Chemistry 112L -- General Chemistry Laboratory I
Tentative Laboratory Schedule Fall 2008
Date Lab Number Title
8/26 or 8/27 XXX Lab Safety and Procedures, Check Out Equipment
9/2 or 9/3 110 The Metric System
9/9 or 9/10 111 Measurement of Density
9/16 or 9/17 113 Determination of Iron
9/23 or 9/24 114 Energy Changes in Physical Processes
9/30 or 10/1 115 Energy Changes in Chemical Processes
10/7 or 10/8 120 Anion Analysis
10/14 or 10/15 122 Group I Cation Analysis
10/21 or 10/22 124 Group II Cation Analysis
10/28 or 10/29 117 Determination of the Formula of a Hydrate
11/4 or 11/5 118 Determination of a Chemical Formula
11/11 or 11/12 140 Standardization of Sodium Hydroxide
11/18 or 11/19 142 Determination of the Concentration of an Unknown Acids
11/25 or 11/26 XXX No Lab Scheduled - Thanksgiving Vacation
12/2 or 12/3 145 Buffer Solutions
12/9 or 12/10 XXX Check In Equipment
Except under unusual circumstances, students will not be permitted to make-up more than two labs. All labs must be made-up within two weeks of the day that the lab was missed. Graded lab reports will normally be returned two weeks after the scheduled completion date. 

Laboratory Objectives

  1. Learn the value of clean glassware in the first experiment, and use clean glassware for the remainder of the semester.
Experiment 110
  1. Be able to define: Meniscus, accuracy, precision, percent error.
  2. Be able to accurately measure length, volume and mass.
  3. Become familiar with metric units for measuring length, volume and mass.
  4. Know the SI units as well as commonly used units for each of the measurements.
  5. Be able to calculate the relationship between the English and metric units of measurement.
  6. Be able to correctly use significant figures in measurements and calculations.
  7. Be able to use dimensional analysis to perform conversions.
  8. Be able to perform calculations to determine percent error.
Experiment 111
  1. Be able to define: Density.
  2. Be able to accurately measure the density of a solid or liquid.
  3. Be able to compare the results of two experiments and determine which data is more reliable.
  4. Be able to use dimensional analysis to perform calculations.
  5. Be able to perform calculations to determine percent error.
  6. Improve your ability to use significant figures correctly.
  7. Be able to explain why units of g/mL or g/cm3 are used with density.
Experiment 113
  1. Be able to define: ppm, ion.
  2. Become familiar with the preparation and use of standard curves.
  3. Gain an understanding of the units of concentration used to express hardness (parts per million, ppm).
  4. Accurately determine the iron content of water samples.
  5. Become familiar with, and proficient in the use of, volumetric glassware.
Experiment 114
  1. Be able to define: Calorie, calorie, joule, energy, specific heat, heat of fusion, heat of vaporization, calorimeter.
  2. Understand the concept of energy and the unit used to measure energy changes (calorie).
  3. Use a calorimeter to measure energy changes.
  4. Calculate the heat of fusion for ice from experimental measurements.
  5. Measure the conversion of electrical energy into thermal energy.
  6. Be able to perform calculations to determine the amount of energy required or released by a chemical or physical change.
Experiment 115
  1. Be able to define: heat of solution, hygroscopic, heat of reaction, endothermic, exothermic.
  2. Understand the concept of energy and the unit used to measure energy changes (calorie).
  3. Use a calorimeter to measure energy changes.
  4. Measure the heat absorbed or evolved when an ionic compound dissolves in water.
  5. Measure the heat of reaction for a chemical reaction.
  6. Be able to perform calculations from experimental data to determine the heat of solution or heat of reaction.
Experiment 120
  1. Be able to define: qualitative analysis, anion, supernate, precipitate.
  2. Become familiar with the methods for qualitative analysis of anions.
  3. Be able to analyze a known mixture of anions.
  4. Accurately determine the anions present in an unknown mixture.
Experiment 122
  1. Be able to define: deionized water, cation, group I cation.
  2. Become familiar with the methods for qualitative analysis of cations.
  3. Be able to analyze a known mixture of Group I cations.
  4. Accurately determine the cations present in an unknown mixture.
Experiment 124
  1. Be able to define: decant, cation, group II cation.
  2. Become familiar with the methods for qualitative analysis of cations.
  3. Be able to analyze a known mixture of Group II cations.
  4. Accurately determine the cations present in an unknown mixture.
Experiment 117
  1. Be able to define: hydrate, crucible, mole.
  2. Become familiar with weight relations in chemical reactions.
  3. Be able to determine the percent of water in a hydrate.
  4. Accurately determine the formula of a hydrate.
Experiment 118
  1. Be able to define: emperical formula, molecular formula.
  2. Become familiar with weight relations in chemical reactions.
  3. Be able to determine the percent composition of a chemical compound.
  4. Accurately determine the emperical formula for a chemical compound.
Experiment 140
  1. Be able to define: acid, base, neutralization, titration, normal solution, molarity, equivalence point.
  2. Become familiar with acids, bases and the reactions of acids and bases.
  3. Gain familiarity with normality as a unit of concentration and with the concept of equivalents.
  4. Prepare a standard solution of acid.
  5. Standardize a solution of sodium hydroxide.
  6. Become familiar with the calculations involved in acid-base titrations.
Experiment 142
  1. Be able to define: no new terms.
  2. Become familiar with acids, bases and the reactions of acids and bases.
  3. Gain familiarity with normality as a unit of concentration and with the concept of equivalents.
  4. Use a standard sodium hydroxide solution in the volumetric analysis of an acid solution.
  5. Become familiar with the calculations involved in acid-base titrations.
Experiment 145
  1. Be able to define: buffer.
  2. Learn the differences between a buffered solution and an unbuffered solution.
  3. Prepare a buffer solution and study the properties of the solution.
  4. To appreciate the importance of pH control.