Download Comparing Solubilities Lab Report

Chemistry
Name
Period
Comparing Solubilities Lab
Background:
Compounds fall into three categories: ionic, polar covalent or nonpolar covalent. When
compounds combine they follow the rule of “like dissolves like”.
Materials:
Solvents
Distilled Water
Ethyl Alcohol (C2H5OH)
n-hexane (C6H14)
Solutes
Sucrose Sugar (C12H22O11)
Salt
Naphthalene (C10H8)
Calcium Carbonate
4 small test tubes
4 stoppers
scooper
pipette
test tube rack
Procedure A:
1. Test the solubility of the various solvents in each other. Mix 1 mL of each solvent with 1 mL of the
other solvents in three separate test tubes. Record color, clarity, and if the mixture is soluble (S),
slightly soluble (SS), or insoluble (I). Record your results in Data Table 1-1 before agitation.
2. Place a stopper in each test tube. Agitate the test tube, and record the results after agitation Data
Table 1-1.
3. Clean the test tubes well prior to Procedure B.
Procedure B:
1. Add 1 mL of H2O solvent into each of the four test tubes.
2. Place a match head’s amount of each solute into the 4 test tubes (only 1 solute per tube).
3. Record the results in Data Table 1-1 before agitation.
4. Place a stopper in each test tube and agitate. Record your observations in Data Table 1-1.
5. Clean the test tubes. Repeat the procedure using the other two solvents.
CAUTION: Hexane is to be disposed in the HAZARDOUS WASTE CONTAINER!
Data Table 1-1: Observations of solutes in solvents
SOLUTES
SOLVENTS
Sugar
Salt
Naphthalene
SOLVENTS
CaCO3
Water
Ethanol
Hexane
Water (no ag.)
w/ agitation
Ethanol (no ag.)
w/ agitation
Hexane (no ag.)
w/ agitation
Sketch:
1. Write the molecular formula and draw the structural formula for each solvent (3) and each solute (4)
used in this experiment.
2. Label each substance as ionic, polar or nonpolar. If the molecule is polar covalent, show the position
of the partial charges (δ+ or δ-) on the molecule.
Conclusion:
1. Which of the solutes are soluble in hexane? Are these solutes polar or nonpolar? Explain your
decision.
2. Which solvents were soluble in each other?
3. Which solvent was soluble in the other two? Explain what must be true about the structure of this
solvent.
4. Which of the chemicals used in this experiment do you think are organic? What characteristic(s) of
these structures make them organic?
5. What is the structural difference between a polar and an ionic molecule? Do they behave differently?
If so, how does each behave? Explain their behaviors.
6. Write your conclusion paragraph