Postprint.
|
|
- Victoria Gilmore
- 5 years ago
- Views:
Transcription
1 Postprint This is the accepted version of a paper published in Applied Geochemistry. This paper has been peerreviewed but does not include the final publisher proof-corrections or journal pagination. Citation for the original published paper (version of record): Gustafsson, J., Lumsdon, D. (2014) Comment on "Citrate adsorption can decrease soluble phosphate concentration in soils: Results of theoretical modelling'' by Marek Duputel, Nicolas Devau, Michel Brossard, Benoit Jaillard, Davey L. Jones, Philippe Hinsinger and Frederic Gerard (2013). Applied Geochemistry, 46: Access to the published version may require subscription. N.B. When citing this work, cite the original published paper. NOTICE: this is the author s version of a work that was accepted for publication in Applied Geochemistry. Changes resulting from the publishing process, such as peer review, editing, corrections, structural formatting, and other quality control mechanisms may not be reflected in this document. Changes may have been made to this work since it was submitted for publication. A definitive version was subsequently published in Applied Geochemistry, [VOL 46, (25 February 2014)] DOI / j.apgeochem Permanent link to this version:
2 1 2 3 NOTICE: this is the author s version of a work that was accepted for publication in Applied Geochemistry. A definitive version was subsequently published in Applied Geochemistry 46, 85-89, Comment on Citrate adsorption can decrease soluble phosphate concentration in soils: Results of theoretical modeling by Marek Duputel, Nicolas Devau, Michel Brossard, Benoît Jaillard, Davey L. Jones, Philippe Hinsinger and Frédéric Gérard (2013) 9 10 Jon Petter Gustafsson a,b,* and David G. Lumsdon c a Swedish University of Agricultural Sciences, Department of Soil and Environment, Box 7014, Uppsala, Sweden b KTH Royal Institute of Technology, Division of Land and Water Resources Engineering, Teknikringen 76, Stockholm, Sweden c The James Hutton Institute, Environmental & Biogeochemical Science Group, Craigiebuckler, Aberdeen, Scotland AB15 8QH, UK *Corresponding author at: Swedish University of Agricultural Sciences, Department of Soil and Environment, Box 7014, Uppsala, Sweden. Tel. +46 (0) address: jon-petter.gustafsson@slu.se (J P Gustafsson). 1. Introduction In their recent paper Duputel et al. (2013) predict using a multi-site surface complexation model that citrate can decrease inorganic phosphorus (P) solubility in the presence of common soil minerals. Duputel et al. (2013) even suggest, that special attention should be given to microbiologically-mediated citrate degradation in order to avoid the risk of obtaining an adverse effect of citrate adsorption on available P. To the present date the general scientific consensus is that citrate enhances soluble P in soil solution. Previous work 1
3 shows that citrate and some other carboxylic acids decrease P sorption (e.g. Geelhoed et al. 1998) and therefore increase solubility. In early work on soil P, citric acid was used as an extractant (Dyer, 1894). The authors suggest that their modelled citrate effect only occurs on soils where adsorption is influenced by phyllosilicate clays. In this comment we report that this conclusion is the result of a series of unfortunate data and modelling errors, which mean that the modelling exercise of Duputel et al. (2013) is completely wrong. The work of Duputel et al. (2013) builds on the modelling approach of Devau et al. (2014). Together these two papers provide the details necessary for us to reproduce their modelling approach and explain the associated errors. To model ion adsorption on mineral surfaces (goethite, kaolinite, illite and montmorillonite) they used the CD-MUSIC (Charge Distribution MUlti SIte Complexation) model (Hiemstra and van Riemsdijk, 1996). For their soil model they used the soil content of these four mineral surfaces as a model input to simulate adsorption by the whole soil. In our comment we intend to explain why these errors are the result of miscomprehended modelling approach rather than merely simple typographical errors. It is important that the propagation of these mistakes in the scientific literature is arrested because: 1. Plant breeding programs of research are being conducted that are based on the hypothesis that root exudation of citrate will enable enhanced recovery of soil P reserves. 2. It is misleading for other modellers working on issues related to soils and water quality. 3. Understanding P solubility in soils is of global significance to food production. We have found that the model calculations and parameters of Duputel et al. (2013) and those of Devau et al. (2014) contain three fundamental errors that make their model calculations invalid. In addition the paper of Duputel et al. (2013) also contains some typographical mistakes concerning the citation of data sources and errors in the tables containing the modeling parameters, the most important of which will be listed. The three fundamental errors are: 1. The data used to derive model parameters for P adsorption on kaolinite were incorrectly digitized from the cited source reference. 2
4 Calculation errors concerning the magnitude of the reported intrinsic surface complexation constants for the formation of bidentate P complexes on kaolinite, illite and montmorillonite. 3. Errors resulting from an incorrect use of conditional equilibrium constants concerning the formation of bidentate P complexes and the binding of electrolyte ions in the compact part of the double layer. Below we will first describe the three fundamental errors in some detail, and then secondly we will show with illustrated model calculations that by implementing these errors we can reproduce the model output of Duputel et al. (2013) for P adsorption on kaolinite, illite and montmorillonite Errors associated with the optimization of PO 4 adsorption to clay minerals 2.1. Data for P adsorption on kaolinite To derive the model parameters for P adsorption by kaolinite, Duputel et al. (2013) report using the P adsorption data published by Ioannou and Dimirkou (1997). However when we were checking our calculations we digitized the adsorption data from both Duputel et al. (2013) and the original source data of Ioannou and Dimirkou (1997) and found a major divergence. We show the data from the two sources in Fig. 1. A similar error also appears in the data shown in Fig. 3 of Devau et al. (2014). This error means that the model parameters derived from fitting the data points shown in Duputel et al. (2013) would make P sorption by kaolinite stronger than it actually is (assuming that all other the parts of model calculation were all performed correctly, which we will show they were not). Furthermore because kaolinite is one of the four mineral surfaces used in their soil model, this error will alter the calculated distribution of adsorbed P on the other mineral surfaces. It would also impact the modelled competitive adsorption between phosphate and citrate on the kaolinite mineral Errors resulting from incorrect intrinsic equilibrium constants Duputel et al. (2013) claim that they need to convert intrinsic equilibrium constants to conditional equilibrium constants for the bidentate P complexes prior to calculations. The first thing we note is that they have made a mistake in this conversion, which will mislead others who try to use their published intrinsic equilibrium constants for modeling P 3
5 adsorption. They use an equation given by Hiemstra and van Riemsdijk (1996), in which the relationship between the conditional equilibrium constant and an intrinsic constant for a bidentate complex is given by: log K P-2, cond = log K P-2, int log(ρan s ) (1) where log K P-2, cond is the conditional equilibrium constant for a bidentate complex involving phosphate, log K P-2, int is the corresponding intrinsic constant, ρ is the suspension density in kg L -1, A is the specific surface area in m 2 kg -1, and N s is the adsorption site density in mol m -2. Under these conditions, equation (2) can be simplified to log K P-2, cond = log K P-2, int - log [ SOH] (2) where [ SOH] is the concentration of surface adsorption sites (in mol L -1 ). This is the equation normally coded in chemical equilibrium software (Wang and Giammar, 2013). The authors used equation (1) to calculate the conversion factor between intrinsic and conditional equilibrium constants (see our Table 1). However, when applying equation (1) they have used incorrect units (i.e. for N s they used sites nm -2 instead of mol m -2 ). As a result, the conditional equilibrium constants (as shown in Table 1) are actually between five and six orders of magnitude lower than the real ones if one assumes the intrinsic equilibrium constants as shown in Table 1 are correct (which they are not). This numerical error can be easily verified by examination of the conditional equilibrium constants given in Fig. A.1, Supplementary Information, and those for the intrinsic equilibrium constants given in Table A.1, Supplementary Information. For example, consider kaolinite, the log K (conditional) values for the two bidendate surface complexes are given as 26.5 and If one calculates the factor log(ρan s ) from equation (1), using the incorrect units for N s (i.e. 2.0 sites nm -2 ) a value of is obtained. It can be verified that the value of was used in equation (1) to calculate the intrinsic equilibrium constants given in Table A.1 (Supplementary Information). The true value of the factor for kaolinite should have been (i.e. log( /N A )), where N A is Avogadro s number. The same error has also been repeated for illite and montmorillonite. This error means that the reported intrinsic constants are too large and all wrong. For surface complexation modelling, the intrinsic 4
6 constants are regarded as the gold standard thermodynamic equilibrium constant and are used by other modellers for model input, therefore if others were to use these values it would be impossible to model the original data from which they were derived. Furthermore the authors in their approach will compound this error further because they use the derived intrinsic constants to model their soil data. However, the mineral suspension density(ρ) in the modeled soils is different to that used for the modelling of P sorption on the pure mineral phases. Therefore, the authors require a new conversion (log(ρan s )) factor to change the miscalculated intrinsic log K values back into conditional values. This obviously introduces another layer of error Errors resulting from an incorrect use of conditional equilibrium constants In their modelling, Duputel et al. (2013) maintain that conditional equilibrium constants must be used for certain surface reactions when using the CD-MUSIC model. In particular they used conditional constants for: i) the formation of bidentate P surface complexes, and ii) the binding of electrolyte ions such as K + and Cl - (e.g. see foot notes in Table A.1 and A.3 in the Supplementary Information section of Duputel et al., 2013). First, Duputel et al. (2013) claim (p. 122) that conditional values should be used for some equilibrium constants according to the CD-MUSIC model (see Table A, p. 506 in Hiemstra and van Riemsdijk, 1996). In this case, the authors failed to recognize that the conversion to conditional equilibrium constants takes place inside modern geochemical software codes such as Visual MINTEQ, ORCHESTRA and PHREEQC, which is why, intrinsic equilibrium constants should always be used in the input. The important thing to note is that Duputel and colleagues, because of this error, carried out the conversion to conditional equilibrium constants twice (i.e. first outside and then inside the software), which lead to errors which become serious especially when there are large differences in [ SOH] between the calibration data set and the data set subject to model predictions. In part, the senior author feels that he may have some responsibility for the latter mistake, since it has not been clear in the Visual MINTEQ documentation that the conversion to conditional equilibrium constants for bidentate complexes takes place inside the software. However, again it would have been easy for the authors to test their model on another published data set, and again they would have discovered their mistake. 5
7 Second, in the paper of Duputel et al. (2013), the authors state on page 122 that: Conditional log K values were used for the formation of monovalent ions such as Cl - as outersphere surface complexes onto variable-charged surface sites of minerals In support of their argument, the authors cite Hiemstra and van Riemsdijk (1996), who used conditional equilibrium constants to account for the reactions of a NaNO 3 electrolyte. In the case of NO - 3 adsorption to goethite the conditional equilibrium constant can be defined as: log K NO3 = log K NO3,int + log [NO 3 - ] (4) where log K NO3 is the conditional equilibrium constant for NO - 3 adsorption to goethite, whereas log K NO3,int is the intrinsic equilibrium constant for NO - 3 adsorption to goethite. The reason why Hiemstra and van Riemsdijk (1996) used a version of equation (4) in their modeling was that they did not use Na + - or NO 3 as chemical components in the electrolyte ion-binding reactions shown in their table of chemical reactions (this can be seen in their table on p. 506). Therefore only when Na + and NO - 3 are not defined as chemical components, should the equilibrium constants be rewritten as conditional equilibrium constants. However, in almost all later applications of the CD-MUSIC model, e.g. Weng et al. (2012), the electrolyte ions have been included as chemical components in the set of reactions, and in such cases the intrinsic equilibrium constants should be used. From the text of Duputel et al. (2013), it seems clear that the authors did not understand the reason why Hiemstra and van Riemsdijk (1996) used conditional equilibrium constants for electrolyte ion binding. As a consequence they were misled to believe that conditional equilibrium constants (according to equation 1) should always be used, also when the electrolyte ions are included as chemical components. This error is further supported by our model simulations shown in Fig. 2 as explained below. It would have been easy for the authors to test their model on, for example, published acid-base titration data for goethite. They would then quickly find out that they had entered the wrong path. In fact, this error will strongly affect the simulation of phosphate binding to (hydr)oxide surfaces and is therefore a very serious one. This is because the binding electrolyte ions will strongly affect the potential gradient near the surface
8 Modeling of phosphate and citrate adsorption to clay minerals. In this section we investigate whether we can replicate the model fits of Duputel et al. (2013) when accounting for the aforementioned errors. For the purpose of this comparison we will accept all the parameters and constants used by the authors. Two model fits are produced by use of Visual MINTEQ ver. 3.0 (Gustafsson, 2012); one normal fit using intrinsic constants as reported by the authors, and the other one using the conditional equilibrium constants as used by Duputel et al. (2013) and which include the errors described. Table 1 shows the constants and model parameters considered. To double-check the accuracy of our model simulations we also used ORCHESTRA (Meeussen, 2003), with identical results. The reader is referred to either Lumsdon (2012) or Devau et al. (2014) for definition of the constants used. For all clay minerals our model calculation using the reported intrinsic equilibrium constants (Table A.1, Supplementary Information) from Duputel et al. (2013) grossly overestimated PO 4 adsorption (Fig. 2) whereas when we used the incorrect conditional equilibrium constants as given by Duputel et al. (2013) we correctly replicated (Fig. 3) the model lines given by Duputel et al. (2013, Fig. A.1, Supplementary Information). This in turn lends support to our conclusion that Duputel and coworkers made the series of mistakes as described earlier. Obviously the large errors in the phosphate parameters will modify the competitive adsorption of citrate and other components. We also made efforts to replicate the model fits for citrate as reported by the authors. However, in this case we were not successful. For this reason we can only state that the given surface complexation parameters simply do not result in the citrate model fits shown in the paper. We tried several different ways to interpret the author s model parameters, but in no case did the model result in decreased P solubility as a result of increased citrate concentrations. Therefore we question the authors claim that the CD-MUSIC model shows that citrate can decrease P availability in certain soils Other miscellaneous errors and related typos In Table A.1 (Supplementary Information) the values for the Boltzmann factors for Cl - are wrong. They are given as (1, 0, 1), but they should be (1, 0, -1). 7
9 The Boltzmann factors for the K + complex are given as (-1, 1, 0). In recent papers in which the CD-MUSIC model has been used (e.g. Weng et al. 2012), the Boltzmann factors for the interaction of a monovalent cation and a surface site is given as (0, 1, 0). Also in Table A.3 (Supplementary Information) the reaction information for the formation of the potassium outer sphere complex is incorrect, because there is a proton missing in the reaction product. For Fig. 2 in the Duputel et al. (2013) paper, the reference cited as the source of the data for citrate adsorption on kaolinite and illite does not contain these data. The correct reference is probably to a different paper by Lackovic et al. (i.e. Lackovic et al., 2003). Table A.1 (Supplementary Information) shows that a bidentate and a monodentate citrate complex are used to model citrate adsorption on kaolinite, but in Table A.3 (Supplementary Information) two bidentate complexes (with the same log K values as those in Table A.1, Supplementary Information) are given as the reactions needed to model citrate adsorption by kaolinite. In both Table A.1 and Table A.3 the log K value for the ( SOH 2 ) 2 CitH - complex, claimed to be important for illite, is suspiciously low (10, implicating that the complex is unimportant at all conditions). Moreover the Boltzmann factors (3, -2, -1) are not reasonable as there are only two surface groups that can protonate. In Table A.1 (Supplementary Information) there are several errors in the stated surface reactions for the interaction of Ca 2+ with goethite; to be specific the protons in the reaction products do not balance the number of protons in the reactants. The proton stoichiometry for the Ca 2+ complexes on illite and kaolinite is not balanced Implications for modeling PO 4 adsorption to whole soils. Further problems of the model approach of Duputel et al. (2013) will become apparent when applying it to soils. We have not attempted a detailed analysis of the errors that would result. However, one fundamental point of concern is that the intrinsic constants for PO 4 adsorption to clay minerals were too high since they were incorrectly back-calculated from the conditional equilibrium constants. On the other hand, the intrinsic constants for 8
10 goethite, as reported by the authors were genuine intrinsic constants obtained from the literature e.g. Weng et al. (2008). As a result PO 4 will be disproportionately more strongly adsorbed to clay minerals than to iron (hydr)oxides. This is probably the reason why Devau et al. (2009, 2011) predicted illite to be the most important sorbent for P in their model for a clay soil, despite the fact that < 30 % of any added P is adsorbed to illite in laboratory systems (Manning and Goldberg, 1996) Conclusions. The issues identified here show that the modelling approach of Duputel et al. (2013) and Devau et al. (2014) leads to meaningless model parameters, because the model parameters in some cases were fitted to incorrect data, and in other cases the model parameters were derived by applying a series of incorrect modelling procedures. Based on our findings we believe that the modelling methodology, equilibrium constants and conclusions of Duputel, Devau and their co-authors in the paper of Duputel et al. (2013) and in a series of previous papers (Devau et al. 2009, 2010a, 2010b, 2011 and 2014) require major reevaluation Acknowledgements The work was funded by the Swedish Research Council Formas, contract no (JPG) and by the Scottish Government Rural and Environmental Science and Analytical Services (RESAS) Division (DL) References Devau N., Le Cadre E., Hinsinger P., Jaillard B., Gérard F., Soil ph controls the environmental availability of phosphorus: Experimental and mechanistic modelling approaches. Appl. Geochem. 24, Devau N., Le Cadre E., Hinsinger P., Jaillard B., Gérard F., 2010a. Erratum to Soil ph controls the environmental availability of phosphorus: Experimental and mechanistic modelling approaches [Appl. Geochem. 24 (11), ]. Appl. Geochem. 25, Devau N., Le Cadre E., Hinsinger P., Gérard F., 2010b. A mechanistic model for understanding root-induced chemical changes controlling phosphorus availability. Ann. Bot. 105, Devau, N., Hinsinger, P., Le Cadre, E., Colomb, E., Gérard, F., Fertilization and ph effects on processes and mechanisms controlling dissolved inorganic phosphorus in soils. Geochim. Cosmochim. Acta 75,
11 Devau, N., Hinsinger, P., Le Cadre, E., Colomb, E., Gérard, F., Reply to the comment by D.G. Lumsdon on Fertilization and ph effects on processes and mechanisms controlling dissolved inorganic phosphorus in soils by N. Devau, P. Hinsinger, E. Le Cadre, E. Colomb and F. Gérard. Geochim. Cosmochim. Acta 124, Duputel, M., Devau, N., Brossard, M., Jaillard, B., Jones, D.L., Hinsinger, P., Gérard, F., Citrate adsorption can decrease soluble phosphate concentrations in soils: results of theoretical modeling. Appl. Geochem. 35, Dyer, B., On the analytical determination of probably available mineral plant food in soils. J. Chem. Soc. 65, Geelhoed, J.S., Hiemstra, T., van Riemdijk, W.H., Competitive interaction between phosphate and citrate on goethite. Environ. Sci. Technol. 32, Gustafsson, J.P., Visual MINTEQ. Available from: www2.lwr.kth.se/english/oursoftware/vminteq/index.html. Hiemstra, T., van Riemsdijk, W.H., A surface structural approach to ion adsorption: the charge distribution (CD) model. J. Colloid Interface Sci. 179, Iannou, A., Dimirkou, A., Phosphate adsorption on hematite, kaolinite and kaolinite-hematite (k-h) systems as described by a constant capacitance model. J. Colloid Interface Sci. 192, Lackovic, K., Johnson, B. B., Angove, M. J., Wells, J. D., Modeling the adsorption of citric acid onto Muloorina illite and related clay minerals. J. Colloid Interface Sci. 267, Lumsdon, D.G., Comment on Fertilization and ph effects on processes and mechanisms controlling dissolved inorganic phosphorus in soils by Nicolas Devau et al. (2011). Geochim. Cosmochim. Acta 92, Manning, B.A., Goldberg, S., Modeling arsenate competitive adsorption on kaolinite, montmorillonite and illite. Clays Clay Miner. 44, Meeussen J. C. L., ORCHESTRA: An object-oriented framework for implementing chemical equilibrium models. Environ. Sci. Technol. 37, Wang, Z., Giammar, D.E., Mass action expressions for bidentate adsorption in surface complexation modeling: theory and practice. Environ. Sci. Technol. 47, Weng, L. P., van Riemsdijk, W. H., Hiemstra, T., Humic Nano-Particles at the Oxide-Water Interface: Interactions with Phosphate Ion Adsorption. Environ. Sci. Technol. 42, Weng, L. P., van Riemsdijk, W. H,, Hiemstra, T., Factors controlling phosphate interaction with iron oxides. J. Environ. Qual. 41,
12 Table 1 CD-MUSIC constants and model parameters according to Duputel et al. (2013). Kaolinite Illite Montmorillonite Data source Iannou and Manning and Manning and Dimirkou (1997) Goldberg Goldberg (1996) (1996) log K H log K P log K P a / b a / b a / b log K P a / 32.0 b a / b a / b log K Na a / -2.6 b - log K K -1.6 a / -2.6 b - - log K Cl 7.50 a / 6.50 b 7.50 a / 6.50 b 7.50 a / 6.50 b mineral concentration ( g l -1 ) Specific surface area (m 2 g -1 ) Site density (sites nm -2 ) log(ρan s ) c (incorrect) log(ρan s ) (true value) C 1 (F m -2 ) C 2 (F m -2 ) a Intrinsic log K values according to Duputel et al. (2013) b Conditional log K values according to Duputel et al. (2013) and assumed to be valid for the specified data sources only. c The use of incorrect and true values of log(ρan s ) is explained in the main text. 11
13 Fig. 1. Phosphate adsorption by kaolinite (1.0 g dm -3 ), for total P concentrations of 40.3 µm (circles) and 81 µm (triangles). Original data (open symbols) were digitized from the source reference (Iannou and Dimirkou, 1997). The closed symbols were digitized from Duputel et al. (2013)
14 Fig. 2. Phosphate adsorption onto illite, montmorillonite and kaolinite. Observations are shown as points; these data were digitized from the source references (Iannou and Dimirkou, 1997; Manning and Goldberg, 1996). Solid lines are model fits when the intrinsic equilibrium constants, as reported by Duputel et al. (2013) are used. The model parameters required to produce the model fits are given in Table
15 Fig. 3. Phosphate adsorption onto illite, montmorillonite and kaolinite. Data points digitized from Duputel et al. (2013) are shown with open symbols. Data shown as filled circles were digitized from the source references (Iannou and Dimirkou, 1997; Manning and Goldberg, 1996). Solid lines are model fits when the conditional equilibrium constants as reported by Duputel et al. (2013) are used. 14
Multicomponent Transport of Sulfate in a Goethite-Silica Sand System at Variable ph and Ionic Strength
Environ. Sci. Technol. 1999, 33, 3443-3450 Multicomponent Transport of Sulfate in a Goethite-Silica Sand System at Variable ph and Ionic Strength JOHANNES C. L. MEEUSSEN,*, JUTTA KLEIKEMPER, ANDREÄ M.
Adsorption of ions Ion exchange CEC& AEC Factors influencing ion
Adsorption of ions Ion exchange CEC& AEC Factors influencing ion exchange- Significance. Adsorption of ions Ion adsorption and subsequent exchange are important processes that take place between soil colloidal
Adsorption Isotherm of Phosphate Ions onto lica and Amino-modified lica from Lapindo Mud Jaslin Ikhsan 1,2, ti Sulastri 1, Erfan Priyambodo 1 1 Department of Chemistry Education, Faculty of Mathematics
Energy and Resources Recovery from Reverse Osmosis Desalination Concentrate
Energy and Resources Recovery from Reverse Osmosis Desalination Concentrate Tushar Jain; PhD advisor: Haizhou Liu Department of Chemical and Environmental Engineering, University of California, Riverside,
Electronic Supplementary Information Reactivity Ferrihydrite versus Ferritin
Electronic Supplementary Material (ESI) for Environmental Science: Nano. This journal is The Royal Society of Chemistry 16 1 Electronic Supplementary Information for Reactivity of Ferrihydrite and Ferritin
Chapter 7: Anion and molecular retention
I. Anions and molecules of importance in soils Anions of major importance to agricultural soils and soil chemistry are: H 2 PO - 4, HPO 2-4, SO 2-4, HCO - 3, NO - 3, Cl -, F - and OH -. Also, micronutrients
SOIL COLLOIDS PROPERTIES AND ION RINDING. CRC Press. University of Bueno Aires Buenos Aires, Argentina. Taylor & Francis Croup
SOIL COLLOIDS PROPERTIES AND ION RINDING Fernando V. Molina University of Bueno Aires Buenos Aires, Argentina CRC Press Taylor & Francis Croup Boca Raton London New York CRC Press is an imprint of the
Surface Complexation.
Surface Complexation. Jean-François Gaillard, Notes for CE-367 OBJECTIVES To show how the presence of particles in natural and engineered systems controls the fate of many trace elements. The concepts
EXTRAPOLATION STUDIES ON ADSORPTION OF THORIUM AND URANIUM AT DIFFERENT SOLUTION COMPOSITIONS ON SOIL SEDIMENTS Syed Hakimi Sakuma
EXTRAPOLATION STUDIES ON ADSORPTION OF THORIUM AND URANIUM AT DIFFERENT SOLUTION COMPOSITIONS ON SOIL SEDIMENTS Syed Hakimi Sakuma Malaysian Institute for Nuclear Technology Research (MINT), Bangi, 43000
Zinc isotope fractionation during sorption onto
Zinc isotope fractionation during sorption onto kaolinite Damien Guinoiseau, Alexandre Gélabert, Julien Moureau, Pascale Louvat and Marc F. Benedetti * Supplementary information Number of pages: 19 Number
Chemical Sciences Division, Oak Ridge National Laboratory, Oak Ridge, Tennessee
Supplementary Information Ion Exchange Thermodynamics at The Rutile-Water Interface: Flow Microcalorimetric Measurements and Surface Complexation Modeling of Na- K-Rb-Cl-NO3 Adsorption Tyler Hawkins 1,
Effect of Humic Acid on the Selenite Adsorption onto Hematite
Effect of Humic Acid on the Selenite Adsorption onto Hematite MYOUNG-JIN KIM, MIJEONG JANG, and SE YOUNG PAK Department of Environmental Engineering Korea Maritime University 1, Dongsam-dong, Yeongdo-gu,
Effects of phthalic and salicylic acids on Cu(II) adsorption by variable charge soils
iol Fertil Soils (26) 42: 443 449 DOI.7/s374-6-89-2 ORIGINL PPER Renkou Xu. Shuangcheng Xiao. Dan Xie. Guoliang Ji Effects of phthalic and salicylic acids on Cu(II) adsorption by variable charge soils
Isotherm equation of sorption of electrolyte solutions on solids: how to do heterogeneous surface from homogeneous one?
Ŕ periodica polytechnica Chemical Engineering 53/ (009) 55 60 doi: 0.33/pp.ch.009-.04 web: http:// www.pp.bme.hu/ ch c Periodica Polytechnica 009 RESEARCH ARTICLE Isotherm equation of sorption of electrolyte
Phosphate release induced by the reaction of synthetic lepidocrocite (γ-feooh) with dissolved sulfide
Phosphate release induced by the reaction of synthetic lepidocrocite (γ-feooh) with dissolved sulfide MSc. thesis - Kevin van Riel (3381269) 22 April 2013 Supervisor: Dr. Thilo Behrends Geochemistry Department
Lecture 14: Cation Exchange and Surface Charging
Lecture 14: Cation Exchange and Surface Charging Cation Exchange Cation Exchange Reactions Swapping of cations between hydrated clay interlayers and the soil solution Also occurs on organic matter functional
STUDIES ON THE SORPTION OF PHOSPHATE ON SOME SOILS OF INDIA SATURATED WITH DIFFERENT CATIONS
I.J.S.N., VOL. 2(2) 211: 327-333 ISSN 2229 6441 STUDIES ON THE SORPTION OF PHOSPHATE ON SOME SOILS OF INDIA SATURATED WITH DIFFERENT CATIONS Bansal, O. P. Chemistry Department, D.S. College, Aligarh-221
Cation Exchange Capacity, CEC
Cation Exchange Capacity, CEC The basic building blocks of clay minerals are: silicon atoms surrounded by four oxygen atoms (tetrahedra), and aluminium atoms surrounded by six hydroxide groups (dioctahedra),
Effect of Ferrihydrite Crystallite Size on Phosphate Adsorption Reactivity. Xionghan Feng *,,, Donald L. Sparks
1 2 Supporting Information Effect of Ferrihydrite Crystallite Size on hosphate Adsorption Reactivity 3 4 5 Xiaoming Wang, Wei Li *,,, Richard Harrington,, Fan Liu, John B. arise,, Xionghan Feng *,,, Donald
Chem 121H Honors General Chemistry Hour Exam #1 NAME ID#
Not all pieces of information on this page are needed to complete this exam correctly Particle Mass/u Proton 1.007276 Neutron 1.008665 Electron 0.00054858 Isotope Mass/u H-1 1.007825 H-2 2.01400 H-3 3.016005
SOIL and WATER CHEMISTRY
SOIL and WATER CHEMISTRY An Integrative Approach MICHAEL E. ESSINGTON CRC PRESS Boca Raton London New York Washington, D.C. Table of Contents Chapter 1 The Soil Chemical Environment: An Overview 1 1.1
Ion adsorption modeling as a tool to characterize metal (hydr)oxide behavior in soil
Ion adsorption modeling as a tool to characterize metal (hydr)oxide behavior in soil Promotor: Prof. dr. W. H. van Riemsdijk Hoogleraar in de Bodemscheikunde en chemische bodemkwaliteit Promotiecommissie
Lecture 15: Adsorption; Soil Acidity
Lecture 15: Adsorption; Soil Acidity Surface Complexation (Your textbook calls this adsorption ) Surface Complexation Both cations and anions can bind to sites on the external surfaces of soil minerals
http://www.diva-portal.org This is the published version of a paper presented at 16th International Conference on Heavy Metals in the Environment (ICHMET), SEP 23-27, 2012, Rome, ITALY. Citation for the
Lab 8 Dynamic Soil Systems I: Soil ph and Liming
Lab 8 Dynamic Soil Systems I: Soil ph and Liming Objectives: To measure soil ph and observe conditions which change ph To distinguish between active acidity (soil solution ph) and exchangeable acidity
CLASS EXERCISE 5.1 List processes occurring in soils that cause changes in the levels of ions.
5 SIL CHEMISTRY 5.1 Introduction A knowledge of the chemical composition of a soil is less useful than a knowledge of its component minerals and organic materials. These dictate the reactions that occur
Groundwater chemistry
Read: Ch. 3, sections 1, 2, 3, 5, 7, 9; Ch. 7, sections 2, 3 PART 14 Groundwater chemistry Introduction Matter present in water can be divided into three categories: (1) Suspended solids (finest among
Surface Complexation of Selenite on Goethite: MO/DFT Geometry and Charge Distribution*
CROATICA CHEMICA ACTA CCACAA 80 (-4) 1 4 (007) ISSN-0011-164 CCA-174 Original Scientific Paper Surface Complexation of Selenite on Goethite: MO/DFT Geometry and Charge Distribution* Tjisse Hiemstra**,
THE BINDING OF ORGANIC CONTAMINANTS TO HUMIN
THE BINDING OF ORGANIC CONTAMINANTS TO HUMIN S. Kohl and J.A. Rice *, Department of Chemistry & Biochemistry, South Dakota State University, Brookings, SD, 57007-0896 ABSTRACT It has been recognized for
A few more details on clays, Soil Colloids and their properties. What expandable clays do to surface area. Smectite. Kaolinite.
A few more details on clays, Soil Colloids and their properties What expandable clays do to surface area Kaolinite Smectite Size 0.5-5 µm External surface 10-30 m 2 /g Internal surface - Size 0.1-1 µm
Colloids and Surfaces B: Biointerfaces
Colloids and Surfaces B: Biointerfaces 116 (2014) 591 596 Contents lists available at ScienceDirect Colloids and Surfaces B: Biointerfaces journal homepage: www.elsevier.com/locate/colsurfb Adsorption
1. Let s quickly review some of the phosphorus fixation reactions in soils. 2. At low ph (acidic conditons below 6.0), phosphorus fixation occurs
1 1. Let s quickly review some of the phosphorus fixation reactions in soils. 2. At low ph (acidic conditons below 6.0), phosphorus fixation occurs between phosphates and iron or aluminum in the soil solution
Treatment of Colloids in the Safety Case
Treatment of Colloids in the Safety Case Clay Colloids in Aqueous Systems 3 4 February 2016, Berlin Dr Amy Shelton, Radioactive Waste Management (RWM) KBS-3 Concept Based on the multi- barrier principles
Adsorption of alkali metal cations and halide anions on metal oxides: prediction of Hofmeister series using 1-pK triple layer
Adsorption (2010) 16: 295 303 DOI 10.1007/s10450-010-9245-y Adsorption of alkali metal cations and halide anions on metal oxides: prediction of Hofmeister series using 1-pK triple layer model Wojciech
GEOCHEMISTRY, GROUNDWATER AND POLLUTION,
GEOCHEMISTRY, GROUNDWATER AND POLLUTION, 2 ND EDITION C.A.J. APPELO Hydrochemical Consultant, Amsterdam, the Netherlands D. POSTMA Environment & Resources DTU, Technical University of Denmark, Kgs. Lyngby,
Mass Action Expressions for Bidentate Adsorption in Surface Complexation Modeling: Theory and Practice
This is an open access article published under an ACS AuthorChoice License, which permits copying and redistribution of the article or any adaptations for non-commercial purposes. pubs.acs.org/est Mass
EFFECT OF SOLID-SOLUTION RATIO ON ANION ADSORPTION HYDROUS METAL OXIDES
EFFECT OF SOLID-SOLUTION RATIO ON ANION ADSORPTION ON HYDROUS METAL OXIDES THET SU HLAING NATIONAL UNIVERSITY OF SINGAPORE 2004 EFFECT OF SOLID-SOLUTION RATIO ON ANION ADSORPTION ON HYDROUS METAL OXIDES
Potential Impacts of Tailings and Tailings Cover. Fertilization on Arsenic Mobility in Surface and. Ground Waters
Potential Impacts of Tailings and Tailings Cover Fertilization on Arsenic Mobility in Surface and Ground Waters Sierra Rayne * and Kaya Forest Water Treatment Technology Program, Thompson Rivers University,
Dissolution of clay sediments in acid-sulfate systems
Dissolution of clay sediments in acid-sulfate systems Irshad Bibi 1, Balwant Singh 1, Ewen Silvester 2 1 Faculty of Agriculture, Food and Natural Resources, The University of Sydney, Sydney, NSW 2006,
Effect of Heat Treatment on Phosphate Sorption by Soils from Different Ecologies
Effect of Heat Treatment on Phosphate Sorption by Soils from Different Ecologies 1* Aghedo, J.E., 2 Ukpebor, E. and 3 Oviasogie, P.O., 4 Omorogbe, S.O. 1Department of Chemistry, College of Education, Ekiadolor,
Name: Final Test. / n 2 Rydberg constant, R H. = n h ν Hydrogen energy, E n
200 points Chemistry 121A Dr. Jay H. Baltisberger December 13, 1999 SHOW ALL CALCULATIONS & USE PROPER SIGNIFICANT FIGURES AND UNITS Avogadro s number, N A = 6.02x10 23 Planck s constant, h = 6.626x10
Particles in aqueous environments
Lecture 11 Particle-Aqueous Solute Interactions Today 1. Particle types and sizes 2. Particle charges 3. Particle-solute Interactions Next time Please continue to read Manahan Chapter 4. 1. Fresh-salt
Adsorption of heavy metal ions on soils and soils constituents
Journal of Colloid and Interface Science 277 (2004) 1 18 Feature article www.elsevier.com/locate/jcis Adsorption of heavy metal ions on soils and soils constituents Heike B. Bradl Department of Environmental
WM 04 Conference, February 29 March 4, 2004, Tucson AZ ESTIMATING SITE CONCENTRATIONS IN SOILS FOR SURFACE COMPLEXATION MODELING OF SORPTION
ESTIMATING SITE CONCENTRATIONS IN SOILS FOR SURFACE COMPLEXATION MODELING OF SORPTION M. Ewanic, M. North-Abbott, D. Reichhardt, M. H. Zaluski MSE Technology Applications, Inc. ABSTRACT MSE Technology
Chemistry for Today General Organic and Biochemistry 9th Edition Seager
Chemistry for Today General Organic and Biochemistry 9th Edition Seager TEST BANK Full download at: https://testbankreal.com/download/chemistry-today-general-organic-biochemistry-9thedition-seager-test-bank/
Atoms, Molecules, and Ions
Chapter 2 Atoms, Molecules, and Ions Concept Check 2.1 Like Dalton, chemists continue to model atoms using spheres. Modern models are usually drawn with a computer and use different colors to represent
Particle Size Controls on Water Adsorption and Condensation Regimes at Mineral Surfaces
SUPPLEMENTARY MATERIAL Particle Size Controls on Water Adsorption and Condensation Regimes at Mineral Surfaces Merve Yeşilbaş, Jean-François Boily* Department of Chemistry, Umeå University, SE-901 87 Umeå,
CS C1 H Calculating masses
Name: CS C1 H Calculating masses Date: Time: 27 minutes Total marks available: 27 Total marks achieved: Questions Q1. (a) Complete the sentence by putting a cross ( ) in the box next to your answer. The
Chapter 4: Stoichiometry of Chemical Reactions. 4.1 Writing and Balancing Chemical Equations
Chapter 4: Stoichiometry of Chemical Reactions 4.1 Writing and Balancing Chemical Equations A chemical equation represents or symbolizes a chemical reaction. o Substances are represents by their chemical
Soil Colloidal Chemistry. Compiled and Edited by Dr. Syed Ismail, Marthwada Agril. University Parbhani,MS, India
Soil Colloidal Chemistry Compiled and Edited by Dr. Syed Ismail, Marthwada Agril. University Parbhani,MS, India 1 The Colloidal Fraction Introduction What is a colloid? Why this is important in understanding
General Chemistry 1 CHM201 Unit 2 Practice Test
General Chemistry 1 CHM201 Unit 2 Practice Test 1. Which statement about the combustion of propane (C 3H 8) is not correct? C 3H 8 5O 2 3CO 2 4H 2O a. For every propane molecule consumed, three molecules
Chem 11 UNIT 3: STOICHIOMETRY Name:
Chem 11 UNIT 3: STOICHIOMETRY Name: Ms. Pirvu Period: Writing & Balancing Equations Chemical reactions can be described by chemical equations. Recall Law of Conservation of Mass mass cannot be nor. This
Commentary on candidate 3 evidence (Batteries)
on candidate 3 evidence (Batteries) The evidence for this candidate has achieved the following s for each section of this course assessment component. 1 Aim An aim that describes clearly the purpose of
Electrical double layer
Electrical double layer Márta Berka és István Bányai, University of Debrecen Dept of Colloid and Environmental Chemistry http://dragon.unideb.hu/~kolloid/ 7. lecture Adsorption of strong electrolytes from
Soil Fertility. Fundamentals of Nutrient Management June 1, Patricia Steinhilber
Soil Fertility Fundamentals of Nutrient Management June 1, 2010 Patricia Steinhilber Ag Nutrient Management Program University of Maryland College Park Main Topics plant nutrition functional soil model
Chemistry FINAL: CONTENT Review Packet
Chemistry FINAL: CONTENT Review Packet Name: Period: Date: Classification of Matter & Chemical/ Physical Changes 1. are substances that are made up of two or more elements which are chemically combined
Electrochemistry Fall 2017 Fitch/Loyola University Chicago TTh 4:15-5:30; FH105 Office hours 3:15-4:15 T/Th; FH 418 (83119;
Electrochemistry Fall 2017 Fitch/Loyola University Chicago TTh 4:15-5:30; FH105 Office hours 3:15-4:15 T/Th; FH 418 (83119; afitch @luc.edu) Content and Material Electrochemistry is a very diverse area.
OHIO ASSESSMENTS FOR EDUCATORS (OAE) FIELD 009: CHEMISTRY
OHIO ASSESSMENTS FOR EDUCATORS (OAE) FIELD 009: CHEMISTRY June 2013 Content Domain Range of Competencies Approximate Percentage of Assessment Score I. Nature of Science 0001 0003 18% II. Matter and Atomic
CHEM 316/318. Molecule(s) of the day
Molecule(s) of the day Creative minds have been known to survive any sort of bad training. - Anna Freud Your theory is crazy, but it's not crazy enough to be true. Niels Bohr Never express yourself more
Chem 110 General Principles of Chemistry
Chem 110 General Principles of Chemistry Chapter 3 (Page 88) Aqueous Reactions and Solution Stoichiometry In this chapter you will study chemical reactions that take place between substances that are dissolved
* Tsado, P. A. 1, A. O. Osunde 1, C. A. Igwe 2, P.C. Eze 1 and E. Daniya 3
INFLUENCE OF ORGANIC ACIDS ON PHOSPHATE SORPTION AND AVAILABILITY IN AN ALFISOL OF NIGERIAN GUINEA SAVANNA * Tsado, P. A. 1, A. O. Osunde 1, C. A. Igwe 2, P.C. Eze 1 and E. Daniya 3 1 Department of Soil
NCFE Released Items. Correct Answer = D Number of protons = atomic number
Correct Answer = D Number of protons = atomic number Pa = 91 protons U = 92 protons Np = 93 protons Pu = 94 protons Info from Unit 3 Correct Answer = B Valence electrons are the electrons in the HOEL.
Solubility of arsenic in Swedish contaminated soils experiments and modelling
Solubility of arsenic in Swedish contaminated soils experiments and modelling Ann-Sophie Heldele Master s Thesis in Environmental Science EnvEuro European Master in Environmental Science Examensarbeten,
GCSE CHEMISTRY REVISION LIST
GCSE CHEMISTRY REVISION LIST OCR Gateway Chemistry (J248) from 2016 Topic C1: Particles C1.1 Describe the main features of the particle model in terms of states of matter and change of state Explain, in
Husein Ajwa, Emeritus Department of Plant Sciences UC Davis
Husein Ajwa, Emeritus Department of Plant Sciences UC Davis HUSEIN AJWA Plant Sciences Department, UC Davis 1636 East Alisal St., Salinas, CA 93905 Office: (831) 755-2823, Fax: (831) 755-2898 email: haajwa@ucdavis.edu
Atom exchange between aqueous Fe(II) and structural Fe in clay minerals
Supporting Information Environmental Science and Technology Atom exchange between aqueous Fe(II) and structural Fe in clay minerals Anke Neumann 1,, Lingling Wu 2, Weiqiang Li 2, Brian L. Beard 2, Clark
Adsorption of Sb(V) on Goethite: Effect of ph, Ionic Strength, and Competition with Phosphate
Adsorption of Sb(V) on Goethite: Effect of ph, Ionic Strength, and Competition with Phosphate Jianhong Xi Supervised by Liping Weng Outline General introduction Material and methods Experimental results
Chapter 4. Types of Chemical Reactions and Solution Stoichiometry
Chapter 4 Types of Chemical Reactions and Solution Stoichiometry Chapter 4 Table of Contents 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition
Soil ph: Review of Concepts
Soils and Water, Spring 008 Soil ph: Review of Concepts Acid: substance that can donate a proton Base: substance that can accept a proton HA H A HA and A - are called conjugate acid-base pairs. The strength
Isolation and purification treatments change the metal-binding properties of humic acids: effect of HF/HCl treatment
Environ. Chem. 2018, 14, 417 424 CSIRO 2017 doi:10.1071/en17129_ac Supplementary material Isolation and purification treatments change the metal-binding properties of humic acids: effect of HF/HCl treatment
Supplemental Materials. Sorption of Tetracycline to Varying-Sized Montmorillonite Fractions
Supplemental Materials Sorption of Tetracycline to Varying-Sized Montmorillonite Fractions 6 7 8 9 10 11 1 Huaizhou Xu, 1, Xiaolei Qu, 1 Hui Li, Cheng Gu 1, and Dongqiang Zhu 1* 1 State Key Laboratory
Modelling lead(ii) sorption to ferrihydrite and soil organic. matter
NOTICE: this is the author s version of a work that was accepted for publication in Environmental Chemistry. A definitive version was subsequently published in Environmental Chemistry, -, 0. http://dx.doi.org/.1/en1
Distribution of radionuclides in soils dependence on soil parameters
Landesmessstelle für Radioaktivität Fachbereich 01 Fachbereich Physik/Elektrotechnik Distribution of radionuclides in soils dependence on soil parameters BIOPROTA-Meeting Nancy 24.05.2012 Contents modelling
Name: Chemistry Unit Review Science 9
Name: Chemistry Unit Review Science 9 Do not forget to study for notes, assignments and quizzes! 1. Classify each of the following as a physical or a chemical change. a) Garbage rotting d) Digesting food
ELECTRONIC SUPPLEMENTARY INFORMATION (ESI)
Electronic Supplementary Material (ESI) for Environmental Science: Nano. This journal is The Royal Society of Chemistry 216 ELECTRNIC SUPPLEMENTARY INFRMATIN (ESI) Spectral Characterization and Surface
From soil clays to erosion processes Jaime Cuevas UAM
From soil clays to erosion processes Jaime Cuevas UAM Clay erosion in safety assessment in Deep Geological Repositories (DGR) Compacted bentonite will produce colloidal particles (Fissures; active fractures)
PHOSPHATE ADSORPTION BY THE MIXED INORGANIC ION EXCHANGER BASED ON FE-MN HYDROUS OXIDES: EQUILIBRIUM AND FTIR STUDIES
Proceedings of the 14 th International Conference on Environmental Science and Technology Rhodes, Greece, 35 September 2015 PHOSPHATE ADSORPTION BY THE MIXED INORGANIC ION EXCHANGER BASED ON FEMN HYDROUS
NMR T 1 relaxation study of 133 Cs and 23 Na adsorbed on illite
American Mineralogist, Volume 83, pages 661 665, 1998 NMR T 1 relaxation study of 133 Cs and 23 Na adsorbed on illite YEONGKYOO KIM* AND R. JAMES KIRKPATRICK Department of Geology, University of Illinois,
Influence of soil type and land use on the nature of mobile colloids: implications for the metal transfer in soils
Symposium no. 01 Paper no. 1289 Presentation: poster Influence of soil type and land use on the nature of mobile colloids: implications for the metal transfer in soils CITEAU Laëtitia, LAMY Isabelle, van
Interaction of copper and fulvic acid at the hematite water interface
Pergamon PII S0016-7037(01)00695-0 Geochimica et Cosmochimica Acta, Vol. 65, No. 20, pp. 3435 3442, 2001 Copyright 2001 Elsevier Science Ltd Printed in the USA. All rights reserved 0016-7037/01 $20.00.00
Weathering and Soils
OCN 401-11 Oct. 13, 2011 KCR Weathering and Soils Biogeochemistry Chapter 4: The Lithosphere Introduction: the context Rock Weathering Soil Chemical Reactions Soil Development (see text) Weathering Rates
SIMPLE METHOD FOR DETERMINATION OF CARBONATE ADSORPTION AT ELEVATED CARBON DIOXIDE CONCENTRATION
Clay Science 12, 97-101 (2003) SIMPLE METHOD FOR DETERMINATION OF CARBONATE ADSORPTION AT ELEVATED CARBON DIOXIDE CONCENTRATION SHIN-ICHIRO WADA* and HIROYUKI ONO** * Faculty of Agriculture, Kyushu University,
Modelling lead(ii) sorption to ferrihydrite and soil organic matter
CSIRO PUBLISHING Environ. Chem. 211, 8, 485 492 Research Paper www.publish.csiro.au/journals/env Modelling lead(ii) sorption to ferrihydrite and soil organic matter Jon Petter Gustafsson, A,D Charlotta
Adsorption and Precipitation of Organic Phosphonates onto the Calcite Stepped Surfaces Wu LEI 1,a, Chun-Yu CHEN 2,b,*, Ni BAI 2,c
International Conference on Material Science and Application (ICMSA 2015) Adsorption and Precipitation of Organic Phosphonates onto the Calcite Stepped Surfaces Wu LEI 1,a, Chun-Yu CHEN 2,b,*, Ni BAI 2,c
Adsorption of perfluorooctanoic acid (PFOA) using graphene-based materials
Adsorption of perfluorooctanoic acid (PFOA) using graphene-based materials Supriya Lath (PhD Student, The University of Adelaide) Prof. Mike McLaughlin Dr. Divina Navarro Prof. Dusan Losic Dr. Anu Kumar
Scientific registration n o : 728 Symposoum n o : 6 Presentation : Poster CHOUDHARY O.P., HUNDAL H.S., KUMAR S.
Scientific registration n o : 728 Symposoum n o : 6 Presentation : Poster Competitive Adsorption of Phosphate, Molybdate, Borate and Silicate in Binary-anion mixture with soils Adsorption compétitive de
IB Chemistry Solutions Gasses and Energy
Solutions A solution is a homogeneous mixture it looks like one substance. An aqueous solution will be a clear mixture with only one visible phase. Be careful with the definitions of clear and colourless.
Pyrite in acid sulfate soils: transformation and inhibition of its oxidation by application of natural materials
Symposium no. 28 Paper no. 97 Presentation: oral Pyrite in acid sulfate soils: transformation and inhibition of its oxidation by application of natural materials SHAMSHUDDIN Jusop and SARWANI Muhrizal
General Chemistry. Contents. Chapter 5: Introduction to Reactions in Aqueous Solutions. Electrolytes. 5.1 The Nature of Aqueous Solutions
General Chemistry Principles and Modern Applications Petrucci Harwood Herring 8 th Edition Chapter 5: Introduction to Reactions in Aqueous Solutions Philip Dutton University of Windsor, Canada N9B 3P4
NOTE. Separation of chlorophenols using columns of hydroxyaluminium interlayered clays
Clay Minerals (1997) 32, 143-147 NOTE Separation of chlorophenols using columns of hydroxyaluminium interlayered clays Clay minerals play an important role in the retention, transport and chemistry of
Temperature and wetting effects on phosphate sorption by soil
Temperature and wetting effects on phosphate sorption by soil G.M. Hijink October 2010 MSc Thesis Soil Quality SOQ-80439 Table of Contents 1. SUMMARY 1 2. INTRODUCTION 3 3. THEORY 5 3.1. BACKGROUND 5
LECTURE 9 - Acids and Bases
LECTURE 9 - Acids and Bases Note: Slide numbers refer to the PowerPoint presentation which accompanies the lecture. Acids & Bases, slide 1 here Acids The classical definition of an acid is a substance
General Chemistry. Chapter 5: Introduction to Reactions in Aqueous Solutions. Principles and Modern Applications Petrucci Harwood Herring 8 th Edition
General Chemistry Principles and Modern Applications Petrucci Harwood Herring 8 th Edition Chapter 5: Introduction to Reactions in Aqueous Solutions Philip Dutton University of Windsor, Canada N9B 3P4
9.1.1 CHEMICAL EQUATIONS AND STOICHIOMETRY
9.1.1 CHEMICAL EQUATIONS AND STOICHIOMETRY Work directly from Zumdahl (Chapter 3). Work through exercises as required, then summarise the essentials of the section when complete. A chemical equation is
Name: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW
Name: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW Unit 1: Nature of Science What rules must be obeyed to safely conduct an experiment? What are the components of a good scientific experiment? What
CHEM 103 Aqueous Solutions
CHEM 103 Aqueous Solut Lecture Notes February 28, 2006 Prof. Sevian 1 Agenda What is a solution made of? Solubility of ionic compounds (salts), acids, and molecular compounds Exchange react that produce
Chapter 12 & 13 Test Review. Bond, Ionic Bond
Chapter 12 & 13 Test Review A solid solute dissolved in a solid solvent is an Alloy What is happening in a solution at equilibrium? The Ionic rate of Bond dissolving is equal to the rate of crystallization.
organisms CaCO 3 + H 2 O + CO 2 shallow water
Weathering and Reverse weathering Step I:Weathering of igneous rocks 1. Igneous rocks are mainly composed of Al, Si and O 2 with minor and varying quantities of Na, K, Ca and Mg composing pheldspar minerals
Chapter 7 An Introduction to Chemical Reactions. An Introduction to Chemistry by Mark Bishop
Chapter 7 An Introduction to Chemical Reactions An Introduction to Chemistry by Mark Bishop Chapter Map Chemical Reaction A chemical change or chemical reaction is a process in which one or more pure substances
During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:
Example 4.1 Stoichiometry During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Suppose that a particular plant consumes 37.8 g of CO 2