Concentration effect of Sodium Chloride Salt on Benzoic Acid Solubility and Dissociation into Water at 298 K Temperature

Mishra, Shiv Prakash

doi:10.9734/irjpac/2021/v22i630416

Cited by 2 publications

(2 citation statements)

References 15 publications

(21 reference statements)

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“…Notably, the each solute substances having a specific solvation and dissociation properties into a given solvent, which is depends on various factors such as pressure, temperature, intermolecular forces, bonding and polarity of substances etc [1][2][3]. A slightly changing is appears due to solute-solvent interactions when by addition of small amount of solute into water like solvent, then it trying to dissolve in it and get ionizes with their ionic strength in respect of temperature [4][5][6][7].…”

Section: …………………………………………………………………………………………………… Introduction:-mentioning

confidence: 99%

Thermodynamic Based Aqueous Solvation and Dissociation of Benzoic Acid

Mishra¹,

Singh²

2023

IJAR

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In article, we have reported a thermodynamic based study of aqueous solvation of benzoic acid (C6H5COOH) at 288 to 318 Kelvin temperature. At this temperature range the dissociation constant (Ka) of benzoic acid into aqueous solvent has been determined by applying of titration method against standard basic solution of NaOH at different ionic strength of NaCl. Although, in observation, the value of Ka is being inversely proportional in respect of temperature in between 289 K to 303 K, and at higher temperature in between 303 K to 314 K, it being directly proportional. This reports that, there are no regular correlation in between temperature and Ka of that acid. Graphically, the plot has shown the value of Ka of benzoic acid is being 4.176 at 298 K temperature. In finding of precious results for benzoic acid solvation and its dissociation into water the applying Vant Hoff equation with Gibbs free energy change relationship (âˆ†G = âˆ†H - Tâˆ†S) for reaction (endothermic or exothermic) process at standard condition of thermodynamic parameters as in terms of enthalpy (H) and entropy (S). Where, the thermodynamic parameters value (in kJ.mol-1) are being as âˆ†G = 12.507, âˆ†H = 3.823 and âˆ†S = -29.14, but, at 298 K it is show that, the acid dissociation into aqueous is an endothermic process and non-spontaneous.

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Section: …………………………………………………………………………………………………… Introduction:-mentioning

confidence: 99%

Thermodynamic Based Aqueous Solvation and Dissociation of Benzoic Acid

Mishra¹,

Singh²

2023

IJAR

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“…Indeed, the each solute substances having a specific solubility or dissociation into a given solvent, which is depends on various factors such as pressure, temperature, intermolecular forces, bonding and polarity of substances etc [1][2][3]. A slightly changing is appears due to solutesolvent interactions when by addition of small amount of solute into water like solvent, then it trying to dissolve in it and get ionizes with their ionic strength in respect of temperature [4][5][6][7][8]. Although, the dissociation of solute into solvent have earlier reported [9], but, it proved well by Nernst in 1891 with given partition law, K = C A /C B [10].…”

Section: Introductionmentioning

confidence: 99%

Gibbs Free Energy Change (∆G) in Aqueous Dissociation of Benzoic Acid at Temperature ‘K’: A Thermodynamic Study

Mishra

Singh²

2022

CSIJ

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In article, we have reported a thermodynamic based study of the Gibbs free energy change (∆G) in aqueous dissociation of benzoic acid at Kelvin temperature range in between of 288 K to 318 K. Thermodynamically, at this Kelvin temperatures range the dissociation constant (Ka) of benzoic acid into aqueous solutions have been determined by applying of titration method against standard basic solution of NaOH at different concentrations or ionic strength of NaCl. In observation, the value of Ka is being inversely proportional with respect to temperature in between 289 K to 303 K, and at higher temperature in between 303 K to 314 K, it being directly proportional. This is reported that, there are no regular correlation in between temperature and Ka of that acid. In graph, the plot has shown the value of Ka of benzoic acid is being 4.176 at 298 K temperature. Thus, in finding of precious results for benzoic acid dissociation into water an applying the Gibbs free energy change relationship (∆G = ∆H - T∆S) for endothermic or exothermic reaction process at standard condition of thermodynamic parameters. These parameters value (in kJ.mol-1) are being as ∆G = 12.507, ∆H = 3.823 and ∆S = -29.14. And, at 298 K, it is show that the acid dissociation into aqueous solvent is an endothermic and non-spontaneous process with ordered entropy (∆S).

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Concentration effect of Sodium Chloride Salt on Benzoic Acid Solubility and Dissociation into Water at 298 K Temperature

Cited by 2 publications

References 15 publications

Thermodynamic Based Aqueous Solvation and Dissociation of Benzoic Acid

Thermodynamic Based Aqueous Solvation and Dissociation of Benzoic Acid

Gibbs Free Energy Change (∆G) in Aqueous Dissociation of Benzoic Acid at Temperature ‘K’: A Thermodynamic Study

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