab will
introduce you to the common organic solvents.
Some organic solvents are soluble in water, while some are not. It is important to know which
ones are insoluble, because they can be used to separate compounds through extraction and washing.
Solubility is determined by what intermolecular forces are present, and how strong they are. If a
solvent can engage in hydrogen bonding, or has dipole forces, and there aren’t too many nonpolar
bonds present, then it will most likely dissolve in water. The strength of the intermolecular forces is
often referred to as polarity – polar molecules have strong intermolecular forces, while nonpolar
molecules have weak intermolecular forces.
iii.schematic procedures:
\
Procedure :
Prepare the 15 organic solvents, each vial contains of 4 ml of each solvents. Then , test the 15 sovents in
water and observe if it is miscible or immiscible.Place the 15 organic solvents in a graduated cylinder and
see which is more dense or less dense.If the solvents stays above it is less dense but if it go in the bottom
of the water it is more dense than the other solvents.
Iv.RESULTS AND DISCUSSION
Solvent
Salicylic acid
Description or
structure
C7H6O3
Lewis structure
Functional group
Di
electric
constant
phenol group
and carboxylic
acid
Water
solubility
Density
Boiling
point
Melting
point
miscible
1.443
g/cm3
211 °C,
159.0 °C
miscible
.6548 g
mL−1
68-69 °C
-96--94 °C
hexane
CH3(CH2)4CH3
Alkane
napthalene
C10H8
Aromatic
hydrocarbon
6.95
immiscible
1.14 g/cm³
218 °C
80.26 °C,
Acetic acid
CH3CO2H
carboxylic
acids.
6.2
miscible
1.049 g
cm-3
118119 °C
16-17 °C
acetone
CH3COCH3
Ketone
20.7
miscible
0.791 g
cm−3
56-57 °C
1.9
-95--93 °C
Ethanol
CH3CH2OH
Alcohol
24.3
Miscible
0.789
g/cm3
78.37 °C
−114 °C
Isopropyl
alcohol
(CH3)2CHOH
Alcohol
17.9
Miscible
0.786
g/cm3
82.5 °C
−89 °C
Mouthwash
/methyl
salicylate
C6H4(HO)
COOCH3
Ester and
alcohol
6.93
immiscible
1.174
g/cm³
220 - 224
°C
-9 °C
m-xylene
C6H4(CH3)2
Aromatic
hydrocarbon
2.4
immiscible
0.86 g/mL
139 °C,
-48 °C,
Benzoic acid
C6H5COOH
aromatic
carboxylic acid
immiscible
1.27 g/cm3
249.2 °C
122.41 °C
Formalin
CH2O
aldehydes
miscible
0.8153
g/cm³
-19 °C
-92 °C,
Ammonia
NH3
miscible
0.86 kg/m3
−33.34 °C
−77.73 °C
25
Questions
1) Petroleum ether (a solvent which is derived from petroleum) has a dielectric constant of 2.0. Would
it be classified as polar or nonpolar? Would you expect it to be miscible or immiscible with water?
Why?
- It is immiscible in water because water is polar and petroleum is non polar it wil not mix together
2) Only one of the common solvents is more dense than water. Which is it? Explain why it makes
sense that this solvent should be unusually dense.
Naphthalene because it has density of 11.03g/ml while water has 100g/milt is denser than water
therefore it will sink
3) Organic liquids A, B, and C have densities of 0.69 0 , 0.955 g/ml, and 1.126 g/ml. A and C are low
polarity solvents, while B is a high polarity solvent. When each is added to water, how would you
expect them to behave?
When each is added to water organic liquid c w/a density of1.126g/ml will sink followed by liquid b
with a density of0.956g/ml the liquid a with w/c density is 0.650g/ml
4) Why are the boiling points we measured in the lab lower than the ones in the catalogue? Are
melting points affected by this issue? Why or why not?
Temperature affects the melting points of a substance.the boiling point is differ in our boiling point in
catalogue
5) Explain the following observations:
a) ethyl acetate has a higher boiling point than hexane, even though they are approximately the
same molecular weight
the lower the density the lower of boiling point
b) methanol has a lower boiling point that ethanol even though it is more polar
polarity does not affect the boiling point of a substance
c) ethanol has a higher boiling point than ethyl ether even though ethyl ether is heavier
weight cannot affect the boiling point
6) The known melting point of 2-methylbenzamide is 140.2 oC. If you took the melting point of a
sample of this compound, how would you interpret the following results?
a) 139.2-140.5oC
b) 137.7-143.2oC
c) 149.1-150.3oC
the results of the melting point depend on the amount of the sample
7) 2-Methylbenzamide and 3-nitrobenzoic acid both have a melting point of 140.2oC. However, if you
mixed them together and took the melting point, it would not be140.2 oC. Why not? (Hint - this
is not
the result of a chemical reaction!)
because of their different polarity that affect the melting point of each substance.
v.conclusion.
We determine the melting ,boiling point and density of an organic solvents.