What is Acetone?
Acetone is a colourless liquid at room temperature with a very distinct odour. Acetone is often used as a solvent, and it is also applied to thinning of oil-based paints and cleaning up of oils. It's used as a chemical additive in nail polish remover, to dissolve paint on glass bottles, and even to start up diesel engines.
Definition of Acetone
Acetone is an organic compound with the structural formula (CH3)2CO. It is the smallest and simplest member of the ketone family, also known as propanone. It is a colourless, volatile, highly flammable liquid used as a solvent in industrial products' manufacture. You can obtain Acetone by heating anhydrous calcium acetate in the laboratory. It is reminiscent of fruit. It is a natural product in the human body due to metabolic processes. It is a manufactured chemical also found naturally in the environment. Pure Acetone contains only the ions or molecules of Acetone. The most common use of Acetone in everyday life is as a nail polish remover.
Uses of Acetone in Daily Life
For the preparation of many compounds such as chloroform, sulphonal(a hypnotic), an artificial scent, cordite(a smokeless powder), etc.
For the extraction of essential oils.
Conventionally in household products, including cosmetics and natural care products.
As a solvent to wash the glass apparatus.
As a cleaning agent to remove harsh greases ranging from fabrics to engines of automobiles or other motor vehicles.
It keeps your shoes shiny and clean
It can deep clean your keyboard and stubborn marks from glass windows and metal.
As a sanitiser for beauty products
The most crucial use of Acetone is in the medical field in producing pills, tablets, and liquid medicines to maintain the proper density for increasing medicine efficiency.
Rubber Cement: Acetone is the main ingredient in rubber cement. It produces a strong bond and sets quickly but can dry out and crack over time.
Adhesives: Acetone is often used in glues, pastes, and adhesives because it dissolves the surfaces to which the substance will be applied. Acetone also acts as a thinner for some of these products.
Dissolving Agents: Acetone is a good solvent for fats, oils, plastics, and natural rubber. Acetone is used to make paints thinner and dissolve waxes out of cloth.
Preparation of Explosives: Acetone can be made from sodium bicarbonate (baking soda) and red phosphorus. Since both acetone and sodium bicarbonate are very volatile, a violent explosion will result if the ingredients come in contact with fire or a spark.
In addition, Acetone is sometimes added to gasoline as an additive to make it burn more smoothly.
Household Cleaner: Mixtures of Acetone, water, and detergents are common in cleaning products meant for wooden surfaces, metal jewellery, glass cookware, and other items.
Nail Polish Remover: Acetone is used to remove nail polish by dissolving the ingredients that make it stick to nails. It works especially well with artificial nails when applied sparingly with a cotton ball.
Oil Cleanup: When oil spills into water, a solution of 1 part acetone to 9 parts water can be used to break up the oil and make it easier for natural bacteria to clean up the spill. However, this should only be done as a last resort since other compounds may have an adverse effect on wildlife.
Industrial Uses of Acetone
Acetone is used as a solvent for acetylene, cellulose acetate, cellulose nitrate, celluloid, varnishes, lacquers, etc.
It is added to the natural gas fuel in the petroleum industry to give them better efficiency.
To remove the oil content from the water's surface in case of any accidental spill thus, saving marine life, which could have died due to depletion of oxygen.
For the safe transportation of highly flammable chemical fuel, acetylene.
In the electronic industry for cleaning small electronic gadgets.
Acetone Storage
Acetone must be stored in a jar with a tight lid as it is a highly flammable liquid in a place where there are no stoves or heat-producing sources. Store it in a fireproof container if you have to keep a large amount of Acetone
Safety Tips for Working with Acetone
Acetone can be hazardous to life if not handled appropriately. By taking some simple steps, you ensure a safe environment for yourself as well as for others. The steps you must take while working with Acetone are :
Make sure you are wearing chemical safety goggles and a shield.
Wear chemically protected clothing like gloves, boots, aprons, and avoid prolonged contact.
Make sure the area is well ventilated.
Make sure the place is dry enough so that the surface does not soak the liquid.
Keep the fire extinguisher with you.
Don't mix other compounds or solvents with Acetone.
Work in a well-ventilated area, so there is no inhalation of the fumes.
Keep the windows open when you paint.
Do not smoke or use any type of open flame in the area that is exposed to acetone fumes.
Make sure there are no open flames or heat sources near you.
Do not store chlorine or bleach in the same location as Acetone.
Don't use your acetone container as a wastebasket.
Do not try to store Acetone in plastic containers as it will dissolve the container over time and corrode metals.
Laboratory Preparation of Acetone
To prepare Acetone in the laboratory, heat it with anhydrous calcium acetate.
(CH3COO)2Ca → CH3COCH3 + CaCO3
Take the fused calcium acetate mixed with little iron filings in a retort fitted with a water condenser and a receiver. The reaction is gently heated when Acetone distils over and collects in the receiver. The distillate is shaken with a saturated sodium bisulfite solution to purify the Acetone obtained when you obtain colourless crystals. These crystals on distillation with a saturated sodium carbonate solution give Acetone an aqueous solution, which is dried over anhydrous calcium chloride and redistilled to get pure Acetone.
Chemical Properties of Acetone
In the presence of dry HCl, Acetone condenses together to form mesityl oxide, which further condenses Acetone's third molecule to form phorone.
2 CH3COCH3 → C6H10O + H20
C6H10O + CH3COCH3 → C9H14O
Acetone uses conc. H2S04 to give mesitylene or 1,3,5 trimethylbenzene.
3 CH3COCH3 → C9H12 + 3H20
Solved Examples
1. How Can Acetone be Prepared from Acetyl Chloride?
Solution: The best way to achieve Acetone from acetyl chloride in one step is the use of Acetone with dimethyl chloride. Using dimethyl chloride with acetyl chloride gives acetone and cadmium chloride as products.
2 CH3COCl + Cd(CH3)2 → 2 CH3COCH3 + CdCl2
2. How Can Acetone be Prepared from Isopropyl Alcohol?
Solution: Acetone is mainly manufactured from isopropyl alcohol or propane-2-ol from the petroleum industry. To obtain Acetone, pass the vapours of isopropyl over with copper catalyst heated at 573K.
(CH3)2CHOH → CH3COCH3 + H2
Conclusion
All the chemical properties of Acetone are summarised in this article. Acetone has many uses in various industries, mainly the chemical industry. It also has its own hazards when not handled properly, which is why one must take necessary precautions while working with it. With this article, you have gained knowledge about all the different properties of Acetone and how it is prepared in the laboratory.
Thanks for reading! Stay tuned for more articles to come, and feel free to leave your comments or questions in the section below.
FAQs on Uses of Acetone
1. What is acetone and what are its key chemical properties?
Acetone, also known as propanone, is a colourless, volatile, and flammable organic compound with the chemical formula (CH₃)₂CO. It is the simplest member of the ketone family. Its key properties include:
- Solvency: It is an excellent solvent, capable of dissolving many polar and non-polar substances, making it miscible with water, oils, and various plastics.
- Physical State: At room temperature, it is a liquid with a distinct, somewhat fruity odour.
- Boiling Point: It has a low boiling point of 56.2°C, which makes it highly volatile.
- Vapour Density: Its vapour is significantly heavier than air, causing it to accumulate in low-lying areas, which is a key safety consideration.
2. What are the most common everyday uses of acetone?
Acetone is a common ingredient in many household and personal care products due to its powerful solvent properties. Some common examples of its use include:
- Nail Polish Remover: It is the primary active ingredient in most nail polish removers, where it effectively dissolves the tough polymers in nail enamel.
- Paint and Varnish Thinner: It is used to thin oil-based paints, lacquers, and varnishes, and to clean brushes and tools after use.
- Cleaning Agent: It can effectively remove stubborn substances like superglue, permanent marker ink, and heavy grease from glass and metal surfaces.
- Surface Preparation: Before painting or applying adhesives, acetone is often used to clean and degrease surfaces to ensure better adhesion.
3. How is acetone used in industrial and pharmaceutical applications?
In industry, acetone is a crucial chemical intermediate and solvent. Its major applications include:
- Chemical Manufacturing: It is a precursor for synthesising other chemicals like methyl methacrylate (for acrylic plastic), bisphenol A (for polycarbonates), and mesityl oxide.
- Pharmaceuticals: It is used as a solvent in the production of pills and liquid medicines to help control the density and ensure the proper delivery of active ingredients.
- Safe Transport of Acetylene: Acetylene gas is highly explosive when compressed on its own. It is dissolved in acetone for safe transport and storage in cylinders.
- Textile Industry: It is used for degreasing wool and degumming silk.
4. What is the chemical formula and structure of acetone?
The chemical formula for acetone is C₃H₆O. Its structural formula, which provides more detail, is written as (CH₃)₂CO. The structure features a central carbon atom that is double-bonded to an oxygen atom (forming a carbonyl group) and also single-bonded to two separate methyl groups (–CH₃). This specific arrangement makes acetone the simplest and most important ketone.
5. How is pure acetone prepared in a laboratory setting?
A standard laboratory method for preparing acetone is the dry distillation of anhydrous calcium acetate. In this process, solid calcium acetate is heated, causing it to decompose into acetone and solid calcium carbonate. The chemical equation for this reaction is:
(CH₃COO)₂Ca(s) → CH₃COCH₃(g) + CaCO₃(s)
The resulting acetone vapour is then passed through a condenser to cool it back into a liquid, which is then collected. The collected liquid can be further purified if required.
6. Why is acetone considered such an effective and versatile solvent?
Acetone's effectiveness as a solvent is a direct result of its molecular structure. It contains both a polar carbonyl group (C=O) and two non-polar methyl groups (–CH₃). This dual characteristic allows it to interact with and dissolve a wide range of substances:
- The polar C=O group allows it to dissolve other polar substances and makes it completely miscible with water.
- The non-polar methyl groups allow it to dissolve non-polar compounds like fats, oils, greases, and many organic polymers.
This ability to dissolve both polar and non-polar materials makes it an exceptionally versatile solvent.
7. How can you chemically distinguish between acetone and acetaldehyde?
Acetone (a ketone) and acetaldehyde (an aldehyde) can be distinguished using simple chemical tests that rely on the fact that aldehydes are easily oxidised while ketones are not. Two common distinguishing tests are:
- Tollens' Test (Silver Mirror Test): When warmed with Tollens' reagent, acetaldehyde is oxidised and reduces the silver ions, forming a distinctive silver mirror on the inner surface of the test tube. Acetone does not react.
- Fehling's Test: When heated with Fehling's solution, acetaldehyde gives a brick-red precipitate of copper(I) oxide. Acetone shows no reaction with Fehling's solution.
8. What are the most critical safety precautions when handling acetone and why are they important?
Handling acetone requires strict safety measures due to its inherent properties. The most critical precautions are:
- Ensure Excellent Ventilation: This is crucial because acetone is highly volatile (evaporates quickly) and its vapours are much heavier than air. Without good airflow, flammable and intoxicating fumes can accumulate near the floor.
- Eliminate All Ignition Sources: Acetone is extremely flammable. It must be kept far from open flames, sparks, hot surfaces, and static electricity to prevent fire or explosion.
- Wear Protective Gear: Chemical-resistant gloves and safety goggles are essential. Acetone can dissolve natural skin oils, leading to severe dryness and irritation, and can cause significant eye damage upon contact.
9. Is it safe to apply pure acetone directly to the skin?
No, it is not safe or recommended to apply pure acetone directly to the skin for prolonged periods. Although it's used in diluted forms in products like nail polish removers, pure acetone is a powerful degreasing agent. It strips the skin of its natural protective oils and lipids, leading to severe dryness, cracking, redness, and dermatitis. Any use should be brief, targeted, and followed by washing the area with soap and water and applying a moisturiser.
10. Beyond its use as a solvent, how does acetone act as a building block in other chemical reactions?
Acetone is an important precursor, or starting material, in several organic synthesis reactions. For example:
- Aldol Condensation: Under basic or acidic conditions, two molecules of acetone can react with each other to form mesityl oxide, an important industrial chemical. This can react with a third acetone molecule to form phorone.
- Aromatic Synthesis: In the presence of a strong acid catalyst like concentrated sulfuric acid, three acetone molecules can condense to form mesitylene (1,3,5-trimethylbenzene), an aromatic compound.
These reactions demonstrate acetone's role as a versatile building block for creating more complex molecules.
