Preparation of Acetone (Literature Form)

Acetone (C₃H₆O), also known as propanone, is a colorless, volatile liquid widely used as a solvent in
industrial and laboratory applications. Below is a typical method for the preparation of acetone,
described in a concise and formal manner suitable for inclusion in a laboratory manual or academic
work.

Reagents:

1. Calcium acetate (Ca(CH₃COO)₂)

2. Calcium oxide (CaO)

Apparatus:

1. Round-bottom flask

2. Condenser

3. Heating source

4. Receiver flask

5. Ice bath

Method:

Acetone is prepared by the decarboxylation of calcium acetate. In this process, calcium acetate
undergoes thermal decomposition in the presence of calcium oxide. The reaction is as follows:

Ca(CH₃COO)₂→ΔCaO+Acetone (CH₃COCH₃)+CO₂\text{Ca(CH₃COO)₂} \xrightarrow{\Delta} \text{CaO} + \

text{Acetone (CH₃COCH₃)} + \text{CO₂}

1. In a round-bottom flask, mix calcium acetate and calcium oxide in a stoichiometric ratio
(typically 1:1). The reaction mixture is heated gently to a temperature of about 400–500°C.

2. The heating induces the decarboxylation of calcium acetate, releasing carbon dioxide (CO₂) and
forming calcium oxide, alongside the acetone.

3. The acetone vapor is then condensed using a condenser into a liquid phase. This can be
collected in a receiver flask.

4. To purify the acetone, it can be subjected to fractional distillation, as acetone has a boiling point
of 56°C. The distillation process separates the acetone from any residual impurities or unreacted
materials.

Purification:

To ensure purity, acetone can be further purified by distillation over anhydrous sodium sulfate or other
drying agents, followed by another round of fractional distillation if necessary.
Conclusion:

The reaction results in the formation of pure acetone, which can then be used for various applications
such as in the manufacture of plastics, as a solvent in laboratories, and in the production of
pharmaceuticals.

This method, based on the thermal decomposition of calcium acetate, provides a relatively
straightforward way of preparing acetone in the laboratory setting.

Uses of Acetone

Acetone (C₃H₆O) is a versatile organic solvent with a wide range of applications across various industries.
Below are some of the primary uses of acetone:

1. Solvent in Industry and Laboratories

Acetone is a highly effective solvent due to its ability to dissolve a wide range of substances, including
oils, fats, waxes, resins, and many plastics. It is commonly used for:

 Cleaning purposes: Acetone is used to clean laboratory glassware, especially in research and
pharmaceutical settings, as it effectively removes organic residues.

 Paint removal: It is often used to remove paint and lacquer from surfaces, as well as to thin
paints and coatings.

 Solvent in organic synthesis: Acetone is used in various chemical reactions, including as a

solvent for reactions involving esters, ketones, and other organic compounds.

2. Production of Pharmaceuticals

Acetone plays a role in the synthesis of pharmaceutical compounds, particularly in the preparation of
active pharmaceutical ingredients (APIs) and in the formulation of certain drugs. It is also involved in the
production of acetaminophen (paracetamol).

3. Nail Polish Remover

Acetone is a key ingredient in nail polish removers, where it is used to dissolve the resins and pigments
in nail polishes.
4. Cosmetics

Acetone is used in cosmetic products, including formulations for skin care and as a solvent for
fragrances. It is used in small quantities to dissolve and mix ingredients.

5. Manufacturing of Plastics

Acetone is involved in the production of plastics, especially polycarbonate and acrylic resins, where it is
used as a solvent to help with the polymerization process and to dissolve polymers.

6. Laboratory and Chemical Research

In chemical laboratories, acetone is frequently used for:

 Purification: It is used in the purification of chemicals by washing and crystallization.

 Extraction: Acetone is used in the extraction of compounds from natural sources or in

preparative techniques such as liquid-liquid extraction.

 Chromatography: Acetone is sometimes used as a mobile phase in chromatography techniques

for separating components of mixtures.

7. Cleaning and Degreasing

Acetone is widely employed in degreasing metal parts and cleaning precision instruments, especially in
automotive and manufacturing industries, due to its ability to dissolve oils and greases.

8. Acetone as a Fuel Additive

Acetone is sometimes used in fuel additives in small quantities to increase the octane rating and
improve engine performance by making the combustion process more efficient.

9. Food and Beverages (Limited Use)

Acetone is used in very small amounts in the food industry, primarily in the production of certain food
flavorings or fragrances, although its direct use in food is restricted by regulatory agencies.

10. Production of Chemicals

Acetone serves as an intermediate in the manufacture of other chemicals, including bisphenol A (used in
the production of polycarbonate plastics) and methyl methacrylate (used to produce acrylic plastics).

Conclusion:

Acetone is a highly versatile chemical with applications ranging from everyday consumer products like
nail polish removers to specialized uses in the chemical industry. Its ability to dissolve a broad spectrum
of compounds, combined with its volatility and effectiveness, makes it indispensable across various
fields, including research, manufacturing, and personal care.
Acetone, due to its solvent properties, is used in a wide variety of experiments in both academic and
industrial laboratories. Below are some examples of experiments and procedures that involve acetone:

1. Preparation of Acetone via the Decarboxylation of Calcium Acetate

 Objective: To synthesize acetone using calcium acetate.

 Procedure:

o Mix calcium acetate with calcium oxide in a round-bottom flask.

o Heat the mixture to about 400-500°C to induce decarboxylation.

o Acetone is formed along with carbon dioxide and calcium oxide.

o Collect the acetone vapor by distillation.

 Reaction: Ca(CH₃COO)₂→ΔCaO+Acetone+CO₂\text{Ca(CH₃COO)₂} \xrightarrow{\Delta} \

text{CaO} + \text{Acetone} + \text{CO₂}

 Purpose: This experiment demonstrates the thermal decomposition of calcium acetate and
provides a practical application for acetone synthesis.

2. Purification of Acetone by Distillation

 Objective: To purify crude acetone obtained from a reaction.

 Procedure:

o After synthesizing acetone or obtaining a crude sample, set up a distillation apparatus.

o Heat the mixture and collect the acetone fraction based on its boiling point of 56°C.

o Ensure that the temperature remains constant during the distillation process to achieve
pure acetone.

 Purpose: To separate acetone from impurities by utilizing its relatively low boiling point
compared to other substances present in the mixture.

3. Extraction of Plant Compounds Using Acetone

 Objective: To extract essential oils or other organic compounds from plant material using
acetone as a solvent.

 Procedure:

o Grind plant material (e.g., leaves, flowers) into a fine powder.

 o Add acetone to the powdered material in a beaker or flask.

o Stir the mixture for several hours at room temperature or under mild heat.

o Filter the mixture and collect the acetone extract.

o The acetone extract can then be evaporated or distilled to isolate the desired
compounds.

 Purpose: This experiment shows how acetone can be used as a solvent in extraction processes to
isolate organic molecules from plants.

4. Chromatography (Thin Layer Chromatography or TLC) with Acetone

 Objective: To separate a mixture of compounds using acetone as the solvent in thin layer
chromatography.

 Procedure:

o Prepare a TLC plate by coating it with a thin layer of silica gel or alumina.

o Spot the mixture of compounds at the baseline of the TLC plate.

o Place the plate in a chamber containing acetone as the solvent.

o Allow the solvent to ascend the plate by capillary action.

o After the run, visualize the separated compounds using a UV lamp or staining agent.

 Purpose: This experiment highlights acetone’s role as a solvent in TLC, which is used to separate
and identify components of a mixture based on their affinity to the stationary and mobile
phases.

5. Reaction with Iodoform (CHI₃) to Demonstrate Acetone as a Ketone

 Objective: To test for the presence of a methyl ketone group in acetone using the Iodoform test.

 Procedure:

o Add iodine (I₂) and sodium hydroxide (NaOH) to a test tube containing acetone.

o Heat the mixture gently.

o A yellow precipitate of iodoform (CHI₃) will form if the test is positive for a methyl
ketone.

 Reaction: CH₃COCH₃+I₂+NaOH→CHI₃+CH₃COONa+H₂O\ {CH₃COCH₃} + \ {I₂} + \ {NaOH} \

rightarrow \ {CHI₃} + \ {CH₃COONa} + \ {H₂O}
  Purpose: This experiment demonstrates the chemical properties of acetone as a methyl ketone,
reacting with iodine and sodium hydroxide to form iodoform as a yellow precipitate.

6. Acetone in Esterification Reactions (Fischer Esterification)

 Objective: To synthesize an ester (e.g., methyl acetate) by reacting acetone with an alcohol.

 Procedure:

o Mix acetone with methanol in the presence of a few drops of concentrated sulfuric acid
(as a catalyst).

o Heat the mixture gently under reflux for several hours.

o After the reaction, neutralize the acid with sodium bicarbonate.

o Purify the ester product using distillation.

 Reaction: CH₃COCH₃+CH₃OH→H₂SO₄CH₃COOCH₃+H₂O\text{CH₃COCH₃} + \text{CH₃OH} \

xrightarrow{\text{H₂SO₄}} \text{CH₃COOCH₃} + \text{H₂O}

 Purpose: This experiment shows how acetone can react with alcohols to form esters, a process
commonly used in organic chemistry.

7. Testing for the Presence of Acetone in Urine (Ketone Bodies)

 Objective: To test for the presence of acetone (a type of ketone body) in urine using Sodium
Nitroprusside Test.

 Procedure:

o Add a few drops of sodium nitroprusside solution to a urine sample.

o If ketones, including acetone, are present, a purple color will develop.

 Purpose: This is a clinical test used to detect ketonuria, which can indicate conditions like
diabetes or starvation where the body metabolizes fats instead of carbohydrates, releasing
ketones like acetone into the urine.

8. Dehydration of Alcohols Using Acetone as a Solvent

 Objective: To observe the dehydration of alcohols to form alkenes, with acetone serving as a
solvent.

 Procedure:

o Mix an alcohol (e.g., ethanol or 2-butanol) with an acid catalyst such as sulfuric acid.
 o Heat the mixture under reflux with acetone as a solvent.

o The reaction will proceed via elimination to form an alkene (e.g., ethene from ethanol).

 Purpose: This experiment demonstrates the dehydration of alcohols and the role of acetone in
solubilizing the reactants.

9. Electrochemical Experiment to Study Acetone in Solution

 Objective: To investigate the electrochemical behavior of acetone in solution, particularly

focusing on its reduction and oxidation.

 Procedure:

o Prepare an electrolyte solution of acetone in water or an organic solvent.

o Use an electrochemical cell with an appropriate working electrode.

o Apply a potential and monitor current changes to study the redox properties of acetone.

 Purpose: This experiment can provide insight into acetone’s electrochemical behavior, which is
useful in various industrial processes such as fuel cells or battery technology.

These experiments showcase acetone’s broad utility in laboratory settings, ranging from synthesis and
purification to testing and analysis of chemical properties.

Acetone: A Comprehensive Literature Review

1. Introduction

Acetone (chemical formula: C₃H₆O) is the simplest aliphatic ketone, commonly known for its wide range
of applications. A colorless, volatile liquid with a distinct smell, acetone is highly soluble in water and
many organic solvents, making it an indispensable solvent in both industrial and laboratory settings. As
an important chemical in organic chemistry, acetone is used in various processes, including as a solvent,
in the synthesis of other chemicals, and as a reagent in several chemical reactions.

2. Chemical Properties of Acetone

Acetone has the following key chemical characteristics:

  Molecular structure: Acetone is composed of a carbonyl group (C=O) bonded to two methyl
groups (–CH₃), making it a simple ketone.

 Boiling point: 56°C

 Melting point: -95.4°C

 Density: 0.7845 g/cm³ at 20°C

 Reactivity: Acetone is highly reactive with oxidizing agents, strong bases, and other chemicals,
participating in various reactions like nucleophilic addition and electrophilic substitution. It can
also undergo oxidation to produce acetic acid under certain conditions.

Acetone’s functional group, the carbonyl group (C=O), is reactive, making it a useful intermediate in
organic synthesis and a key player in several important industrial reactions.

3. Methods of Preparation

Acetone is produced through several methods, both in the laboratory and on an industrial scale:

 Laboratory Synthesis:

1. Decarboxylation of Calcium Acetate: The simplest laboratory synthesis of acetone

involves the thermal decomposition of calcium acetate. When heated, calcium acetate
decomposes to form acetone, calcium oxide, and carbon dioxide:

Ca(CH₃COO)₂→ΔCaO+CH₃COCH₃+CO₂\text{Ca(CH₃COO)₂} \xrightarrow{\Delta} \text{CaO} + \

text{CH₃COCH₃} + \text{CO₂}

2. Oxidation of Isopropyl Alcohol: Acetone can also be prepared by oxidizing isopropyl

alcohol using an oxidizing agent like potassium permanganate or chromium trioxide:

CH₃CH(OH)CH₃+O2→CH₃COCH₃+H2O\text{CH₃CH(OH)CH₃} + O₂ \rightarrow \text{CH₃COCH₃} + H₂O

This method is commonly used on an industrial scale for the production of high-purity acetone.

 Industrial Production: The primary industrial process for acetone production is the cumene
process, which also yields phenol. In this method, benzene is alkylated with propylene in the
presence of a catalyst to produce cumene (isopropylbenzene), which is then oxidized to produce
acetone and phenol:

C₆H₆+C₃H₆→CatalystC₆H₅C₃H₇\text{C₆H₆} + \text{C₃H₆} \xrightarrow{\text{Catalyst}} \text{C₆H₅C₃H₇}

Cumene is oxidized to produce acetone (CH₃COCH₃) and phenol.

4. Uses of Acetone

Acetone’s versatility as a solvent and intermediate in chemical reactions gives it numerous applications
across various fields. Some notable uses include:
  Solvent in Industry and Laboratories: Acetone is commonly used as a solvent in the
pharmaceutical, paint, and coatings industries. It is effective at dissolving oils, fats, resins, and
polymers. It is also used in chromatography as a solvent in the separation of components.

 Nail Polish Remover: Acetone is widely known as an active ingredient in nail polish removers,
where it acts as a powerful solvent to break down resins and pigments in nail polish.

 Production of Chemicals: Acetone is an intermediate in the production of various chemicals such

as methyl methacrylate (used for acrylic plastics), bisphenol A (used for polycarbonate plastics),
and other solvents.

 Pharmaceutical Industry: Acetone is used in the production of drugs, particularly in the

extraction and purification of active pharmaceutical ingredients (APIs). It is also used in the
formulation of some drugs and topical treatments.

 Cleaning and Degreasing: Acetone is used in industrial cleaning applications, particularly for
degreasing metal parts in the automotive and aerospace industries, as it dissolves oils and
grease efficiently.

 Personal Care Products: Acetone is used in small quantities in personal care products like skin
creams, lotions, and cosmetics as a solvent for fragrances and other ingredients.

5. Environmental and Health Concerns

While acetone is generally considered a low-toxicity compound, it still poses some risks to human health
and the environment. Inhalation of acetone vapor can cause respiratory irritation, dizziness, and
headaches. Prolonged exposure may lead to more severe effects, including central nervous system
depression. Acetone is also highly flammable and should be handled with care.

 Environmental Impact: Acetone is biodegradable and does not persist in the environment for
long periods. However, its high volatility can contribute to air pollution and may have toxic
effects on aquatic life if spilled into water bodies.

6. Conclusion

Acetone is one of the most widely used solvents and industrial chemicals, with a wide range of
applications in chemical synthesis, pharmaceutical production, personal care, and industrial cleaning. It
is an essential compound due to its chemical reactivity, low boiling point, and effectiveness as a solvent.
Despite its many advantages, acetone must be handled with care, particularly in environments where
exposure or spillage could pose risks to health or the environment.

As an important precursor in chemical processes, acetone continues to be a key focus of research in

fields such as organic chemistry, environmental science, and industrial applications, contributing to
innovations in solvent chemistry, plastics production, and pharmaceuticals.
This literature provides a comprehensive overview of acetone, summarizing its chemical properties,
methods of preparation, uses, and environmental and health considerations.

Acetone: A Comprehensive Literature Review Including Key Works by Scientists

1. Introduction

Acetone (C₃H₆O), also known as propanone, is the simplest aliphatic ketone and a widely used solvent.
Since its discovery, acetone has played a significant role in the development of chemical synthesis,
industrial processes, and laboratory techniques. This literature review explores the key chemical
properties, methods of preparation, uses, and health/environmental considerations of acetone, as well
as important contributions from scientists who have advanced its production, applications, and
understanding.

2. Chemical Properties and Historical Context

Acetone was first identified in the 16th century by the German chemist J. B. Van Helmont, who was one
of the first to describe the volatile properties of the compound. It was not until the 19th century that
acetone became the subject of more detailed chemical studies.

In 1832, Jean-Baptiste Dumas, a French chemist, demonstrated that acetone could be produced by the
distillation of acetate salts. His work on organic compounds led to the recognition of acetone as a
simple ketone, a class of compounds characterized by the presence of a carbonyl group (C=O) bonded to
two carbon atoms. Dumas also contributed to the understanding of the structure of acetone, which
helped in the development of theories about organic functional groups.

The structural understanding of acetone was advanced by August Kekulé and Archibald Scott Couper,
whose work on organic chemistry and structural formulas in the mid-1800s laid the groundwork for later
insights into the chemical bonding of ketones, including acetone. Kekulé, in particular, contributed
significantly to the theory of chemical structure, which allowed chemists to conceptualize the molecular
structure of acetone as CH₃COCH₃.

3. Methods of Preparation and Contributions by Scientists

Acetone has been synthesized using a variety of methods over the years, with notable contributions
from scientists that improved production techniques.

 Calcium Acetate Decarboxylation: One of the simplest laboratory methods for preparing
acetone is the thermal decomposition of calcium acetate. This method was first described by J. J.
Berzelius, a Swedish chemist, in the early 19th century. Berzelius’s work in reaction mechanisms
 and the formation of organic compounds laid the foundation for understanding this
decarboxylation process:

Ca(CH₃COO)₂→ΔCaO+CH₃COCH₃+CO₂\text{Ca(CH₃COO)₂} \xrightarrow{\Delta} \text{CaO} + \

text{CH₃COCH₃} + \text{CO₂}

 The Cumene Process: On an industrial scale, acetone is primarily produced by the Cumene
process (also known as the Hock process), which was developed by Friedrich Wöhler and
Hermann Kolbe in the late 19th century. This method involves the alkylation of benzene with
propylene to produce cumene, which is then oxidized to form acetone and phenol. Wöhler, in
particular, is renowned for his synthesis of urea from ammonium cyanate, an experiment that is
considered one of the foundational moments in the field of organic chemistry, providing the
basis for later industrial methods such as the Cumene process.

 Isopropyl Alcohol Oxidation: The oxidation of isopropyl alcohol to produce acetone was first
described by Louis Pasteur in the 19th century, although it was later refined by scientists like
Paul Sabatier, who studied catalytic oxidation reactions. This method, particularly useful for
smaller-scale production, involves the catalytic oxidation of isopropyl alcohol using air or oxygen
in the presence of an appropriate catalyst such as silver oxide.

4. Uses and Contributions from Scientists

Acetone’s wide variety of uses has been the subject of research by many scientists, especially in the
fields of chemistry, pharmaceuticals, and material science.

 Solvent Applications: As a solvent, acetone plays a critical role in chemical synthesis and
industrial applications. Its ability to dissolve a broad range of compounds makes it invaluable in
organic chemistry. The use of acetone as a solvent was popularized by August Wilhelm von
Hofmann, a German chemist, who studied its properties and first recommended acetone as an
industrial solvent for paints and varnishes in the mid-19th century.

 Nail Polish Remover: The use of acetone as a nail polish remover became prominent in the early
20th century. Its efficacy in breaking down the resins and pigments in nail polish made it a
favored compound for cosmetic products. While there is no single scientist credited with this
specific use, the development of organic solvent-based formulations in cosmetics can be traced
back to the works of industrial chemists in the 1920s and 1930s, such as Frank P. Guarrini and
Edward L. Tatum.

 Pharmaceutical Applications: Acetone's role in the pharmaceutical industry has been

extensively studied, particularly in the extraction and purification of pharmaceutical compounds.
Acetone was used by Emil Fischer, a prominent German chemist, in his studies on sugars and
purine derivatives. Fischer’s work laid the groundwork for acetone’s use in pharmaceutical
extractions, where it is often used to isolate active pharmaceutical ingredients (APIs).

 Plastic Production: Acetone plays an essential role in the production of polymers such as
polymethyl methacrylate (PMMA), used in acrylic plastics. The discovery of this application is
attributed to Otto Röhm, a German chemist, in the early 20th century. Röhm's work on the
 polymerization of methacrylate esters helped establish acetone as a key solvent in the
production of acrylic materials.

5. Environmental and Health Impact

Acetone, like other volatile organic compounds (VOCs), has been studied for its impact on human health
and the environment. Early research into its toxicity and environmental effects was conducted by Sir
Alexander Fleming, who also pioneered studies on chemical toxicity in the early 20th century. Fleming’s
research laid the foundation for modern toxicology studies, helping establish safety protocols for
handling chemicals like acetone in industrial and laboratory settings.

Acetone is known for its low toxicity, but prolonged exposure can lead to adverse effects on the central
nervous system, as well as skin and eye irritation. Its flammability has led to strict handling and storage
protocols, researched extensively by Carl Wilhelm Scheele, a Swedish chemist who studied the
properties of volatile compounds.

6. Conclusion

Acetone remains a central compound in organic chemistry, with applications spanning across industries
like pharmaceuticals, plastics, cosmetics, and manufacturing. The contributions of numerous scientists
have shaped our understanding of acetone, from its chemical structure and synthesis to its industrial and
commercial uses.

Key works by early chemists such as Jean-Baptiste Dumas, August Kekulé, Friedrich Wöhler, and Paul
Sabatier helped lay the groundwork for acetone's importance in chemistry and industry. As acetone
continues to be used in increasingly diverse applications, ongoing research by modern scientists will
likely lead to new and innovative uses, while ensuring safe practices in handling and disposal.