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Electrolyte solutions
Published in W. John Rankin, Chemical Thermodynamics, 2019
Strong electrolytes dissociate completely into ions, while weak electrolytes dissociate only partially. The principal solute species in a solution of a strong electrolyte are ions, while the principal species in a solution of a weak electrolyte is the un-dissociated compound. All ionic compounds are strong electrolytes. Even nearly insoluble ionic compounds (such as AgCl, PbSO4, CaCO3) are strong electrolytes because the small amounts that do dissolve in water do so principally as ions; that is, there is virtually no undissociated form of the compound in solution. Molecular compounds may be non-electrolytes (e.g., sucrose and ethanol), weak electrolytes or strong electrolytes. Strong acids and strong bases are strong electrolytes. Weak electrolytes include weak acids and weak bases. Some examples of aqueous electrolytes are listed in Table 12.1.
A review of thermodynamic concepts
Published in Ronald L. Fournier, Basic Transport Phenomena in Biomedical Engineering, 2017
In the previous discussion on the Gibbs-Donnan effect, the aqueous solution contained a strong electrolyte such as NaCl. Recall that a strong electrolyte in water completely dissociates into its constituent ions. Oftentimes, in biological systems, our aqueous solutions will also contain weak electrolytes such as weak acids or weak bases. Weak acids and bases only partially dissociate. An important example of a weak acid is acetic acid (CH3COOH or HOAc), and an example of a weak base is aqueous ammonia or ammonium hydroxide (NH4OH). Weak acids and weak bases, because of their partial dissociation, will affect the concentration of H+ and, as a result, the pH of the solution.
Interference screws 3D printed with polymer-based biocomposites (HA/PLA/PCL)
Published in Materials and Manufacturing Processes, 2023
J. Jamari, D.F. Fitriyana, P. S. Ramadhan, S. Nugroho, R. Ismail, A.P Bayuseno
Furthermore, the commercial interference E-screw experienced a faster mass reduction because it contains more hydroxyapatite than the biocomposite from which all interference screws are currently made. Azevedo et al.[27] conducted a study combining PCL and hydroxyapatite and confirmed that the biocomposite with the highest HA composition would degrade faster than the biocomposite with the lowest hydroxyapatite content. The current findings are also comparable to those of Moura et al. [34] who combined PLA, PCL, and HA. According to the findings of this study, the highest HA addition (10%) will result in more degraded composites. This result demonstrated that combining PLA and PCL with the addition of HA caused the biocomposite to degrade quickly. Because the NaCl solution is a strong electrolyte, the more HA immersed in the strong electrolyte solution, the faster the degradation rate.
A performance study of electrochemical micro-machining on SS 316L using suspended copper metal powder along with stirring effect
Published in Materials and Manufacturing Processes, 2022
J.R. Vinod Kumaar, R. Thanigaivelan, M. Soundarrajan
In ECMM, the general drawback is the accumulation of waste metals and their toxic by-products in the form of slurry mixed up with the electrolyte. Disposing of the toxic electrolyte becomes hazardous to the environment.[25] To overcome this problem, this paper mainly focuses on using an environmental-friendly citric acid electrolyte for conducting experiments at various levels of concentration. Aqueous citric acid is basically a weak acid to machine SS 316L. Though citric acid is a weak base electrolyte, increasing the higher level of concentration doesn’t mean that it becomes a strong electrolyte. Citric acid belongs to the category of polyprotic acids. In citric acid solution, the dissociation happens only partially with the water, only a few H+ and (C6H5O7)3-- ions are present in the solution. Citric acid usually stays together as H3C6H5O7 molecules in aqueous solution.
The electric conductance of dilute sulfuric acid in water: a new theoretical interpretation
Published in Molecular Physics, 2021
If the above analysis is wrong and HSO4− and SO42− do exist in the aqueous solution of the parent acid, and therefore α2 is a valid physical quantity, and thus, also K2 is a valid constant (except that Sherrill and Noyes were unable to calculate it accurately) then we ‘only’ end up with a strong conflict with thermodynamics, because aqueous H2SO4 behaves as a 1–3 strong electrolyte, not a 1–1/1–2 one. (For more detail, see Supplemental Material, SM-3.) Arguing that the DH–SiS and DHO–SiS theories are inadequate for judging the valence family of aqueous sulfuric acid is to no avail since the 1–3 behaviour of the acid is strictly apparent from a simple inspection of γ± data (see Ref. [1] and Ref. [37], 5–98 to 5–101; also, SM-3), and the theories only quantify the behaviour and establish the ISPs of the ionised acid, through theorising the structure of the acid and its ions. Furthermore, the theory–experiment fit is excellent for very many electrolytes of the various valence families, both for activity (DH–SiS) [7] and conductivity (DHO–SiS) [23]. It seems unexplainable why theory ‘fails’ just in the case of H2SO4, as diprotic acid, in water; why in methanol the anticipated 1–1/1–2 behaviour is, in contrast, fully manifested by DHO–SiS.