By Werner Stumm
"Like the former versions, this considerably revised and up to date 3rd variation has been written to supply readers with an excellent figuring out of the final chemical rules underlying common water chemistry: chemical thermodynamics and kinetics, acids and bases, dissolved carbon dioxide, atmosphere-water interactions, steel ions in aqueous options, precipitation and dissolution, oxidation and reduction, equilibria, and the solid-solution interface." "To support the reader seize the fundamental parts of aquatic chemistry, the authors illustrate key rules with a variety of quantitative examples and an entire variety of problem-solving tools, together with algebraic, graphical, and numerical equipment according to electronic computation." "Designed for either reference in addition to lecture room use, Aquatic Chemistry, during this new version, continues to be the authoritative source at the basics of traditional water chemistry."--Jacket. Read more...
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Additional info for Aquatic chemistry : chemical equilibria and rates in natural waters
Vapor pressure lowering of dilute NaCl solutions obeys Raoult's law for the solvent water—that is, pw = p^xw— and the vapor pressure corresponds to two solute species. The chemical potential of aqueous NaCl must then be the sum of the chemical potentials of the Na+(aq) and Cl(aq) ionic species: ^2 = MNaCl = MNa+ + MCI~ 0) In dilute solution, theoretical expressions for the individual ions are MNa+ = MNa+ + RT lli mNa+ (ii) /*ci = /*ci + RT\n ma- (iii) with MNa+ + MCl- s (iv) MNaClCaq) Therefore the total chemical potential is of the form MNaCl(eq) ~ MNaCl(aq) + RT In tflNa+mc, (v) Adopting the convenient brief notation m+ = mNa+ (vi) m_ = m cl and recognizing that stoichiometry requires ^NaCl = m Na + = m Q\ (vii) the result is MNaCI = MNaCI + RT \l\ W + m _ = MNaci + # 7 In mNaci (viii) For a nonideal electrolyte solution, for example, NaCl, the chemical potential on the molal scale must then be expressed as Mwaci = MNaa + RT In a +a _ (ix) MNaCi = Mwaci + RT In 7 + m + 7_m_ (x) or 40 Chemical Thermodynamics and Kinetics where a± and a_, and 7+ and 7 .
The principles of thermodynamics are based on experience and experiments. , their translational, vibrational, rotational, and electronic energies). ] First Law: Heat and Work As usually presented for equilibrium systems of fixed composition, the first law is dE = dq - dw (11) (heat transfer to the system is considered positive and work done by the system is considered negative) Forms of Work For PVT systems, only "pV" work is considered: dw — —p dV. dE is an exact differential, E being a function of the state of the system only, but dw and dq are both path-dependent quantities; that is, their values depend on whether changes in a system take place under quasistatic (reversible) or under irreversible conditions.
The dielectric constant € is dimensionless. 854 x 10~12 J" 1 C 2 m _ l . 2 J"1 C 2 m~ ! 998 x 10 8 ms- ! S 202 B l Tb Ifly ia HO 1 Er r4 |fXl|4ff'Sd'l? 085 | ^ iH«]2«y t A! 3 9 -VIIIA- Re Os »■» l r Lpt 2 [%i|5fH8d*7? 02J) 9 9 ( a i . 1 INTRODUCTION Natural waters obtain their equilibrium composition through a variety of chemical reactions and physicochemical processes. In this chapter we consider principles and applications of two alternative models for natural water systems: thermodynamic models and kinetic models.