Measurement of pH in Acetic Acid-Sodium Acetate Buffer Solutions | Chapter 9 | Chemistry and Biochemistry: Research Progress Vol. 6

A buffer solution refers to a system that has the property of being able to eliminate or diminish the influence of external conditions on a chemical system. In pH determination, various factors influence the pH of a buffer solution, including changes in temperature, ionic strength, hydrogen ion activity, dilution, and the addition of electrolyte salts. Acidic buffers have a pH of less than 7, where for neutral buffer solutions the pH is 7, and if any buffers have a pH of more than 7, it is known as basic buffers, respectively. In this study, the preparation of acetic acid-sodium acetate buffer solutions was reported, and its pH was determined by using a pH meter at about 25°C. In preparation of buffer solutions, firstly, 1.5 ml of glacial acetic acid was taken into a 100 ml standard flask for making up 0.2M of acetic acid solution, and 0.64 g of sodium acetate was dissolved in 100 ml of distilled water. Then, 36.2 ml of prepared solution of sodium acetate was taken into a 100 ml standard flask and 14.8 ml of prepared acetic acid was added to make its volume 100 ml by using distilled water, making it a buffer. In measuring the pH of prepared buffer solutions, a calibrated digital pen pH meter was used for quick resolution of readings with accuracy. The pH of acetic acid-acetate buffer solutions was gradually raised by adding a small quantity of 5N NaOH solution into the buffer sample, and the adjusted pH was adjusted to 4.7. By meticulously outlining the preparation process and employing a calibrated pH meter for precise pH determination, this study enhances the understanding of buffer systems' behaviour when subjected to pH changes. Such insights are crucial for maintaining stable conditions in biochemical experiments and industrial processes, where pH control is vital for optimal performance and reaction outcomes.

 

Author(s) Details

Shiv P. Mishra
Department of Chemistry, Shia PG College, Lucknow-226020, UP, India.

R. P. Singh
K.N.I.P.S.S., Sultanpur-228118, (U.P.), India.

 

Please see the book here:- https://doi.org/10.9734/bpi/cbrp/v6/5689

Exploring the Synthesis, Isolation, and Characterization of a Derivative of (Pyrazol-4-yl)acetic Acid within the Framework of Chemical Investigation | Chapter 6 | Current Innovations in Chemical and Materials Sciences Vol. 9

 

The present investigation is related to the construction of novel 3-(3-bromophenyl)-2-(1,3-diphenyl-1H-pyrazol-4-yl)acrylic acid by reacting methyl 1,3-diphenyl-1H-pyrazole-4-carboxylate with 3-bromophenyl aldehyde. The hydrazone prepared from acetophenone and phenyl hydrazine was subjected to the Vilsmeier-Haack reagent and after the usual workup, 4-formyl pyrazole was obtained. The 4-formylpyrazole was further converted into methyl pyrazole-4-carboxylate via various intermediates such as (1,3-diphenyl-1H-pyrazol-4-yl)methanol, 4-(chloromethyl)-1,3-diphenyl-1H-pyrazole, and 2-(1,3-diphenyl-1H-pyrazol-4-yl)acetonitrile. The methyl 1,3-diphenyl-1H-pyrazole-4-carboxylate is a key scaffold that was further used for Knoevenagel condensation with substituted aldehydes to get the (pyrazol-4-yl)acetic acid derivatives. All intermediates and the final target were characterized by their spectral data.

Author(s) Details:

Karan Singh,
Department of Chemistry, Indira Gandhi University, Meerpur, Rewari-122502, Haryana, India.

Harshita Phougat
Department of Chemistry, Indira Gandhi University, Meerpur, Rewari-122502, Haryana, India.

Please see the link here: https://stm.bookpi.org/CICMS-V9/article/view/14337

Study on a Potassium Recovery Method for the KCl Form in Biomass Incineration Ash Utilizing Different Extraction and Recovery Methods | Chapter 10 | Research Aspects in Chemical and Materials Sciences Vol. 1

 The goal of this research was to separate potassium ion from calcium ion, which affects potassium purity when extracted and recovered from incineration ash, as well as to lessen the environmental burden of the final waste liquid. Potassium tartrate is made by extracting calcium as calcium tartrate using acetic acid, a weak acid, then adding tartaric acid to the filtrate to separate calcium as calcium tartrate, then concentrating and evaporating the solution. All of the experiments were carried out in a batch mode. When the solid–liquid ratio was 1:20, an acetic acid solution of 0.5 mol/L was utilised for extraction, and the extraction extent was 95.4 percent. Following the filtration of the extract, 10 mL of 10% tartaric acid was added to 20 mL of extract, resulting in solid precipitation. When the solids were separated and potassium was dissolved in the acid, 72 percent of the extract was recovered. The syngenite technique works best when a magnesium dosage of 5 mmol/L is added, and the Ca:K ratio is 1:2.1 with 42mol percent K at pH 11. This might be a suggestion as to which way of recovering K is most successful and efficient.

Author(s) Details:

Hiroyuki Harada,
Graduate School of Comprehensive Academic Studies, Prefectural University of Hiroshima, Japan.

Endar Hidatat,
Graduate School of Comprehensive Academic Studies, Prefectural University of Hiroshima, Japan.

Afan Bagus Mananda,
Graduate School of Comprehensive Academic Studies, Prefectural University of Hiroshima, Japan.

Please see the link here: https://stm.bookpi.org/RACMS-V1/article/view/7107