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Incompatible Chemicals Environmental Health and Safety 2809 Daley Drive Ames, Iowa 50011-3660 Phone: (515) 294-5359 Fax: (515) 294-9357 www.ehs.iastate.edu 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 Bases – aqueous substance that can accept hydrogen ion activity hydrogen ions. Also called Alkali if OH- ions are involved. EXTREMELY STRONG ACIDS SUPERBASES Fluoroantimonic acid (HSbF6) Butyl lithium (n-BuLi) Magic Acid (FSO3HSbF5) Lithium diisopropylamide (LDA)(C6H14LiN) Carborane superacid H(CHB11Cl11) Lithium diethylamide (LDEA) Fluorosulfuric acid (FSO3H) Sodium amide (NaNH2) Triflic acid (CF3SO3H) Sodium hydride (NaH) Lithium bis(trimethylsilyl) amide (((CH3)3Si)2NLi) STRONG ACIDS (strongest to weakest) Perchloric acid (HClO4) STRONG BASES (strongest to weakest) Hydroiodic acid (HI) Potassium hydroxide (KOH) Hydrobromic acid (HBr) Barium hydroxide (Ba(OH)2) Hydrochloric acid (HCl) Ceasium hydroxide (CsOH) Sulfuric acid (H2SO4) Sodium hydroxide (NaOH) Nitric acid (HNO3) Strontium hydroxide (Sr(OH)2) Calcium hydroxide (Ca(OH)2) WEAK ACIDS Lithium hydroxide (LiOH) Acetic acid (C2H4O2) Rubidium hydroxide (RbOH) Citric acid (C6H8O7) Magnesium hydroxide (Mg(OH)2) Boric acid (H3BO3) Phosphoric acid (H3PO4) ORGANIC BASES (weak) Hydrofluoric acid (HF, weak but very corrosive) 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 Organic Acids – organic compounds (contains atoms and release hydrogen ions when carbon) with acidic properties. Not water dissolved in water. soluble (except *). Boric acid (H3BO3) Acetic acid (C2H4O2) Formic acid* (CH2O2) Chromic acid (H2CrO4) Amino acids Lactic acid* (C3H6O3) Hydrobromic acid (HBr) Arachidic acid Lauric acid (C12H24O2) (C20H40O2) Hydrochloric acid (HCl) Benzoic acid (C7H6O2) Myristic acid (C14H28O2) Hydrofluoric acid (HF) Butyric acid (C4H8O2) Oxalic acid* (C2O4H2) Hydroiodic acid (HI) Capric acid (C10H20O2) Palmitic acid (C16H32O2) Nitric acid (HNO3) Caproic acid (C6H12O2) Pelargonic acid (C9H18O2) Perchloric acid (HClO4) Caprylic acid (C8H16O2) Propionic acid* (C3H6O2) Phosphoric acid (H3PO4) Citric acid* (C6H8O7) Pyruvic acid (C3H4O3) Sulfuric acid (H2SO4) Enanthic acid Stearic acid (C18H36O2) (C7H14O2) Fatty acids Valeric acid (C5H10O2) Oxidizers or Oxidizing Agent – produces Reducing Agents – combines with oxygen oxygen and gains electrons during a or loses electrons to a reaction, thereby reaction; may start or assist the experiencing oxidation. combustion of other materials Ammonium nitrate (NH4NO3) Aluminum (Al) Astatine (At) Carbon (C) Bromine (Br2) Caesium (Cs) Chlorine (Cl2) Chromium (Cr) Chlorite, chlorate, perchlorate and other Copper (Cu) analogous halogen compounds Fluorine (F2) Formic acid (CH2O2) Hexavalent chromium compounds such as Hydrazine (N2H4) Chromic and Dichromic acids and Chromium trioxide, Pyridinium chlorochromate and Chromate/Dichromate Hydrogen peroxide (H2O2) Hydrogen (H2) Iodine (I2) Hydroiodic acid (HI) Nitric acid (HNO3) Iron (Fe) Nitrous oxide (N2O) Lithium (Li) Osmium tetroxide (OsO4) Lithium aluminum hydride (LiAlH4) Oxygen (O2) Magnesium (Mg) Ozone (O3) Nitrites Perchloric acid (HClO4) Organic materials Permanganates Oxalic acid (C2O4H2) Peroxide compounds Phosphorus (P) Potassium nitrate (KNO3) Potassium (K) Sodium hypochlorite (NaOCl, bleach) Rubidium (Rb) Sulfuric acid (H2SO4) 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 .
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