Download Incompatible Chemicals

Environmental Health and Safety
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Phone: (515) 294-5359
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Incompatible Chemicals
On the topic of incompatibility Pohanish and Greene state that: “The term incompatibility is used to
describe a wide range of chemical reactions that might include the generation of heat resulting
from contact of a chemical with moisture; decomposition; the generation of toxic gases; the
heating, overflow, and rupture of containers; polymerization; the formation of new and possibly
more dangerous compounds; fire, detonation, and explosion; or any combination of these or other
actions.”
Today, most chemical manufacturers have settled on a five color scheme used on container labels
for segregating chemicals. Red for flammables, blue for health hazards, yellow for oxidizers, white
for corrosives, and a fifth color for less hazardous materials. The following tables are provided to
assist laboratories with storage of reactive chemicals when container labels do not include
segregation colors. In each table, chemicals listed on the left may react with chemicals listed on
the right. Reaction rates and intensities will vary based on concentration of the reactant chemicals.
Refer to container labels and safety data sheets (SDS) for storage requirements for chemicals
stored in your area. Where possible, store reactive chemicals separated by distance, location or
through use of secondary containment.
Acids – dissolves in water and gives solution
hydrogen ion activity
EXTREMELY STRONG ACIDS
Fluoroantimonic acid (HSbF6)
Magic Acid (FSO3HSbF5)
Carborane superacid H(CHB11Cl11)
Fluorosulfuric acid (FSO3H)
Triflic acid (CF3SO3H)
STRONG ACIDS (strongest to weakest)
Perchloric acid (HClO4)
Hydroiodic acid (HI)
Hydrobromic acid (HBr)
Hydrochloric acid (HCl)
Sulfuric acid (H2SO4)
Nitric acid (HNO3)
WEAK ACIDS
Acetic acid (C2H4O2)
Citric acid (C6H8O7)
Boric acid (H3BO3)
Phosphoric acid (H3PO4)
Hydrofluoric acid (HF, weak but very corrosive)
Bases – aqueous substance that can accept
hydrogen ions. Also called Alkali if OH- ions are
involved.
SUPERBASES
Butyl lithium (n-BuLi)
Lithium diisopropylamide (LDA)(C6H14LiN)
Lithium diethylamide (LDEA)
Sodium amide (NaNH2)
Sodium hydride (NaH)
Lithium bis(trimethylsilyl) amide (((CH3)3Si)2NLi)
STRONG BASES (strongest to weakest)
Potassium hydroxide (KOH)
Barium hydroxide (Ba(OH)2)
Ceasium hydroxide (CsOH)
Sodium hydroxide (NaOH)
Strontium hydroxide (Sr(OH)2)
Calcium hydroxide (Ca(OH)2)
Lithium hydroxide (LiOH)
Rubidium hydroxide (RbOH)
Magnesium hydroxide (Mg(OH)2)
ORGANIC BASES (weak)
Pyridine (C5H5N)
Methyl amine (CH3NH2)
Imidazole (C2H4N2)
Benzimidazole (C7H6N2)
Histidine (C6H9N3O2)
Phosphazene bases
Hydroxides of some organic cations
Alanine (C3H5O2NH2)
Ammonia (NH3)
Reviewed 2015
Mineral Acids – contains no carbon
atoms and release hydrogen ions when
dissolved in water.
Boric acid (H3BO3)
Chromic acid (H2CrO4)
Hydrobromic acid (HBr)
Hydrochloric acid (HCl)
Hydrofluoric acid (HF)
Hydroiodic acid (HI)
Nitric acid (HNO3)
Perchloric acid (HClO4)
Phosphoric acid (H3PO4)
Sulfuric acid (H2SO4)
Oxidizers or Oxidizing Agent – produces
oxygen and gains electrons during a
reaction; may start or assist the
combustion of other materials
Ammonium nitrate (NH4NO3)
Astatine (At)
Bromine (Br2)
Chlorine (Cl2)
Chlorite, chlorate, perchlorate and other
analogous halogen compounds
Fluorine (F2)
Hexavalent chromium compounds such as
Chromic and Dichromic acids and Chromium
trioxide, Pyridinium chlorochromate and
Chromate/Dichromate
Hydrogen peroxide (H2O2)
Iodine (I2)
Nitric acid (HNO3)
Nitrous oxide (N2O)
Osmium tetroxide (OsO4)
Oxygen (O2)
Ozone (O3)
Perchloric acid (HClO4)
Permanganates
Peroxide compounds
Potassium nitrate (KNO3)
Sodium hypochlorite (NaOCl, bleach)
Sulfuric acid (H2SO4)
Organic Acids – organic compounds (contains
carbon) with acidic properties. Not water
soluble (except *).
Acetic acid (C2H4O2)
Formic acid* (CH2O2)
Amino acids
Lactic acid* (C3H6O3)
Arachidic acid
Lauric acid (C12H24O2)
(C20H40O2)
Benzoic acid (C7H6O2)
Myristic acid (C14H28O2)
Butyric acid (C4H8O2)
Oxalic acid* (C2O4H2)
Capric acid (C10H20O2)
Palmitic acid (C16H32O2)
Caproic acid (C6H12O2) Pelargonic acid
(C9H18O2)
Caprylic acid (C8H16O2) Propionic acid* (C3H6O2)
Citric acid* (C6H8O7)
Pyruvic acid (C3H4O3)
Enanthic acid
Stearic acid (C18H36O2)
(C7H14O2)
Fatty acids
Valeric acid (C5H10O2)
Reducing Agents – combines with oxygen
or loses electrons to a reaction, thereby
experiencing oxidation.
Aluminum (Al)
Carbon (C)
Caesium (Cs)
Chromium (Cr)
Copper (Cu)
Formic acid (CH2O2)
Hydrazine (N2H4)
Hydrogen (H2)
Hydroiodic acid (HI)
Iron (Fe)
Lithium (Li)
Lithium aluminum hydride (LiAlH4)
Magnesium (Mg)
Nitrites
Organic materials
Oxalic acid (C2O4H2)
Phosphorus (P)
Potassium (K)
Rubidium (Rb)
Silicon (Si)
Silver (Ag)
Sodium (Na)
Sodium borohydride (NaBH4)
Sulfur (S)
Tin (Sn)
Reviewed 2015
Special Hazards
Segregate oxidizing acids (nitric, perchloric and chromic) from all other materials.
Store water reactives away from water sources or aqueous solutions. Examples include metals
such as sodium and potassium; acid anhydrides and acid chlorides; and fine metal powders such
as zinc.
Store pyrophoric chemicals (butyllithium, methyllithium, white phosphorus, etc.) in an inert
environment. To be used with extreme caution, by trained personnel. Refer to page 23 of the
Laboratory Safety Manual for more information.
References
National Research Council. 1995. Prudent Practices in the Laboratory: Handling and Disposal of
Chemicals. Washington, D.C.: National Academy Press.
Lewis, Richard J. 2007. Hawley’s Condensed Chemical Dictionary. 15th Edition. New York: John
Wiley & Sons, Inc.
Pohanish, Richard P., & Greene, Stanley A., 1997. Rapid Guide to Chemical Incompatibilities. New
York: Van Nostrand Reinhold.
Reviewed 2015