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Home , Enanthic acid, Fluorosulfuric acid, Magic acid, Perchloric acid, Rubidium hydroxide, Strontium hydroxide

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 activity hydrogen . Also called if OH- ions are involved. EXTREMELY STRONG Fluoroantimonic (HSbF6) Butyl lithium (n-BuLi) (FSO3HSbF5) Lithium diisopropylamide (LDA)(C6H14LiN) Carborane H(CHB11Cl11) Lithium diethylamide (LDEA) (FSO3H) Sodium amide (NaNH2) (CF3SO3H) Sodium hydride (NaH) Lithium bis(trimethylsilyl) amide (((CH3)3Si)2NLi) STRONG ACIDS (strongest to weakest) (HClO4) STRONG BASES (strongest to weakest) Hydroiodic acid (HI) Potassium (KOH) Hydrobromic acid (HBr) (Ba(OH)2) (HCl) Ceasium hydroxide (CsOH) (H2SO4) (NaOH) (HNO3) hydroxide (Sr(OH)2) (Ca(OH)2) WEAK ACIDS (LiOH) (C2H4O2) hydroxide (RbOH) Citric acid (C6H8O7) (Mg(OH)2) Boric acid (H3BO3) Phosphoric acid (H3PO4) ORGANIC BASES (weak) (HF, weak but very corrosive) Pyridine (C5H5N) Methyl amine (CH3NH2) Imidazole (C2H4N2) Benzimidazole (C7H6N2) Histidine (C6H9N3O2) Phosphazene bases 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) (C12H24O2) (C20H40O2) Hydrochloric acid (HCl) Benzoic acid (C7H6O2) (C14H28O2) Hydrofluoric acid (HF) (C4H8O2) Oxalic acid* (C2O4H2) Hydroiodic acid (HI) (C10H20O2) (C16H32O2) Nitric acid (HNO3) (C6H12O2) (C9H18O2) Perchloric acid (HClO4) (C8H16O2) * (C3H6O2) Phosphoric acid (H3PO4) Citric acid* (C6H8O7) Pyruvic acid (C3H4O3) Sulfuric acid (H2SO4) Enanthic acid (C18H36O2) (C7H14O2) Fatty acids (C5H10O2)

Oxidizers or – produces Reducing Agents – combines with 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 nitrate (NH4NO3) Aluminum (Al) (At) Carbon (C) Bromine (Br2) Caesium (Cs) (Cl2) Chromium (Cr) Chlorite, chlorate, 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) (I2) Hydroiodic acid (HI) Nitric acid (HNO3) Iron (Fe) Nitrous (N2O) Lithium (Li) Osmium tetroxide (OsO4) Lithium aluminum hydride (LiAlH4) Oxygen (O2) Magnesium (Mg) (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