The Henry's Law constant for quinoline is estimated as 1.7X10-6 atm-cu m/mole(SRC) derived from its vapor pressure, 0.06 mm Hg(1), and water solubility, 6,110 mg/l(2). This Henry's Law constant indicates that quinoline is expected to volatilize from water surfaces(3). Based on this Henry's Law constant, the volatilization half-life from a model river (1 m deep, flowing 1 m/sec, wind velocity of 3 m/sec)(3) is estimated as 25 days(SRC). The volatilization half-life from a model lake (1 m deep, flowing 0.05 m/sec, wind velocity of 0.5 m/sec)(3) is estimated as 186 days(SRC). Quinoline is not expected to volatilize from dry soil surfaces(SRC) based upon its vapor pressure(1).
Literature: (1) Daubert TE, Danner RP; Physical and Thermodynamic Properties of Pure Chemicals Data Compilation. Washington, DC: Taylor and Francis (1989) (2) Smith JH et al; Environmental pathways of selected chemicals in freshwater systems. Part II. Athens, GA: USEPA-600/7-78-074 (1978) (3) Lyman WJ et al; Handbook of Chemical Property Estimation Methods. Washington, DC: Amer Chem Soc pp. 15-1 to 15-29 (1990)
The measured log Koc for quinoline is 2.84(1). The adsorption coefficients of quinoline to Ca-montmorillonite and creek sediments are 7.3 and 10.9, respectively(2). A Koc of 43 was reported using low-organic-carbon subsurface materials(11). According to a classification scheme(3), these Koc values suggest that quinoline is expected to have very high mobility in soil. Quinoline was found to be relatively mobile using a Danish sandy soil(10). Intensity of quinoline added to a natural sand aquifer on the Canadian Air Force Base Borden, Ontario, Canada via a field study using coal tar creosote were found to increase after 278 days, about 25 m from the croesote source, added at an initial concn of 10.1 g/kg creosote(4). Aromatic amines are expected to bind strongly to humus or organic matter in soils due to the high reactivity of the aromatic amino group(7,8), suggesting that mobility may be much lower in some soils(SRC). The pKa of quinoline is 4.90(5), indicating that this compound will partially exist in the protonated form in the environment and cations generally adsorb to organic carbon and clay more strongly than their neutral counterparts(6); therefore, adsorption increases with increasing soil acidity(11). Sorption onto airborne particulates has been observed(9). A Kd value of 0.83 was measured using a Danish sandy soil from Lundgaard, Jutland, characterized by 2.47% organic carbon content, 80.2% sand, 13.2% silt, 4.8% clay, and a pH of 5.8(10).
Literature: (1) Borisover MD, Graber ER; Chemosphere 34: 1761-76 (1997) (2) Reinhold KA et al; Adsorption of energy-related organic pollutants: A literature review USEPA-600/3-79-086 (1979) (3) Swann RL et al; Res Rev 85: 17-28 (1983) (4) Fowler MG et al; Org Geochem 22: 641-9 (1994) (5) Weast TC et al; CRC Handbook of Chemistry and Physics. 66th ed. Boca Raton, FL: CRC Press (1985) (6) Doucette WJ; pp. 141-188 in Handbook of Property Estimation Methods for Chemicals; Boethling RS, Mackay D, eds, Baca Raton, FL: Lewis Publ (2000) (7) Bollag JM et al; J Agric Food Chem 26: 1302-6 (1978) (8) Adrian P et al; Chemosphere 18: 1599-1609 (1989) (9) Dong MW et al; Environ Sci Technol 11: 612-8 (1977) (10) Thomsen AB et al; Environ Sci Technol 33: 2891-8 (1999) (11) Zachara JM et al; Environ Sci Technol 20: 620-7 (1986)