Ch3coo

Understanding CH₃COO⁻: The Acetate Ion

Introduction:

CH₃COO⁻, more commonly known as the acetate ion, is a fundamental chemical species found in various organic and inorganic contexts. It's the conjugate base of acetic acid (CH₃COOH), a weak organic acid ubiquitous in vinegar and other natural processes. Understanding the acetate ion involves grasping its structure, properties, reactions, and applications, spanning chemistry, biology, and even industrial processes. This article provides a comprehensive overview of the acetate ion, explaining its key characteristics and significance in different fields.

1. Structure and Bonding:

The acetate ion is a negatively charged anion with a molecular formula of CH₃COO⁻. Its structure features a methyl group (CH₃) attached to a carboxylate group (COO⁻). The carbon atom in the carboxylate group is double-bonded to one oxygen atom and singly bonded to another, which carries the negative charge. This negative charge is delocalized across both oxygen atoms due to resonance, meaning the negative charge isn't fixed on a single oxygen but is spread out. This resonance stabilization is crucial to the ion's stability and reactivity. The carbon-oxygen bonds in the carboxylate group exhibit a bond order of approximately 1.5, indicating a bond length intermediate between a single and a double bond. This delocalized structure is key to understanding the acetate ion's chemical behaviour.

2. Acid-Base Properties:

As the conjugate base of acetic acid, the acetate ion is a weak base. This means it can accept a proton (H⁺) to reform acetic acid. The equilibrium between acetic acid and the acetate ion is governed by the acid dissociation constant (Ka) of acetic acid. The pKa of acetic acid is approximately 4.76, indicating that it is a relatively weak acid, and consequently, its conjugate base, acetate, is a relatively weak base. In aqueous solutions, the equilibrium reaction can be represented as:

CH₃COOH ⇌ CH₃COO⁻ + H⁺

The position of this equilibrium is influenced by the pH of the solution. In acidic solutions, the equilibrium shifts to the left, favoring the formation of acetic acid. In basic solutions, the equilibrium shifts to the right, favoring the formation of the acetate ion. This reversible nature is exploited in numerous chemical applications.

3. Reactions and Applications:

Acetate ions participate in various chemical reactions. For example, they can react with metal cations to form acetate salts, such as sodium acetate (CH₃COONa), potassium acetate (CH₃COOK), and lead(II) acetate [Pb(CH₃COO)₂]. These salts have diverse applications. Sodium acetate is used as a buffer in biochemical experiments, as a food preservative (E262), and in hot packs due to its ability to undergo exothermic crystallization. Lead(II) acetate, historically used as a sweetener, is now primarily used in certain industrial processes.

Furthermore, the acetate ion can act as a nucleophile in organic chemistry reactions, participating in reactions like esterification and acylations. In esterification, the acetate ion reacts with an alkyl halide to form an ester. This reaction is commonly used in the synthesis of various organic compounds.

4. Biological Significance:

Acetate plays a crucial role in biological systems. It's an important intermediate in the metabolism of carbohydrates and fats. In the citric acid cycle (Krebs cycle), a central metabolic pathway, acetyl-CoA, a derivative of acetate, is a key component that enters the cycle and participates in energy production. Acetate is also involved in the biosynthesis of fatty acids and cholesterol. Moreover, some bacteria can utilize acetate as a primary source of carbon and energy. This metabolic versatility underscores the significant biological importance of the acetate ion.

5. Industrial Relevance:

The industrial applications of acetate are extensive. Besides its use in various salts, it's a crucial component in the production of cellulose acetate, a widely used polymer in making fibers (rayon, acetate silk), photographic films, and coatings. Acetate esters are also used as solvents in various industries. Furthermore, acetic acid, the precursor to the acetate ion, is produced industrially on a large scale through various methods, including the carbonylation of methanol. This highlights the economic significance of acetate and its derivatives.

Summary:

The acetate ion (CH₃COO⁻) is a versatile chemical species with a significant presence in various fields. Its structure, characterized by resonance stabilization, dictates its chemical reactivity. Its weak base properties, biological significance as a metabolic intermediate, and extensive industrial applications as a component in salts, polymers, and solvents highlight its importance. Understanding its behavior within different contexts requires a comprehensive appreciation of its acid-base chemistry, reaction mechanisms, and biological roles.

FAQs:

1. What is the difference between acetic acid and acetate ion? Acetic acid (CH₃COOH) is a weak acid; the acetate ion (CH₃COO⁻) is its conjugate base, formed by the loss of a proton.

2. Is acetate ion soluble in water? Acetate salts are generally water-soluble, meaning they readily dissolve in water.

3. What are the health implications of acetate? In moderate amounts, acetate is generally considered safe. However, excessive intake can lead to metabolic acidosis.

4. How is acetate produced industrially? Acetic acid, the precursor to acetate, is produced industrially through methods like the carbonylation of methanol.

5. What are some common examples of acetate salts? Sodium acetate (CH₃COONa), potassium acetate (CH₃COOK), and lead(II) acetate [Pb(CH₃COO)₂] are common examples.

Search Results:

Acid and Base Equilibrium - Florida State College at Jacksonville For every H3O+ there will be one CH3COO-. Let these concentrations = x. Acid: A proton donor. Base: A proton acceptor. An acid base reaction is one where there is a proton transfer. A …

Self-sacrificed two-dimensional REO(CH3COO) template … In situ formed single-layered (SL) and multi-layered (ML) REO(CH3COO) nanoplates are used as self-sacrificed templates to mediate the synthesis of ultrathin SL and ML RE2O3 nanoplates, …

Journal of Thermal Analysis, Vol. 30 (1985) 1095-1103 - Springer The thermal analysis of acetate clusters of general formula [Fe~IMnO(CH3COO)6(HzO)3]-2H20, with M = Mn,Fe, Coor Ni, was performed in dynamic and quasi-isothermal regimes. The …

Common Polyatomic Ions Name(s) Formula Name(s) Formula Common Polyatomic Ions Name(s) Formula Name(s) Formula ammonium NH4 acetate CH3COO C2H3O2 bromate BrO3 carbonate CO3 2-chlorate ClO3 chlorite ClO2 chromate CrO4 2-

Effects of NO3 , Cl , and CH3COO anions and diethylene glycol … precursor salts (Ce(NO3)3, CeCl3, and Ce(CH3COO)3) were used. The structure, size, and morphology of the synthesized CeO2 NPs were studied. An average crystallite size of 13 to 33 …

Journal of Thermal.~a!vsis, Vot S7(1991)993-1003 - Springer [Fe2NiO(CH3COO)6(H20)3] "2H20(II), we set out to characterize in detail the decomposition and the possibility of influencing this process, in order to draw conclusions concerning the direct …

Ka CH3COOH CH3COOH/OH OH ] = 1. - The University of Sydney Below is a simulation of the weak acid / strong base titration curve for CH3COOH versus OH - obtained in E17. The blue curve represents the titration curve, the red star is the equivalence …

Section 19.1. Acid-Base Buffer Solutions - University of Florida In everyday English, a buffer is something that lessens the impact of an external force. A buffer is a concentrated solution of a weak acid (or base), together with a salt containing the conjugate …

Crystal Structure, Polymorphism, and Anisotropic Thermal … In this paper, we present the crystal structures of the low (LT- -Ca(CH3COO)2), which α matches the previously published reference data for -α Ca(CH3COO)2 and the high-temperature form …

Chapter 17: Acid-Base Equilibria and Solubility Equilibria equilibrium is affected. This is called the common ion effect. Consider adding acetic acid (CH3COOH) and sodium acetate (NaCH3COO) to water. The acetate anion from sodium …

Structure Property Correlations in Aqueous Binary Na+/K ABSTRACT: Highly concentrated aqueous binary solutions of acetate salts are promising systems for differentelectrochemical applications, for example, energy storage devices. The very high …

Spectrographic investigation of single crystals of erbium acetate ... The present article reports an investigation of absorption spectra of Er 3+ in Er(CH3COO)3 9 4H20 single crystals and a determination from spectral data of the interaction between erbium …

Acids and Bases - The University of Sydney A weak acid (e.g. CH3COOH) is in equilibrium with its ions in water and its conjugate (CH3COO–, a weak base) is also in equilibrium in water. The position of equilibrium of a weak acid or base …

COOH CH COO + H - tsfx.edu.au T Organic acids (carboxylic acids) An example is ethanoic acid CH 3 COOH. Ethanoic acid is formed by the oxidation of ethanol. This is why alcoholic drinks go sour if they are left in the air …

Chapter 17 Buffers!! What is ”the common ion effect? It’s what happens when you add more of the product ion to an acid/base reaction. What does that do to the equilibrium? Add product (CH3CO2 -), shift to …

SAFETY DATA SHEET - FUJIFILM Wako Chemicals U.S.A. Formula (CH3COO)2Cu Chemical Name Weight-% Molecular weight ENCS ISHL No. CAS RN Copper(II) acetate 97.0 181.63 (2)-693 * 142-71-2 Note on ISHL No.: * in the table means …

Acetate C H O COO CO Ammonium NH - University of … Name:_____ Memorization For AP Chem Polyatmic Ions AP Chemistry Polyatomic Ion list Acetate C2H3O2-or CH3COO-or CH3CO 2 Ammonium NH 4 Ammonium Carbonate NH 4CO …

SAFETY DATA SHEET - FUJIFILM Wako Chemicals U.S.A. Formula (CH3COO)2Pb·3H2O Chemical Name Weight-% Molecular weight ENCS ISHL No. CAS RN Lead(II) acetate trihydrate 99.0 379.33 2-693 * 6080-56-4 Note on ISHL No.: * in the table …

Crystal, molecular, and electronic structure of carboxylate [Fe ... The crystal has an ionic structure and is composed of [Fe30(CH3COO)6(HzO)3] + complex cations, NO 3 anions, and crystaniTation water molecules. The general view of the complex …

Preparation Of Different Buffer Solutions To learn how to prepare buffers. You are provided with: 0.2M solution of CH3COOH , 0.2M solution of CH3COONa. Determine which is the weak acid and which is the conjugated base …

Ch3coo

Understanding CH₃COO⁻: The Acetate Ion

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