Applications of Environmental Chemistry: A Practical Guide by Eugene R. Weiner

By Eugene R. Weiner

Up till the Nineteen Fifties, waste disposal intended discharging it to the closest river, burning it up or transport it out to sea. Now we're paying the associated fee. present disposal and cleanup rules have a special concentration: correcting the issues attributable to previous erroneous attitudes and preserving a non-degrading setting. kingdom and Federal fresh air and water acts have created the necessity to determine and degree chemical parts that impact the standard of floor and flooring waters and the soils in which they flow.The easy-to-use constitution of this booklet makes it a convenient source. the writer summarizes the chemistry themes most vital in environmental purposes. He contains usually used information similar to: water solubilities, partition coefficients, common abundance of hint metals in soil, and federal ingesting water criteria. Lists containing "rules of thumb" offer equipment for making speedy estimations.Applications of Environmental Chemistry offers the elemental equations, theories, and ideas you want to comprehend - at a realistic point - usually encountered issues in environmental chemistry. It doesn't crush you with extra details yet solutions your most commonly asked questions truly and succinctly.

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Consider the halogen gases fluorine (F2, MW = 38), chlorine (Cl2, MW = 71), bromine (Br2, MW = 160), and iodine (I2, MW = 254). All are nonpolar, with progressively greater molecular weights and correspondingly stronger attractive dispersion forces as you go from F2 to I2. Accordingly, their boiling and melting points increase with their molecular weights. 8°C), and I2 is a solid (mp = 184°C). 2 Some Properties of the First Twelve Straight-Chain Alkanes Alkane Formula Molecular Weight Melting Pointa °C Boiling Point °C methane ethane propane n-butane n-pentane n-hexane n-heptane n-octane n-nonane n-decane n-dodecane CH4 C2H6 C3H8 C4H10 C5H12 C6H14 C7H16 C8H18 C9H20 C10H22 C12H26 16 30 44 58 72 86 100 114 128 142 170 –183 –172 –188 –138 –130 –95 –91 –57 –51 –29 –10 –162 –89 –42 0 36 69 98 126 151 174 216 a Deviations from the general trend in melting points occur because melting points for the smallest alkanes are more strongly influenced by differences in crystal structure and lattice energy of the solid.

7, respectively. Copyright © 2000 CRC Press, LLC L1354/ch03/Frame Page 40 Tuesday, April 18, 2000 1:47 AM either phenolphthalein or methyl orange alkalinity. Whether it is present or not, CaCO3 is used as a proxy for all the base species that are actually present in the water. The alkalinity value is equivalent to the mg/L of CaCO3 that would neutralize the same amount of acid as does the actual water sample. IMPORTANCE OF ALKALINITY Alkalinity is important to fish and other aquatic life because it buffers both natural and humaninduced pH changes.

Small polar molecules are dominated by dipole-dipole forces since the contribution to attractions from dispersion forces is small. However, dispersion forces may dominate in very large polar molecules. Rules of Thumb 1. The higher the atomic or molecular weights of nonpolar molecules, the stronger are the attractive dispersion forces between them. 2. For different nonpolar molecules with the same molecular weight, molecules with a linear shape have stronger attractive dispersion forces than do branched, more compact molecules.

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