A Gibbs Free Energy Change (ΔG) and Aqueous Dissociation of Benzoic Acid at Kelvin Range | Chapter 2 | Progress in Chemical Science Research Vol. 6

 In stage, we have described a thermodynamic located Gibbs free energy change (ΔG) all along in aqueous detachment of benzoic acid (C6H5COOH) in between of 288 upto 318 Kelvin hotness range. The dissociation neverending (Ka) of benzoic acid for aqueous resolutions have been contingent upon applying of titration order against standard basic answer of NaOH at different concentrations as 0.05, 0.10, 0.30, 0.40 and 0.50 of NaCl. In remark, the worth of Ka is being inversely equivalent with increase the hotness (289 K - 303 K), and above at higher hotness in between 303 K to 314 K, it being straightforwardly proportional. This is report that, skilled are no regular equivalence in this hotness range and Ka of that acid. The graph's plot displays the benzoic acid's Ka profit, which is 4.176 at 298 K. Thus, in judgment of precious results for benzoic acid detachment in aqueous an requesting the Gibbs free energy change connection (ΔG = ΔH - TΔS) for endothermic or exothermic reaction process at standard condition of thermodynamic limits. These parameters worth (in kJ.mol-1) are being as ΔG = 12.507, ΔH = 3.823 and ΔS = -29.14. It demonstrates that acid separation into an aqueous solid is an endothermic, non-spontaneous process accompanying entropy (ΔS) at 298 K.

Author(s) Details:

Shiv Prakash Mishra,
Faculty of Science (Chemistry), Dr. Rammanohar Lohia Avadh University (DR.RMLAU), Ayodhya-224001, Uttar Pradesh, India.

R. P. Singh,
Kamla Nehru Institute of Physical and Social Sciences (KNIPSS), Sultanpur-228118, Uttar Pradesh, India.

Please see the link here: https://stm.bookpi.org/PCSR-V6/article/view/9599

Titrimetric Estimation and Phenolphthalein Indicator in Distribution of Benzoic Acid into Water and Benzene-Buffer Solutions| Chapter 7 | Progress in Chemical Science Research Vol. 4

 In the chapter, we described the distribution and solubility of the solute benzoic acid in water and various pH benzene-buffer solutions, which were both tested using the titration method. The partitioning of these acids into hydrophilic solvent (water) and hydrophobic solvent (benzene) layers was studied using the shake-flask acid-base titration method over a 24-hour period at 25°C (room temperature). A phenolphthalein indicator has been employed in titrimetric assessment of the solubility of benzoic acid (solute) in aqueous solvent and in various pH buffer solutions, such as acidic (4.0), neutral (7.0), and basic (9.0). This experiment uses phenolphthalein indicator to titrate several pH benzene-buffer solutions (4.0, 7.0, and 9.0) against 0.01, 0.05, and 0.1N NaOH solutions, with the end point presenting a pink colour for each reading. The concentration of benzoic acid in the water and benzene layers is calculated using the normality determination equation and the distribution coefficient of that acid from the Nernst distribution law equation.

Author(s) Details:

Shiv Prakash Mishra,
Faculty of Science (Chemistry), Dr. Rammanohar Lohia Avadh University, Ayodhya-224001, (UP), India.

Please see the link here: https://stm.bookpi.org/PCSR-V4/article/view/8186

Thermodynamic Van’t Hoff Equation in Aqueous Dissociation of Benzoic Acid at Ordinary Temperature Range | Chapter 7| Progress in Chemical Science Research Vol. 2

The research of the dissociation process of the solute benzoic acid into water solvent at typical temperatures ranging from 288 K to 318 K was reported on in this chapter by the authors. For the given concentrations of NaCl (sodium chloride) volume as its six ionic strengths of 0.00, 0.05, 0.10, 0.30, 0.40, and 0.50 M, respectively, which are titrimetrically analysed with 0.05 M basic NaOH (sodium hydroxide) solution, the dissociation constant (Kc) of that acid is being found as -4.169, -4.045, -3.993, -3.885, -3.8 The pH of each solution is also determined using a digital pH-meter. This observation shows that the pH value of benzoic acid in water at that temperature range is inversely related to NaCl concentrations. At a temperature of 298 K, a value of benzoic acid is plotted against the equilibrium dissociation constant (Kc), illustrating how the rate of acid dissociation into water rises with increasing ionic strength. The dissociation does not always rise as the temperature rises, as shown by the graph for increasing the temperature range to the thermodynamic dissociation constant (Ka).

Author (s) Details

Shiv Prakash Mishra

Faculty of Science (Chemistry), Dr. Rammanohar Lohia Avadh University Ayodhya-224001, Uttar Pradesh, India.

View Book :- https://stm.bookpi.org/PCSR-V2/article/view/7570

Effect of Sodium Chloride Salts on Benzoic Acid Solubility and Dissociation into Water at 298 K| Chapter 4 | Progress in Chemical Science Research Vol. 1

This study looked at the influence of sodium chloride (NaCl) salt concentration on benzoic acid (C6H5COOH) solubility and dissociation in water at 298 K temperature. Titrimetrically against a 0.05 M sodium hydroxide (NaOH) solution, the solubility of benzoic acid in water and their dissociation values in six ranges of 0.00, 0.05, 0.10, 0.30, 0.40, and 0.50 M for each individual ionic strength or concentration of sodium chloride are evaluated at this temperature. The pH of each solution is measured with a calibrated pH metre. At the application temperature, the quantity of NaCl appears to be inversely linked to the pH of benzoic acid in water. The ionic strength (I) of benzoic acid is shown versus the acid's dissociation constant (Kc) in water at a certain 298 K temperature.

Author(s) Details:

Shiv Prakash Mishra,
Faculty of Science, Dr. Rammanohar Lohia Avadh University, Ayodhya-224001, (U.P.), India.

Please see the link here: https://stm.bookpi.org/PCSR-V1/article/view/6761

Effect of pH on Benzoic Acid Solubilization and Its Partition in Water-Benzene Solvents | Chapter 9 | New Innovations in Chemistry and Biochemistry Vol. 3

 The solubility of a substance is determined by the solute-solvent interaction, pH, temperature, and ionic dissociation, among other factors, where the solute is partitioned between two immiscible liquid solvents. The solubility of benzoic acid (solute) as well as its partitioning between hydrophilic water and hydrophobic benzene, which are utilised as solvents at room temperature (25°C), are described in this paper. The distribution of the solute benzoic acid between these two solvents is investigated using the shake-flask and titrimetric methods, as well as the acid-base titration method. At several pH ranges (4.0, 7.0, and 9.0), the solubility of salt benzoic acid and their partition into water and benzene-buffer solutions were also investigated.

Author(S) Details

Shiv Prakash Mishra
Faculty of Science, Dr. Ram Manohar Lohia Avadh University, Ayodhya-224001, (U.P.), India.

View Book:- https://stm.bookpi.org/NICB-V3/article/view/4013