PAGE
Chemistry I 5.0
Lab Manual
Mrs. Ruppel
Table of Contents
Lab Name
Pages
1. Producing and Displaying Experimental Data
3-4
2. Density of Liquids Lab
5-8
3. Density of a Solid Lab
9-10
4. Physical and Chemical Changes Lab
11-14
5. Isotopes of Pennium Lab
15-16
6. Beanium Lab
17-18
7. Flame Test Lab
19-20
8. Distinguishing between Metals, Nonmetals, and Metalloids
21-22
9. Chemical Activity Lab
23-24
10. Models of Covalent Compounds Lab
25-26
11. Mole Lab
27-28
12. Hydrate Lab
29-31
13. Predicting Products Lab
33-36
14. Reactivity of Metals Lab (Single Replacement Lab)
37-38
15. Mole Relationship in a Chemical Reaction
39-41
16. Stoichiometry Lab #2
43-44
17. Determining the Percent Yield of Copper
45-46
18. Heat of Dissolving Lab
47-50
19. Specific Heat of a Metal Lab
51-52
20. Determining the Molar Mass of Butane
53-56
21. Solutions Lab
57-58
22. Penny Alchemy
59-60
23. Molarity and Dilutions
61
24. Determining Solution Concentration using a Spectrophotometer63-64
25. A Study of Chemical Equilibrium
65-68
26. Acid-Base Properties Lab
69-72
27. Determining the Concentration of a Base
73-74
28. Safety Packet
Producing and Displaying Experimental Data
Name ______________________________
20 Points
Date _____________ Period ___________
Objective: In this lab, you are to determine the effect of the concentration of dissolved sodium chloride (NaCl) on the temperature of boiling water. Each time you run the experiment, record the data in the table and then graph the temperature versus the time.
Materials:
250 mL graduated cylinderthermometer
distilled water
Bunsen burner
250 mL beaker
beaker tongs
boiling chips
ring stand
balance
striker
sodium chloride (NaCl)wire gauze
thermometer clamp
iron ring
Procedure:
1. Use your graduated cylinder to measure 150. mL of distilled water. Be sure to read the volume at the bottom of the meniscus. Pour the water into the beaker and add a boiling chip.
2. Set up a ring stand and burner as above. Be sure to clamp the thermometer to the ring stand. Watch that the water level does not fall below the thermometer bulb during the experiment.
3. For Trial A, do NOT add any salt to the water. Begin heating the water with the burner and bring it to a full boil.
4. As soon as the water comes to a full boil, record the temperature. This will be the temperature at time = 0 minutes. Record the temperature after 1, 2, 3, 4, and 5 minutes. Be sure to measure the temperature to the nearest 0.1oC. Record your results in the data table for Trial A.
5. Keep your boiling water and boiling chip for Trial B, but remeasure the water and add more distilled water if there is less than 150. mL. Repeat steps 2 through 5 again, but this time measure 10 g of sodium chloride, NaCl, with the balance and add it to the water before heating it. Record your data in the table for Trial B.
6. If time permits, discard the salt water from Trial B, retain the boiling chip and measure 150. mL of new distilled water. Repeat steps 1 through 5 again adding 20 g of sodium chloride, NaCl, to the water before heating it. Record your data in the table for Trial C.
Data Table:
Trial A Trial B Trial C
Time (min.)
Temp.C
0
1
2
3
4
5
Time (min.)
Temp.C
0
1
2
3
4
5
Time (min.)
Temp. C
0
1
2
3
4
5
Analysis and Conclusions:
1. What is the variable being tested in this experiment? _______________________________
2. The control run was completed during Trial A or Trial B or Trial C. (circle one)
3. You controlled the ________________ (time or temperature) during the experiment. Therefore, ______________ would be considered the independent variable and _______________ would be considered the dependent variable.
4. In a graph, the independent variable is displayed on the ____ axis and the dependent variable is displayed on the ____ axis.
5. Make a graph of all 3 trials using the time and temperature data. Use 3 different colors. Remember to label each axis with a measurement and unit. Also, include a key and title on your graph. The graph should be a smooth curve. Only include temperature values from 90oC+.
0 1 2 3 4 5
Based on YOUR tables and graph, write a general statement describing the relationship between boiling temperature and the amount of sodium chloride dissolved.
_______________________________________________________________________________
______________________________________________________________________________
Density of Liquids Lab
Name _____________________________
Date _______________ Period ________
Introduction:
Have you ever wondered why the oil in bottles salad dressing settles on top of the water and-vinegar mixture? The answer has to do with the different densities of the liquids in the dressing. Oil has a lower density than the water-and-vinegar mixture. When two liquids of different densities are mixed, the liquid that is less dense, in this case the oil, floats above the other liquid.
Density is the mass of a substance per unit volume. The density of any substance is a ratio and may be calculated by dividing the mass of the sample by its volume.
mass
density =
volume
The most common units of measurement for density that you will encounter in this course are g/mL and g/cm3.
When measured at the same temperature and pressure, all samples of a particular substance have the same density regardless of the quantity or shape of the sample. Thus, density is a characteristic property of matter that is often used by chemists to identify a substance.
In this investigation, you will first determine the density of distilled water by finding the density of three separate samples and calculating an average. You will then repeat this procedure for an unknown liquid. Finally, you will compare your measured values with the accepted values for the densities of these liquids and compute the percent error for your results.
Prelab Questions:
1. Define density. What is the formula for density?
2. How can density help you identify an unknown substance?
3. Why is the precision of the laboratory balance that you use in this investigation important? What effect would a less precise balance have on your results?
4. What is the advantage of taking three sets of measurements instead of just one or two when determining the density of each liquid?
5. Why should you avoid skin contact with the unknown solution?
6. Do you expect your measured values for the density of water and the unknown to differ from the accepted values? Explain your answer.
Materials:goggles
balance
apron
graduated cylinderunknown liquidwater
Procedure:Density of Water
1) Mass a 10-mL graduated cylinder to the correct number of places and record data in Table 1.
2) Fill the graduated cylinder with 9-10 mL of distilled water and mass it again. Record in Table 1.
3) Determine the volume of the water using the graduated cylinder. Remember to read at the bottom of the meniscus and to the correct number of places. Record data in Table 1.
4) Repeat steps #1-3 with 2 lesser volumes of water.
5) Empty the graduated cylinder, dry it and go on to step #6.
Density of Unknown
6) Write the mass of the 10-mL graduated cylinder in Table 2.
7) Repeat steps #2-5 with your unknown liquid. Remember to record the liquid # in Table 2.
Data:
TABLE 1: Water
Trial 1
Trial 2
Trial 3
Mass of graduated cylinder and water (g)
Mass of empty graduated cylinder (g)
Mass of water (g)
Volume of water (mL)
Density of water (g/mL)
TABLE 2: Unknown # ________
Trial 1
Trial 2
Trial 3
Mass of graduated cylinder and unknown (g)
Mass of empty graduated cylinder (g)
Mass of unknown (g)
Volume of unknown (mL)
Density of unknown (g/mL)
Calculations:
1) Calculate the mass, volume and density of the water and unknown and write in the data table.
2) Determine the average density of water:
3) Determine the average density of the unknown:
Critical Thinking Questions:
1. Based on your data, which of the liquids in the table below could be your unknown?
________________________________________
TABLE 3: Accepted Values for Density of Various Liquids
LIQUID
DENSITY (g/mL) at 20 (C
Ethanol
0.789
Isopropyl alcohol
0.786
Methanol
0.791
Mineral oil
0.830
W
