Solubility of ammonia in water at low concentrations

Hales, J.M.; Drewes, D.R.

doi:10.1016/0004-6981(79)90037-4

Cited by 126 publications

(57 citation statements)

References 15 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…The values of ^H reported by Hales and Drewes [6] are clearly higher than those of other investigators, a situation [10] Thermodynamic value calculated 57.64 from Wagman data [11] . B108 (2004) 29-60 31 resulting most likely from poor management of temperature changes and control in the experimental procedures, as discussed by Dasgupta and Dong [8].…”

Section: Solubility In Pure Watermentioning

confidence: 73%

Fate of ammonia in the atmosphere?a review for applicability to hazardous releases

Renard

Calidonna

Henley³

2004

Journal of Hazardous Materials

139

View full text Add to dashboard Cite

Section: Solubility In Pure Watermentioning

confidence: 73%

Fate of ammonia in the atmosphere?a review for applicability to hazardous releases

Renard

Calidonna

Henley³

2004

Journal of Hazardous Materials

139

View full text Add to dashboard Cite

“…The diabatic freezing time is determined by the rate of latent heat removal to the underlying rime substrate Inter-and extrapolated from Brownscombe and Hallett (1967); Macklin andPayne (1967, 1969). 2 Calculated for the corresponding LWCs for 3m s −1 (Macklin and Payne, 1967 Calculated at 0 • C and at the corresponding pH (Warneck and Williams, 2012;Barret et al, 2011;Johnson et al, 1996;Compernolle and Müller, 2014;Marsh and McElroy, 1985;Schwartz and White, 1981;Hales and Drewes, 1979;Maahs, 1982). 5 The mass accommodation coefficients (α at 273K) are taken from a review paper (Davidovits et al, 2006) or estimated as described elsewhere (Ervens et al, 2003).…”

Section: Model Descriptionmentioning

confidence: 99%

Chemistry of riming: the retention of organic and inorganic atmospheric trace constituents

Jost

Szakáll²,

Diehl³

et al. 2017

Atmos. Chem. Phys.

View full text Add to dashboard Cite

Abstract. During free fall in clouds, ice hydrometeors such as snowflakes and ice particles grow effectively by riming, i.e., the accretion of supercooled droplets. Volatile atmospheric trace constituents dissolved in the supercooled droplets may remain in ice during freezing or may be released back to the gas phase. This process is quantified by retention coefficients. Once in the ice phase the trace constituents may be vertically redistributed by scavenging and subsequent precipitation or by evaporation of these ice hydrometeors at high altitudes. Retention coefficients of the most dominant carboxylic acids and aldehydes found in cloud water were investigated in the Mainz vertical wind tunnel under dry-growth (surface temperature less than 0 • C) riming conditions which are typically prevailing in the mixed-phase zone of convective clouds (i.e., temperatures from −16 to −7 • C and a liquid water content (LWC) of 0.9±0.2 g m −3 ). The mean retention coefficients of formic and acetic acids are found to be 0.68 ± 0.09 and 0.63 ± 0.19. Oxalic and malonic acids as well as formaldehyde show mean retention coefficients of 0.97 ± 0.06, 0.98 ± 0.08, and 0.97 ± 0.11, respectively. Application of a semi-empirical model on the present and earlier wind tunnel measurements reveals that retention coefficients can be well interpreted by the effective Henry's law constant accounting for solubility and dissociation. A parameterization for the retention coefficients has been derived for substances whose aqueous-phase kinetics are fast compared to mass transport timescales. For other cases, the semi-empirical model in combination with a kinetic approach is suited to determine the retention coefficients. These may be implemented in high-resolution cloud models.

show abstract

“…[10] However, the expression presented in Eqn 5 fails to reproduce the measurements presented within the paper (see Fig. 1), or equivalent measurements presented elsewhere, [2,7,11] which are in good agreement with the dataset of Khoo et al [1] In fact, Eqn 5 implies that when I f is zero (i.e. pure water) there is no temperature effect on pK a , which from the experimental data [1] is clearly incorrect.…”

mentioning

confidence: 93%

“…Note that Eqn 6 shows relatively close agreement with the Khoo et al [1] measured data, as well as other data. [2,7] [1] formulation for ambient NH 3(aq) concentration over an environmental range of (a) temperatures and (b) salinities. The 100% line represents true ambient NH 3 concentration; >100% is an overestimation of the true value while <100% is an underestimation.…”

mentioning

confidence: 99%

See 1 more Smart Citation

Ammonia/ammonium dissociation coefficient in seawater: A significant numerical correction

et al. 2007

View full text Add to dashboard Cite

Environmental context. Quantifying ammonia concentrations in natural waters is important for our understanding of environmental processes that relate, in particular, to aquaculture toxicity and to the transfer of gaseous ammonia into the atmosphere where it plays a role in new particle formation and climate regulation. The proportion of ammonia present in natural waters is determined in part by variations in temperature and salinity. This work identifies that a previous equation for predicting ammonia concentrations over natural temperature and salinity ranges is incorrect and suggests alternative, more appropriate equations. A more accurate estimation of environmental ammonia concentrations is essential if improved estimates are to be made of the flux of ammonia into the atmosphere and the level of ammonia toxicity within aquacultures. Abstract. The equilibrium between ammonia (NH3) and ammonium (NH4+) in aqueous solution is a function of temperature, pH and the ionic strength of the solution. Here we reveal a 30-year-old error in published work on the thermodynamics of ammonium dissociation in seawater, which has propagated throughout the literature. The work in question[1] [K. H. Khoo, C. H. Culberson, R. G. Bates, J. Solution Chem. 1977, 6, 281] presents an incorrect expression for the variation of the acid dissociation coefficient (Ka) of ammonium with temperature and ionic strength. We detail the error and reveal that it can lead to as much as a 500% overestimation in calculated NH3 concentration under environmental conditions. This finding is highly relevant, particularly for studies of ammonia toxicity and air–sea ammonia exchange. In addition, we recommend two expressions that better reproduce previous experimental work: (i) taken from the work of Johansson and Wedborg,[2] and (ii) our own derivation using the dataset of Khoo et al.[1]

show abstract

Solubility of ammonia in water at low concentrations

Cited by 126 publications

References 15 publications

Fate of ammonia in the atmosphere?a review for applicability to hazardous releases

Fate of ammonia in the atmosphere?a review for applicability to hazardous releases

Chemistry of riming: the retention of organic and inorganic atmospheric trace constituents

Ammonia/ammonium dissociation coefficient in seawater: A significant numerical correction

Contact Info

Product

Resources

About