Sodium acetate

Absorption

It is readily available in the circulation after IV administration.

Toxicity

LD50: 25956 mg/kg (Rat.)

Description

Sodium acetate (CH?COONa), the sodium salt of acetic acid, is a colorless deliquescent solid with broad applications. Industrially, it is used to neutralize sulfuric acid waste streams in textiles and as a photoresist for aniline dyes, serves as a concrete sealant to prevent water damage, acts as a seasoning in food, and functions as a buffer solution in laboratories. It is also employed in heating pads, hand warmers, and "hot ice" experiments. Laboratory synthesis involves reactions between acetates and sodium carbonate, bicarbonate, or hydroxide, while industrial production utilizes glacial acetic acid and sodium hydroxide.

Chemical properties

Sodium acetate (CH?COONa, often abbreviated as NaOAc), the sodium salt of acetic acid, is commonly produced by reacting acetic acid with sodium carbonate. This colorless salt is highly soluble in water but less so in alcohol, and finds broad applications, such as a pH modifier in toning baths.

Physical properties

Anhydrous sodium acetate is a colorless crystalline solid with a density of 1.528 g/cm3 and a melting point of 324°C. It is highly soluble in water and moderately soluble in ethanol. The trihydrate form is also a colorless crystal, with a density of 1.45 g/cm3; it decomposes at 58°C, is extremely soluble in water, has a pH of 8.9 for a 0.1M aqueous solution, and is moderately soluble in ethanol at 5.3 g/100mL.

The Uses of Sodium acetate

Sodium acetate is used as a mordant in dyeing and finds applications in photography, food additives, glucose purification, meat preservation, tanning, and as a dehydrating agent. In analytical chemistry, it is employed to prepare buffer solutions. In the food industry, it serves as a preservative for processed meats, often combined with other acid-based preservatives such as lactates and propionates at typical inclusion levels of 0.2–0.5%, and is also used in salad dressings and ready-to-eat meals.

What are the applications of Application

Sodium acetate (NaOAc) is the sodium salt of acetic acid and is generally used in organic chemistry as a weak base. Potassium acetate (KOAc) is commonly used than sodium acetate, usually as a base in palladium-catalyzed reactions. Sodium Acetate, Anhydrous is for precipitation of nucleic acids and preparation of gel stains for protein gel electrophoresis. In addition, Sodium acetate buffer solution is 3 M, non-sterile with pH 5.2±0.1; 0.2 μm filtered, and may be used in various molecular biology applications.

Background

Sodium Acetate is chemically designated CH3COONa, a hygroscopic powder soluble in water. Sodium acetate could be used as an additive in food, industry, concrete manufacturing, heating pads, and buffer solutions. Sodium is the principal cation of extracellular fluid. It comprises more than 90% of total cations at its normal plasma concentration of approximately 140 mEq/liter. The sodium ion exerts a primary role in controlling total body water and its distribution. Acetate ions act as hydrogen ion acceptors, an alternative to bicarbonate. Medically, sodium acetate is an important component as an electrolyte replenisher when given intravenously. It is mainly indicated to correct sodium levels in hyponatremic patients. It can also be used in metabolic acidosis and urine alkalinization.

Indications

Injection, USP 40 mEq is indicated as a source of sodium, for addition to large volume intravenous fluids to prevent or correct hyponatremia in patients with restricted or no oral intake. It is also useful as an additive for preparing specific intravenous fluid formulas when the needs of the patient cannot be met by standard electrolyte or nutrient solutions. Sodium acetate and other bicarbonate precursors are alkalinising agents, and can be used to correct metabolic acidosis, or for alkalinisation of the urine.

Preparation

Sodium acetate is produced by reacting sodium hydroxide or sodium carbonate with acetic acid in an aqueous solution, followed by evaporation to obtain hydrated crystals.

The chemical equations are as follows:

NaOH + CH?COOH → CH?COONa + H?O

Na?CO? + CH?COOH → 2CH?COONa + CO? + H?O

Metabolism

In liver, sodium acetate is being metabolized into bicarbonate. To form bicarbonate, acetate is slowly hydrolyzed to carbon dioxide and water, which are then converted to bicarbonate by the addition of a hydrogen ion.