- •Contents
- •Foreword
- •Preface
- •1 Materials in the Lab
- •2 Measurement
- •3 Joints, Stopcocks, and Glass Tubing
- •4 Cleaning Glassware
- •5 Compressed Gases
- •6 High and Low Temperature
- •7 Vacuum Systems
- •8 The Gas-Oxygen Torch
- •APPENDIX
- •Appendix A Preparing Drawings for a Technician
- •Index
- •Foreword
- •Preface
- •For the Second Edition
- •Please note:
- •1 Materials in the Lab
- •1.1 Glass
- •1.1.1 Introduction
- •1.1.2 Structural Properties of Glass
- •1.1.3 Phase Separation
- •1.1.4 Devitrification
- •1.1.5 Different Types of Glass Used in the Lab
- •1.1.6 Grading Glass and Graded Seals
- •1.1.7 Separating Glass by Type
- •1.1.9 Stress in Glass
- •1.1.11 Tempered Glass
- •1.1.13 Limiting Broken Glass in the Lab
- •1.1.14 Storing Glass
- •1.1.15 Marking Glass
- •1.1.16 Consumer's Guide to Purchasing Laboratory Glassware
- •1.2 Flexible Tubing
- •1.2.1 Introduction
- •1.2.2 Physical Properties of Flexible Tubing
- •1.3 Corks, Rubber Stoppers, and Enclosures
- •1.3.1 Corks
- •1.3.2 Rubber Stoppers
- •1.3.3 Preholed Stoppers
- •1.3.4 Inserting Glass Tubing into Stoppers
- •1.3.5 Removing Glass from Stoppers and Flexible Tubing
- •1.3.6 Film Enclosures
- •1.4 O-Rings
- •1.4.2 Chemical Resistance of O-Ring Material
- •1.4.3 O-Ring Sizes
- •2 Measurement
- •2.1 Measurement: The Basics
- •2.1.1 Uniformity, Reliability, and Accuracy
- •2.1.2 History of the Metric System
- •2.1.3 The Base Units
- •2.1.4 The Use of Prefixes in the Metric System
- •2.1.5 Measurement Rules
- •2.2 Length
- •2.2.1 The Ruler
- •2.2.2 How to Measure Length
- •2.2.3 The Caliper
- •2.2.4 The Micrometer
- •2.3 Volume
- •2.3.1 The Concepts of Volume Measurement
- •2.3.2 Background of Volume Standards
- •2.3.4 Materials of Volumetric Construction #1 Plastic
- •2.3.5 Materials of Volumetric Construction #2 Glass
- •2.3.6 Reading Volumetric Ware
- •2.3.7 General Practices of Volumetric Ware Use
- •2.3.8 Calibrations, Calibration, and Accuracy
- •2.3.9 Correcting Volumetric Readings
- •2.3.10 Volumetric Flasks
- •2.3.11 Graduated Cylinders
- •2.3.12 Pipettes
- •2.3.13 Burettes
- •2.3.14 Types of Burettes
- •2.3.15 Care and Use of Burettes
- •2.4 Weight and Mass
- •2.4.1 Tools for Weighing
- •2.4.2 Weight Versus Mass Versus Density
- •2.4.3 Air Buoyancy
- •2.4.5 Balance Location
- •2.4.6 Balance Reading
- •2.4.7 The Spring Balance
- •2.4.8 The Lever Arm Balance
- •2.4.9 Beam Balances
- •2.4.10 Analytical Balances
- •2.4.11 The Top-Loading Balance
- •2.4.12 Balance Verification
- •2.4.13 Calibration Weights
- •2.5 Temperature
- •2.5.1 TheNature of Temperature Measurement
- •2.5.2 The Physics of Temperature-Taking
- •2.5.3 Expansion-Based Thermometers
- •2.5.4 Linear Expansion Thermometers
- •2.5.5 Volumetric Expansion Thermometers
- •2.5.7 Thermometer Calibration
- •2.5.8 Thermometer Lag
- •2.5.9 Air Bubbles in Liquid Columns
- •2.5.10 Pressure Expansion Thermometers
- •2.5.11 Thermocouples
- •2.5.12 Resistance Thermometers
- •3.1 Joints and Connections
- •3.1.1 Standard Taper Joints
- •3.1.2 Ball-and-Socket Joints
- •3.1.3 The O-Ring Joint
- •3.1.4 Hybrids and Alternative Joints
- •3.1.5 Special Connectors
- •3.2 Stopcocks and Valves
- •3.2.1 Glass Stopcocks
- •3.2.2 Teflon Stopcocks
- •3.2.3 Rotary Valves
- •3.2.4 Stopcock Design Variations
- •3.3.1 Storage and Use of Stopcocks and Joints
- •3.3.2 Preparation for Use
- •3.3.3 Types of Greases
- •3.3.4 The Teflon Sleeve
- •3.3.5 Applying Grease to Stopcocks and Joints
- •3.3.6 Preventing Glass Stopcocks and Joints from Sticking or Breaking on a Working System
- •3.3.7 Unsticking Joints and Stopcocks
- •3.3.8 Leaking Stopcocks and Joints
- •3.3.9 What to Do About Leaks in Stopcocks and Joints
- •3.3.10 General Tips
- •3.4 Glass Tubing
- •3.4.1 The Basics of Glass Tubing
- •3.4.2 Calculating the Inside Diameter (I.D.)
- •3.4.3 Sample Volume Calculations
- •4 Cleaning Glassware
- •4.1 The Clean Laboratory
- •4.1.1 Basic Cleaning Concepts
- •4.1.2 Safety
- •4.1.3 Removing Stopcock Grease
- •4.1.4 Soap and Water
- •4.1.5 Ultrasonic Cleaners
- •4.1.6 Organic Solvents
- •4.1.7 The Base Bath
- •4.1.8 Acids and Oxidizers
- •4.1.9 Chromic Acid
- •4.1.10 Hydrofluoric Acid
- •4.1.11 Extra Cleaning Tips
- •4.1.12 Additional Cleaning Problems and Solutions
- •4.1.13 Last Resort Cleaning Solutions
- •5 Compressed Gases
- •5.1 Compressed GasTanks
- •5.1.1 Types of Gases
- •5.1.2 The Dangers of Compressed Gas
- •5.1.3 CGA Fittings
- •5.1.4 Safety Aspects of Compressed Gas Tanks
- •5.1.5 Safety Practices Using Compressed Gases
- •5.1.6 In Case of Emergency
- •5.1.7 Gas Compatibility with Various Materials
- •5.2 The Regulator
- •5.2.1 The Parts of the Regulator
- •5.2.2 House Air Pressure System
- •5.2.4 How to Use Regulators Safely
- •5.2.6 How to Purchase a Regulator
- •6 High and Low Temperature
- •6.1 High Temperature
- •6.1.1 TheDynamics of Heat in the Lab
- •6.1.2 General Safety Precautions
- •6.1.3 Open Flames
- •6.1.4 Steam
- •6.1.5 Thermal Radiation
- •6.1.6 Transfer of Energy
- •6.1.7 Hot Air Guns
- •6.1.8 Electrical Resistance Heating
- •6.1.9 Alternatives to Heat
- •6.2 Low Temperature
- •6.2.1 TheDynamics of Cold in the Lab
- •6.2.2 Room Temperature Tap Water (=20°C)
- •6.2.8 Safety with Slush Baths
- •6.2.9 Containment of Cold Materials
- •6.2.10 Liquid (Cryogenic) Gas Tanks
- •7 Vacuum Systems
- •7.1 How to Destroy a Vacuum System
- •7.2.1 Preface
- •7.2.2 How to Use a Vacuum System
- •7.2.4 Pressure, Vacuum, and Force
- •7.2.5 Gases, Vapors, and the Gas Laws
- •7.2.6 Vapor Pressure
- •7.2.7 How to Make (and Maintain) a Vacuum
- •7.2.8 Gas Flow
- •7.2.9 Throughput and Pumping Speed
- •7.3 Pumps
- •7.3.1 The Purpose of Pumps
- •7.3.2 The Aspirator
- •7.3.3 Types and Features of Mechanical Pumps
- •7.3.4 Connection, Use, Maintenance, and Safety
- •7.3.5 Condensable Vapors
- •7.3.6 Traps for Pumps
- •7.3.7 Mechanical Pump Oils
- •7.3.8 The Various Mechanical Pump Oils
- •7.3.9 Storing Mechanical Pumps
- •7.3.11 Ultra-High Vacuum Levels Without Ultra-High
- •7.3.12 Diffusion Pumps
- •7.3.13 Attaching a Diffusion Pump to a Vacuum System
- •7.3.14 How to Use a Diffusion Pump
- •7.3.15 Diffusion Pump Limitations
- •7.3.17 Diffusion Pump Maintenance
- •7.3.18 Toepler Pumps
- •7.4 Traps
- •7.4.1 The Purpose and Functions of Traps
- •7.4.2 Types of Traps
- •7.4.3 Proper Use of Cold Traps
- •7.4.4 Maintenance of Cold Traps
- •7.4.5 Separation Traps
- •7.4.6 Liquid Traps
- •7.5 Vacuum Gauges
- •7.5.2 The Mechanical Gauge Family
- •7.5.4 The Liquid Gauge Family
- •7.5.5 The Manometer
- •7.5.6 The McLeod Gauge
- •7.5.7 How to Read a McLeod Gauge
- •7.5.8 Bringing a McLeod Gauge to Vacuum Conditions
- •7.5.10 The Tipping McLeod Gauge
- •7.5.11 Condensable Vapors and the McLeod Gauge
- •7.5.12 Mercury Contamination from McLeod Gauges
- •7.5.13 Cleaning a McLeod Gauge
- •7.5.14 Thermocouple and Pirani Gauges
- •7.5.15 The Pirani Gauge
- •7.5.16 Cleaning Pirani Gauges
- •7.5.17 The Thermocouple Gauge
- •7.5.18 Cleaning Thermocouple Gauges
- •7.5.19 The lonization Gauge Family
- •7.5.20 The Hot-Cathode Ion Gauge
- •7.5.21 Cleaning Hot-Cathode Ion Gauges
- •7.5.24 The Momentum Transfer Gauge (MTG)
- •7.6 Leak Detection and Location
- •7.6.1 AllAbout Leaks
- •7.6.3 False Leaks
- •7.6.4 Real Leaks
- •7.6.5 Isolation to Find Leaks
- •7.6.6 Probe Gases and Liquids
- •7.6.7 The Tesla Coil
- •7.6.8 Soap Bubbles
- •7.6.9 Pirani or Thermocouple Gauges
- •7.6.10 Helium Leak Detection
- •7.6.11 Helium Leak Detection Techniques
- •7.6.13 Repairing Leaks
- •7.7 More Vacuum System Information
- •7.7.1 The Designs of Things
- •8 The Gas-Oxygen Torch
- •8.1.2 How to Light a Gas-Oxygen Torch
- •8.1.3 How to Prevent a Premix Torch from Popping
- •8.2.2 How to Tip-Off a Sample
- •8.2.3 How to Fire-Polish the End of a Glass Tube
- •8.2.4 Brazing and Silver Soldering
- •Appendix
- •A.2 Suggestions for Glassware Requests
- •B.1 Introduction
- •B.2 Polyolefins
- •B.3 Engineering Resins
- •B.4 Fluorocarbons
- •B.5 Chemical Resistance Chart
- •C.1 Chapter 1
- •C.4 Chapter 4
- •C.5 Chapter 5 & Chapter 6
- •C.6 Chapter 7
- •C.7 Chapter 8
- •D.1 Laboratory Safety
- •D.2 Chemical Safety
- •D.3 Chapter 1
- •D.4 Chapter 2
- •D.5 Chapter 3
- •D.6 Chapter 4
- •D.7 Chapter 5 and the Second Half of Chapter 6
- •D.8 Chapter 7
- •D.9 Chapter 8
- •Index
248 |
Cleaning Glassware |
hydroxide (Na(OH)2 or K(OH)2) because sodium and potassium fluorides are highly poisonous.
4.1.11 Extra Cleaning Tips
Cleaning Fritted Filters. Because of the nature of fritted glass, its cleaning requires special mention. Fritted glass is crushed glass (Ace Glass uses crushed glass fibers) separated by size, compacted together, then heated until the pieces stick together. Because the structure is loosely connected, the frit maintains its porous nature, which provides the frit its filtering abilities.
Because different materials get onto and in a frit, different cleaning processes are required to clean a frit. For this reason, storage is an important aspect of frit cleaning. If you know what got on a frit, you know how to clean it. Keeping a frit in a clean, dry, and dust-free area will simplify your cleaning needs. Before a fritted filter is first used, it should be rinsed with hot sulfuric acid and then with distilled water until the filtrate is neutral in pH. This procedure will remove any glass particles and dust that may be on the new frit.
After a frit has just been used, it is important to flush it immediately with distilled water in the opposite direction that it was used. Then proceed with a chemical cleaning. Once the fritted glass is cleaned, rinsed, and dried, store it in a clean, dry, and dust-free area. Some suggested contamination and appropriate cleaning solutions are as follows :
•Fats; Carbon tetrachloride
•Silver chloride; Ammonia
• |
Albumen; Warm ammonia or hydrochloric acid |
• |
Nitric acid: Hot hydrochloric acid with potassium chlorate |
• |
Barium sulfate: Hot concentrated sulfuric acid |
•Organic materials: Potassium permanganate
•General cleaning: Potassium permanganate^
Because of the effects of basic solutions on glass, never let a basic solution (such as NaOH or KOH) remain in contact with a fritted glass filter. Rinse with hydrochloric acid and then with distilled water until the filtrate is neutral in pH.
Removing Tungsten from Glassware. A dark film of tungsten is often deposited on the walls of components of glass vacuum systems having tungsten filaments. This deposit hinders observation within the glassware and can also cause an increase in wall temperature.
Although a solution of HF, or a mixture of HF and HNO3, can remove the tungsten stain, it also removes some of the glass, which can etch the glass and thereby increase pumping time due to increased surface area. If the HF solution is left too
*Treat the filter with a 1% aqueous solution of potassium permanganate followed by a few drops of concentrated sulfuric acid. The heat of the reaction will increase the oxidizing power of the mixture. tTreat the filter with a 1% aqueous solution of potassium permanganate followed by a few drops of concentrated sulfuric acid. The heat of the reaction will increase the oxidizing power of the mixture.
The Clean Laboratory 4.1 |
249 |
Flask
Beaker
Fig.4.4 Removing tar from a flask.
long, the glass can become dangerously thin for a vacuum system.
A tungsten coating can be removed quite successfully with a hypochlorite solution (Clorox bleach, for example). A black opaque coating can be removed in a few minutes, and, if the solution is warmed, the process is even faster. The solution can be reused many times.
Removing Tar from Distillation Flasks. As mentioned in the beginning of this section, the best time to clean glassware is immediately after it is used. The hardest glass pieces to clean are those that have been left for someone else to clean. Tar, however, is always hard to clean and is always left for last (which also makes it more difficult to clean). A simple solution for cleaning tar from the bottom of flasks is to invert the flask into a beaker of acetone and let the vapor of the solvent dissolve the tar (see Fig. 4.4). This technique can remove most of the tar deposit in a few hours. It can be hastened by heating the solvent in a steam bath (do not use an open flame).
The trick to this technique is getting the solvent into the neck of the upsidedown flask. One method is to lightly heat the flask before inserting it into the solvent. Then, as the flask cools, the solvent will be drawn into the flask. Perhaps the simplest method is to place a flexible tube into the neck to allow air out of the flask as it is inverted into the beaker (be sure the tube is not soluble in the solvent).
4.1.12 Additional Cleaning Problems and Solutions15
In the following cleaning procedures, all work should be done in a fume hood, hand and eye protection should be worn, and a lab apron is recommended. After cleaning, an item should be thoroughly rinsed in water followed by a rinse in distilled water. If an item needs to be dried, a final rinse in reagent-grade methanol, ethyl alcohol, or acetone can be used.
Iron Stains. Equal parts hydrochloric acid and water should be used.
Mercury Residue. Use hot nitric acid. The acid used should be collected and returned to your safety supervisor because it now contains a heavy metal and should not be rinsed down the sink under any circumstances.
250 Cleaning Glassware
Permanganate Stains. Use concentrated hydrochloric acid or a saturated solution of oxalic acid at room temperature.
Bacteriological Material. Soak the glassware in a weak Lysol® solution, or autoclave in steam. A number of sources recommend soaking the glassware in a 2% to 4% cresol solution. However, the EPA has recently identified cresol as a hazardous material. Because other options are readily available (see Sec. 4.1.1 through Sec. 4.1.9), there is no reason to use the material. If you have any cresol, contact a hazardous materials disposal firm in your area for removal.
Albuminous Materials. Soak in nitric acid.
Carbonaceous Materials. Soak in a solution of equal parts sulfuric and nitric acid. Be aware of the possible formation of dangerous compounds when organic material is present.
Magnesium Oxide Stains. Instead of HC1, try a 20% to 30% solution of sodium bisulfite (NaHSO3). Because an acid is not being used, SO2 is not liberated.14
4.1.13 Last Resort Cleaning Solutions15
The following solutions should only be used as last resorts for cleaning glassware because of the dangers each present. Each is meant to be used as a soaking solution for glassware and should be left in a fume hood at all times. After soaking, rinse off the solution with copious amounts of water. Before using any of the following materials, strongly consider whether the glassware is worth cleaning.
Alkaline Peroxide. This material is good for removing organics.
Place 100 g of NaOH (sodium hydroxide) into a 500-mL glass beaker. Slowly add 250 mL of water. This solution will get hot (120°C), bubble, and fizzle. Therefore gloves and eye protection are a must.
This material can etch glass if it is left to soak for an extended period of time, therefore you might wish to select an old, worn beaker in which to do the mixing. You must use a glass beaker because of the exothermic reaction that is created when the mixture is first mixed.
If this solution is in a container and allowed to get cold, it can begin to deposit out of solution. The solid can be removed by slowly adding water or a dilute acid.
Alkaline Permanganate. This material is good for removing siliceous deposits and acidic crud.
Place 500 g to 1 kg of NaOH (Sodium Hydroxide) in a 5-liter beaker. Add 4 V2 liters of water. Once dissolved, add 50 mg of KMnO4 (potassium permanganate). This solution will be purple and, after leaving it overnight to allow it to become active, will turn green.
This mixture can be used up to one year. It should be covered to reduce evaporation. During that time some water will evaporate leaving a brown crust of MnO^ This crust can be knocked back into the remaining solution. If too much water has evaporated, simply add water to original levels. If the solution leaves a brown deposit on glassware, the deposit can be removed with HC1 (hydrochloric acid).
References |
251 |
Besides damaging skin tissue, this solution can also stain skin, so be sure to use gloves.
Fuming Sulfuric Acid. This material is good for a wide variety of contaminants.
Use a small amount of heated sulfuric acid in a fume hood. Roll the item around so the acid comes in contact will all areas of the piece. Unless the item needs to soak (for example, 30 minutes of soaking time is recommended for the removal of silicone grease), immediately empty the glassware and rinse. Although more dangerous to use than a base bath, this technique can be used to remove silicone grease from volumetric ware without concerns about altering the volume of volumetric ware.
References
1.F. Sherwood Rowland, "Chlorofluorocarbons and the Depletion of Stratospheric Ozone," American Scientist, 77, pp. 36-45 (1989).
2.Margaret-Ann Armour, "Chemical Waste Management and Disposal," Journal of Chemical Education, 65,pp.A64-8 (1988).
3.Ibid, Ref. 2.
4.P.L. Manske, T.M. Stimpfel, and E.L. Gershey, "A Less Hazardous Chromic Acid Substitute for Cleaning Glassware," Journal of Chemical Education, 67, pp. A280-A282 (1990).
5.L. Holland, The Properties of Glass Surfaces John Wiley & Sons, Inc., NewYork, 1964, p. 295.
6.Dr. Cathy Cobb, personal communication.
7.Pope Pacers (a publication of Pope Scientific), Menomonee Falls, WI 53052, March 1966, p. 17.
8.James Merritt, personal conversation, Nov. 1996.
9.National Research Council, Prudent Practices for Disposal of Chemicalsfrom Laboratories, National Academy Press, Washington D.C., 1983, p.86.
10.Ibid, Ref. 7, p.15.
11.R.W.Burns, "To Remove Stains of Evaporated Tungsten from Inside of Glass Envelopes," Review of Scientific Instruments, 44, p. 1409(1973).
12.E.J. Eisenbraun, "Solvent Saving Procedure for Removing Tar from Distillation
Flasks," Journal of Chemical Education, 63,p. 553 (1986).
13.Kontes Catalogue, 1989, p. XIV.
14.R.E. Schaffrath, "A Suggestion for Cleaning Glassware Coated with MnO2," Journal
of Chemical Education, 43,p. 578 (1966).
15. . P. Page, "Cleaning Solutions for Glassware," British Society of Scientific Glassblowers Journal, 27, p. 122(1989).