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Relevant bibliographies by topics / Solution (Chemistry) Dissociation

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Academic literature on the topic 'Solution (Chemistry) Dissociation'

Author: Grafiati

Published: 4 June 2021

Last updated: 7 February 2022

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Journal articles on the topic "Solution (Chemistry) Dissociation"

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Boichenko, Alexander, Vadim Markov, Hoan Kong, Anna Matveeva, and Lidia Loginova. "Re-evaluated data of dissociation constants of alendronic, pamidronic and olpadronic acids." Open Chemistry 7, no. 1 (2009): 8–13. http://dx.doi.org/10.2478/s11532-008-0099-z.

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AbstractThe dissociation constants of (4-amino-1-hydroxybutylidene)bisphosphonic (alendronic) acid, (3-(dimethylamino)-1-hydroxypropylidene)bisphosphonic (olpadronic) acid and (3-amino-1-hydroxypropylidene)bisphosphonic (pamidronic) acid were obtained in aqueous solutions (0.10 M KCl) and micellar solutions of cetylpyridinium chloride (0.10 M CPC) at 25.0°C. With the exception of the third dissociation constant of alendronic acid, the dissociation constants of alendronic, olpadronic and pamidronic acids in aqueous solutions matched literature data. The possibility of sodium alendronate determi

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Kawakami, Kikuji, Yuko Okabe, and Takashi Norisuye. "Dissociation of dimerized xanthan in aqueous solution." Carbohydrate Polymers 14, no. 2 (1990): 189–203. http://dx.doi.org/10.1016/0144-8617(90)90030-v.

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Diemente, Damon. "Demonstration of ionic dissociation in aqueous solution." Journal of Chemical Education 67, no. 11 (1990): 950. http://dx.doi.org/10.1021/ed067p950.

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Macartney, Donal Hugh, and Lauren Jean Warrack. "Ligand substitution reactions of pentacyanoferrate(II) complexes with N-heterocyclic cations in aqueous solution." Canadian Journal of Chemistry 67, no. 11 (1989): 1774–79. http://dx.doi.org/10.1139/v89-274.

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Kinetic and spectroscopic studies have been carried out in aqueous solution on the formation (from Fe(CN)5OH23−) and dissociation of pentacyanoferrate(II) complexes containing 1-(4-pyridyl)pyridinium and the neutral, protonated, and N-methylated forms of 4,4′-bipyridine (BPY), 1,2-bis(4-pyridyl)ethane (BPA), and trans-1,2-bis(4-pyridyl)ethylene (BPE). The pH dependences of the formation kinetics have been analyzed in terms of the specific rate and acid dissociation constants for these ligands. The rate constants (25.0 °C, I = 0.10 M) for the formation of the dinuclear complexes (NC)5FeLFe(CN)5

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Beach, Daniel G., and Wojciech Gabryelski. "Solution to collision induced dissociation mass spectrometry challenge." Analytical and Bioanalytical Chemistry 410, no. 17 (2018): 3927–30. http://dx.doi.org/10.1007/s00216-018-1044-4.

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Böck, Stefan, Heinrich Nöth, and Astrid Wietelmann. "Solutions of Gallium Trichloride in Ethers: A 71Ga NMR Study and the X-Ray Structure of GaCl3 · Monoglyme." Zeitschrift für Naturforschung B 45, no. 7 (1990): 979–84. http://dx.doi.org/10.1515/znb-1990-0711.

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Solutions of GaCl3 in various ethers have been studied by 71Ga NMR spectroscopy. σ71Ga data indicate that the predominant species in diethylether and tetrahydrofuran solutions are GaCl3 · O(C2H5)2 and GaCl3. 2OC4H8, respectively. However, in monoglyme solution dissociation occurs and the product crystallizing from the solution is [cis-GaCl2(monoglyme)2]GaCl4 as demonstrated by an X-ray structure determination of the solvate GaCl3 · monoglyme.

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Kochergina, L. A., V. P. Vasil’ev, D. V. Krutov, and O. N. Krutova. "The dissociation of ethylenedithiodiacetic acid in aqueous solution." Russian Journal of Physical Chemistry A 81, no. 5 (2007): 717–20. http://dx.doi.org/10.1134/s003602440705010x.

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Saleh, Magda S., Kamal A. Idriss, Mohamed S. Abu-Bakr, and Elham Y. Hashem. "Acid dissociation and solution equilibria of some pyridinecarboxylic acids." Analyst 117, no. 6 (1992): 1003. http://dx.doi.org/10.1039/an9921701003.

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Tilset, Mats, and Vernon D. Parker. "Solution homolytic bond dissociation energies of organotransition-metal hydrides." Journal of the American Chemical Society 111, no. 17 (1989): 6711–17. http://dx.doi.org/10.1021/ja00199a034.

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Partanen, Jaakko I., Pekka M. Juusola, Pentti O. Minkkinen, and Virginie Verraes. "Determination of the second stoichiometric dissociation constants of glycine in aqueous sodium or potassium chloride solutions at 298.15 K." Canadian Journal of Chemistry 81, no. 12 (2003): 1462–70. http://dx.doi.org/10.1139/v03-154.

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Equations were determined for the calculation of the second stoichiometric (molality scale) dissociation constant, Km2, of glycine, in aqueous NaCl and KCl solutions at 298.15 K, from the thermodynamic dissociation constant, Ka2, of this acid and the ionic strength, Im, of the solution. The ionic strength of the solutions considered in this study is determined mostly by the salt alone, and the equations for Km2 were based on the single-ion activity coefficient equations of the Hückel type. New data measured by potentiometric titrations in a glass electrode cell were used in the estimation of t

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Dissertations / Theses on the topic "Solution (Chemistry) Dissociation"

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"First principle studies on the solvation and dissociations of formaldehyde and formic acid in gas phase and aqueous phase." 2012. http://library.cuhk.edu.hk/record=b5549485.

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超臨界水中的溶解和化學反應受到一系列因素的影響，如溶解能，熵以及溶液密度等，是決定化學平衡的基本熱力學量，同時這些又受到溫度和壓強的控制。爲了解釋這些因素的影響，有必要把量子化學的靜態優化與分子動力學模擬相結合和比較。通過量子化學可以得到0K下的優化結構，而分子動力學模擬可以提高實際時間的勢能面。本論文的研究，主要圍繞在氣態下甲醛分子HCHO和甲酸分子HCOOH跟不同數目水分子H2O結合的水合簇結構，以及在常溫水溶液和超臨界水溶液中，甲醛HCHO和甲酸HCOOH的溶解結構和溫度所帶來的熱效應，最後研究甲酸HCOOH在水催化下的離解反應機理。<br>使用化學計算軟件Gaussian03和密度泛函理論方法，用6-311++G(d,p)基組來計算和研究氣態下甲醛分子和甲酸分子的水簇合物。通過不同數目的水分子所得到的最穩定簇合物的結構和能量，來研究甲醛分子HCHO，甲酸根離子HCOO⁻以及甲酸分子HCOOH與水分子相互結合時的氫鍵作用力強弱和簇合物的穩定性。同時，也考慮了甲酸酸解后的水簇合物結構，通過與沒有酸解的水簇合物的比較，為進一步瞭解水溶解中甲酸的酸解離情況提供寶貴的信息。<br>使用基於贗勢和平面波基組，以及密度泛函理論的從頭計算分子動力學軟件VASP，來模擬和研究甲醛分子HCHO和甲酸分子在水溶液中的溶解情況。根據對半徑關聯函數PRDF的統計結果，可以觀察出溶質的溶解結構，以及溶

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Tummanapelli, Anil Kumar. "Ab Initio Molecular Dynamics Studies of Bronsted Acid-Base Chemistry in Aqueous Solutions." Thesis, 2015. http://etd.iisc.ernet.in/2005/3943.

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Knowledge of the dissociation constants of the ionizable protons of weak acids in aqueous media is of fundamental importance in many areas of chemistry and biochemistry. The pKa value, or equilibrium dissociation constant, of a molecule determines the relative concentration of its protonated and deprotonated forms at a speciﬁed pH and is therefore an important descriptor of its chemical reactivity. Considerable eﬀorts have been devoted to the determination of pKa values by deferent experimental techniques. Although in most cases the determination of pKa values from experimental is straightforw

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Book chapters on the topic "Solution (Chemistry) Dissociation"

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Lichtin, Norman N. "Ionization and Dissociation Equilibria in Solution in Liquid Sulfur Dioxide." In Progress in Physical Organic Chemistry. John Wiley & Sons, Inc., 2007. http://dx.doi.org/10.1002/9780470171806.ch3.

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Canuto, Sylvio, Kaline Coutinho, and Benedito J. Costa Cabral. "Hydrogen Bonding and the Energetics of Homolytic Dissociation in Solution." In Fundamental World of Quantum Chemistry. Springer Netherlands, 2004. http://dx.doi.org/10.1007/978-94-017-0448-9_25.

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Oriakhi, Christopher O. "Ionic Equilibria and pH." In Chemistry in Quantitative Language. Oxford University Press, 2009. http://dx.doi.org/10.1093/oso/9780195367997.003.0022.

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Water is a weak acid. At 25°C, pure water ionizes to form a hydrogen ion and a hydroxide ion: H2O ⇋ H+ + OH− Hydration of the proton (hydrogen ion) to form hydroxonium ion is ignored here for simplicity. This equilibrium lies mainly to the left; that is, the ionization happens only to a slight extent. We know that 1 L of pure water contains 55.6 mol. Of this, only 10−7 mol actually ionizes into equal amounts of [H+] and [OH−], i.e., [H+] = [OH−] = 10−7M Because these concentrations are equal, pure water is neither acidic nor basic. A solution is acidic if it contains more hydrogen ions than hydroxide ions. Similarly, a solution is basic if it contains more hydroxide ions than hydrogen ions. Acidity is defined as the concentration of hydrated protons (hydrogen ions); basicity is the concentration of hydroxide ions. Pure water ionizes at 25°C to produce 10−7 M of [H+] and 10−7 M of [OH−]. The product Kw = [H+]×[OH−] = 10−7 M×10−7 M= 10−14 M is known as the ionic product of water. Note that this is simply the equilibrium expression for the dissociation of water. This equation holds for any dilute aqueous solution of acid, base, and salt. The pH of a solution is defined as the negative logarithm of the molar concentration of hydrogen ions. The lower the pH, the greater the acidity of the solution. Mathematically: pH=−log10[ H+] or −log10[H3O+] This can also be written as: pH = log10 1/[H+] or log10 1/[H3O+] Taking the antilogarithm of both sides and rearranging gives: [H+] = 10−pH This equation can be used to calculate the hydrogen ion concentration when the pH of the solution is known.

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Zhang, F. S., and T. R. Yu. "Reactions with Hydrogen Ions." In Chemistry of Variable Charge Soils. Oxford University Press, 1997. http://dx.doi.org/10.1093/oso/9780195097450.003.0013.

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Hydrogen ion is one kind of cation which possesses many properties common to all cations. Hydrogen ion also has its own characteristic features which are of particular significance for variable charge soils. The interactions between hydrogen ions and the surface of soil particles is the basic cause of the variability of both positive and negative surface charges of variable charge soils. The quantity of hydrogen ions in soils determines the acidity of the soil while the acidity of variable charge soils is among the strongest in all the soils. This strong acidity of variable charge soils affects many other chemical properties of the soil. In this chapter, the basic properties of hydrogen ions will be briefly discussed. Then, the products and the kinetics of the interaction between hydrogen ions and variable charge soils will be treated. The dissociation of hydrogen ions from the surface of soil particles has already been mentioned in Chapter 2. After the dissociation of an electron, a hydrogen atom becomes a proton (H+ ion). The ionization energy of hydrogen atoms is 1310 kj mol-1, whereas those of alkali metals, Li, Na, K, and Cs, are 519, 494, 419 and 377 kj mol-1, respectively. This difference in the ionization energy between hydrogen and alkali metals indicates that protons have a particularly strong affinity for electrons. Therefore, protons are apt to form a covalent bond with other atoms by sharing a pair of electrons, or to form a hydrogen bond. Because of the absence of an electronic shell, a proton has a diameter of the order of 10-13 cm, while other ions with electronic shells generally have a diameter of the order of 10-8 cm. Because a proton is so small, it is quite accessible to its neighboring ions and molecules. Therefore, there is very little steric hindrance when protons participate in chemical reactions. The above-mentioned features of proton are the basis for its particular properties. Free proton in solution is extremely unstable because it is very active. In an aqueous solution it will react with water molecules to form a hydrated proton, H3O+.

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Ji, G. L., and H. Y. Li. "Electrostatic Adsorption of Cations." In Chemistry of Variable Charge Soils. Oxford University Press, 1997. http://dx.doi.org/10.1093/oso/9780195097450.003.0006.

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Adsorption of ions is a direct consequence of the carrying of surface charge for soils. Owing to the characteristics of variable charge soils in chemical and mineralogical compositions, these soils possess distinct amphoteric properties. Therefore, they can adsorb cations as well as anions. Under field conditions, most of the variable charge soils carry more negative surface charge than positive surface charge, hence they adsorb more cations than anions. Under certain conditions the quantities of adsorbed cations and anions are equal to each other. In this case the soil is said to be at its iso-ionic point. Generally, for most cations commonly found in soils, the interaction force between them and the surface of soil particles during adsorption is electrostatic in nature. However, owing to the characteristics of variable charge soils, a specific force may also be involved in the adsorption of some cations. This latter topic shall be discussed in Chapter 5. In this chapter, only electrostatic adsorption is dealt with. In the present chapter, the mechanism of electrostatic adsorption of cations by variable charge soils and the factors that may affect this type of adsorption are presented first. Then, the dissociation of adsorbed cations is discussed. Finally, the competitive adsorptions of potassium ions with sodium ions and of potassium ions with calcium ions are examined. According to the definition in physical chemistry, the concentration of solute in the surface layer of the solution is different from that in the interior of the bulk solution. If the concentration of solute in the surface layer is higher than that in the interior, the phenomenon is called adsorption. Conversely, it is called negative adsorption. In soil science, on the other hand, the heterogeneity in distribution of ions in soil colloidal systems is interpreted mainly in terms of electrostatic interactions occurring at the interface between soil colloidal particles and the liquid phase (Bear, 1964). Owing to adsorption or negative adsorption, the concentration of ions at the surface of soil colloidal particles or adjacent to the surface is higher or lower than that in the diffuse layer or the free solution.

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Jolivet, Jean-Pierre. "Water and Metal Cations in Solution." In Metal Oxide Nanostructures Chemistry. Oxford University Press, 2019. http://dx.doi.org/10.1093/oso/9780190928117.003.0005.

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Water has an exceptional ability to dissolve minerals. It is safe and chemically stable, and it remains liquid over a wide temperature range. Thus, it is the best solvent and reaction medium for both laboratory and industrial purposes. Water is able to dissolve ionic and ionocovalent solids because of the high polarity of the molecule (dipole moment μ = 1.84 Debye) as well as the high dielectric constant of the liquid (ε = 78.5 at 25°C). This high polarity allows water to exhibit a strong solvating power: that is, the ability to fix onto ions as a result of electrical dipolar interactions. Water is also an ionizing liquid able to polarize an ionocovalent molecule. For example, the solvolysis phenomenon increases the polarization of the HCl molecule in aqueous solution. Finally, owing to the high dielectric constant of the liquid, water is a dissociating solvent that can decrease the electrostatic forces between solvated cations and anions, allowing their dispersion as H+solvated and Cl−solvated through the liquid. (The attractive force F between charges q and q′ separated by the distance r is given by Coulomb’s law, F = qq′/εr2.) These characteristics are rarely found together in common liquids. The dipole moment of the ethanol molecule (μ = 1.69 Debye) is close to that of water, but the dielectric constant of ethanol is much lower (ε = 24.3). Ethanol is a good solvating liquid, but a poor dissociating one; consequently, it is considered a bad solvent of ionic compounds. Dissolution in water of an ionic solid such as sodium chloride is limited to dipolar interactions with Na+ and Cl− ions and their dispersion in the liquid as solvated ions, regardless of the pH of the solution. Cations with higher charge, especially cations of transition metals, retain a fixed number of water molecules, thereby forming a true coordination complex [M(OH2)N]z+ with a well-defined geometry. In addition to the dipolar interactions, water molecules behave as true ligands because they are Lewis bases exerting an electron σ-donor effect on the empty orbitals of the cation.

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Haymet, A. D. J. "Dissociation and solvation in water and aqueous solutions." In Studies in Physical and Theoretical Chemistry. Elsevier, 1995. http://dx.doi.org/10.1016/s0167-6881(06)80771-8.

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Jolivet, Jean-Pierre. "Condensation in Solution: Polycations and Polyanions." In Metal Oxide Nanostructures Chemistry. Oxford University Press, 2019. http://dx.doi.org/10.1093/oso/9780190928117.003.0006.

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Condensation of metal complexes in solution forms entities in which the cations are linked by hydroxo (HO−) or oxo (O2−) bridges. The reaction is initiated by the addition of a base to an aquocomplex: . . . 2[Cr(OH2)6]3++ 2HO- → [Cr2(OH)2(OH2)8]4+ + 2 H2O . . . or by the addition of an acid to an anionic complex: . . . 2 [CrO4]2- + 2H+ → [Cr2O7]2- + H2O . . . Thus, purely aquo- and purely oxocomplexes are stable in solution, and the condensation of cations is initiated by hydroxylation. With regard to electrically charged hydroxylated complexes, the reaction forms discrete and soluble entities—polycations and polyanions with a molecular complexity which depends on acidity conditions. This chapter presents a detailed study of their formation and structure. With regard to noncharged hydroxylated complexes, the condensation reaction is no longer limited and leads to the formation of a solid (a subject that is examined in the following chapters). The hydroxylation reaction is the key stage to initiate the condensation of cations in solution. It is thus important to precise the mechanism of the successive steps of the process, in order to understand why the behavior of a cation is closely related to its oxidation state, and why the reaction product may be a discrete molecular species or a solid. As a cation generally exhibits its maximum coordination number in the initial monomeric complex and in condensed species, the condensation reaction is a substitution that proceeds according to one of three basic mechanisms: dissociation, association, and interchange or direct displacement [1, 2]. Dissociative substitution is a two-step process involving the formation of a reduced-coordination intermediate: In the first step, a labile ligand, the leaving group, breaks its bond in the starting complex before a nucleophilic entering group completes, in the second step, the cation coordination (Fig. 3.1 a). Associative substitution is also a two-step process in which the intermediate temporarily has increased coordination. The bond with the nucleophilic entering group (first step) occurs prior to the release of the leaving group (second step) (Fig. 3.1 b).

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Pines, Ehud. "The Kinetic Isotope Effect in the Photo-Dissociation Reaction of Excited-State Acids in Aqueous Solutions." In Isotope Effects In Chemistry and Biology. CRC Press, 2005. http://dx.doi.org/10.1201/9781420028027.ch16.

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Chojnowski, Julian, and Włodzimierz Stańczyk. "Dissociative Pathways in Substitution at Silicon in Solution: Silicon Cations R3Si+, R3Si+ ← Nu, and Silene-Type Species R2Si=X as Intermediates." In Advances in Organometallic Chemistry. Elsevier, 1990. http://dx.doi.org/10.1016/s0065-3055(08)60503-1.

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Conference papers on the topic "Solution (Chemistry) Dissociation"

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Tang, Shuyun, and Yunren Qiu. "Selective Separation of Cu (II) and Cd (II) from Aqueous Solution by Shear Induced Dissociation and Ultrafiltration Using Rotating Disk Membrane." In The Second International Conference on Materials Chemistry and Environmental Protection. SCITEPRESS - Science and Technology Publications, 2018. http://dx.doi.org/10.5220/0008189503190322.

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Dias, Filipe, José Páscoa, and Carlos Xisto. "Numerical Analysis of a Multi-Species MHD Model for Plasma Layer Control of Re-Entry Vehicles." In ASME 2018 International Mechanical Engineering Congress and Exposition. American Society of Mechanical Engineers, 2018. http://dx.doi.org/10.1115/imece2018-87467.

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Several critical aspects control the successful reentry of vehicles on the earth’s atmosphere: continuous communication, GPS signal reception and real-time telemetry. However, there are some common issues that can interfere with the instruments operation, the most typical being the radio blackout, in which the plasma layer frequency modifies the electromagnetic waves in a way that makes communications to and from the spacecraft impossible. So far, there have been several proposed techniques to mitigate radio blackout, one of which is the usage of electromagnetic fields. Previous studies have p

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