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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 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