Category: Chemistry Notes PPT

Rennin is also known as chymosin. Rennin meaning is given as a protein-digesting enzyme that curdles milk by transforming the caseinogen into insoluble casein. It is found only in the cud-chewing animal’s fourth stomach, like cows. Its action extends the period where milk is retained in the young animal’s stomach. In animals, which lack rennin, milk can be coagulated by the pepsin action, as is the case rennin in humans. Rennet, which is a commercial form of rennin, is used in the manufacturing of preparing junket and cheese.

There are many useful pepsin and rennin actions that may be applied to humans and other living organisms.

Occurrence

The chymosin can be found in a diverse range of tetrapods, although it is one of the best-known ones to be produced by ruminant animals in the abomasum lining. Chymosin can be produced by gastric chief cells in newborn mammals to curdle the milk that they ingest by allowing a longer residence in better absorption and the bowels. Cats, pigs, seals, and chicks are non-ruminant animals that contain chymosin.

A study that is reported finding a chymosin-like enzyme in a few human infants (rennin in infants), but the others have failed to replicate this specific finding. Humans contain a pseudogene for the chymosin, which does not generate a protein found on chromosome 1. Also, humans have other proteins for milk digestion, such as lipase and pepsin.

In addition to the primate lineage leading up to humans, a few other mammals have also lost the chymosin gene.

Enzymatic Reaction

Chymosin can be used to bring about curd formation and extensive precipitation in cheese-making. Chymosin’s native substrate is K-casein that is particularly cleaved at the peptide bond between the amino acid residues 105 and 106, methionine, and phenylalanine. Calcium phospho caseinate is the resultant product. When a particular linkage between the hydrophilic (acidic glycopeptide) and hydrophobic (para-casein) groups of casein is broken, the hydrophobic groups get to unite and form a 3D network, which traps the milk’s aqueous phase.

Charge interactions between the glutamates and histidines on the kappa-casein and the aspartates of chymosin initiate enzymes, which is binding to the substrate. When chymosin isn’t the binding substrate, a beta-hairpin known as “the flap” will hydrogen bond to the active site, covering it and preventing further substrate binding.

Recombinant Chymosin

Due to the imperfections and scarcity of animal and microbial rennets, producers sought replacements. With genetic engineering development, it became possible to extract the rennet-producing genes from the stomach of animals and insert them into certain fungi, yeasts, or bacteria, to make them form chymosin during the fermentation process.

The microorganisms, which are genetically modified, can be killed after the fermentation, and chymosin is isolated from the fermentation broth so that Fermentation-Produced Chymosin (FPC), which is used by the cheese producers, does not contain any ingredient or GM component. FPC has identical chymosin as the animal source but is produced in an efficient way. Also, the FPC products have been on the market since 1990, and they are considered the ideal milk-clotting enzyme.

FPC was given as the first artificially produced enzyme to be registered and allowed by the United States Food and Drug Administration. About 60% of US hard cheese was made in 1999 with FPC, and it has around 80% of the global market share for rennet.

Coagulation of Milk

In order to understand how to coagulate milk by chymosin, one should know something about milk proteins. Casein is the most abundant protein in milk, and it comes in four different types: alpha-s1, alpha-s2, beta, and kappa. Both the alpha and beta caseins are hydrophobic proteins, which are precipitated readily by calcium – the normal calcium concentration in the milk is far more than required to precipitate these proteins.

But, kappa casein is a distinctly varied molecule, and it is not calcium-precipitable. As the caseins get secreted, they self-associate into the aggregates, known as micelles, where the alpha and beta caseins are kept from the precipitating process by their interactions with kappa casein. In essence, kappa casein preserves the bulk of milk protein soluble while also preventing it from coagulating spontaneously.

Enter chymosin. The chymosin then proteolytically cuts and inactivates kappa casein by converting it into para-kappa-casein and a smaller protein known as macropeptide. On the other side, para-kappa-casein does not hold the ability to stabilize the calcium-insoluble caseins precipitate and the micellar structure, forming a curd.

Besides its physiologic role, chymosin is also a more important industrial enzyme because it can be widely used in cheesemaking. Chymosin was extracted from dried calf stomachs in days gone by; for this purpose, however, the cheesemaking industry has expanded beyond the supply of available calf stomachs (note that these have to be from the young calves).

Also, it turns out that several proteases are able to coagulate milk by converting the casein to paracasein and alternatives to chymosin are available readily. “Rennet” is the term given to any enzymatic preparation that clots milk.

Rubidium is a silvery-white and extremely soft metal and amongst the most highly reactive elements on the periodic table. Rubidium has a density of about one and a half times that of water and is solid at room temperature, although it melts if it is just a bit warmer. It ignites spontaneously when it comes in contact with air and reacts violently with water and even with ice at -100 C, setting fire to the hydrogen that is liberated. Amongst all the other alkali metals, it forms amalgams with the element mercury. It alloys with gold, sodium, potassium and caesium. Its flame is yellowish-violet in colour. In this article, we will learn about Rb element in detail including rubidium element uses, structure, and chemical properties.

What is Rubidium?

Rubidium is a chemical element having the symbol Rb and the atomic number 37. It is an extremely soft, silvery-white coloured metal in the alkali metal group. The rubidium metal shares similarities to the potassium metal and the caesium metal when it comes to the physical appearance, softness and conductivity. It cannot be stored under atmospheric oxygen since a highly exothermic reaction would ensue, sometimes even resulting in the metal catching fire. It is the first alkali metal in the group having a density higher than water, hence it sinks, unlike the other metals that are above it in the group.

Rubidium Structure

The structure of rubidium is shown as below:

Let Us Now Look at the Chemical Properties of Rubidium

Chemical Properties of Rubidium

Rubidium Uses

Rubidium has the following uses:

1. Rubidium compounds are used in the fireworks for giving them a purple colour.

2. Rubidium is used in the thermoelectric generator by using the magnetohydrodynamic principle, wherein the hot rubidium ions are allowed to pass through a magnetic field. 

3. Vaporized rubidium, which is 87Rb, is one of the most commonly used atomic species for the laser cooling and the Bose-Einstein condensation.

4. For cold-atom applications that require tunable interactions, 85Rb is preferable because of its rich Feshbach spectrum.

5. Rubidium is also used for polarizing Helium-3 gas.

6. The resonant element in the atomic clocks utilizes the hyperfine structure of the rubidium’s energy levels, and hence, rubidium is used for high-precision timing.

7. Rubidium is used as the main component of secondary frequency references or rubidium oscillators in the cell site transmitters and several other electronic transmitting, networking, and testing equipment.

8. It is used as a working fluid in vapour turbines, as a getter in vacuum tubes, and as a component of the photocell.

9. Rubidium is used as an ingredient in a special type of glass, production of superoxide by burning in oxygen, the study of potassium ion channels in biology, and as the vapour in the atomic magnetometers.

10. Rubidium-82 is used for the positron emission tomography.

Saturation, any of several physical or chemical conditions defined by the existence of an equilibrium between pairs of opposing forces or of an exact balance of the rates of opposing processes. 

Common Saturated Solution examples include the condition of a solution left in contact with the pure undissolved solvent until there is no further change in solution concentration, and the state of a vapour equally left in contact with the substance’s pure solid or liquid form.

The water is saturated in the first case, when the rate at which the pure substance dissolves to join the solution in the solvent is precisely equal to the rate at which the dissolved substance exits the solution (e.g. by crystallising).

The rate at which the completely condensed (liquid or solid) substance vaporises in the second example is exactly the rate at which the vapour condenses.

A Saturated Solution or vapour contains the greatest concentration of a dissolved or vaporised substance that can be obtained under specified pressure and temperature conditions. While supersaturation (a condition in which concentration reaches the equilibrium value) can be brought on in certain situations, these solutions or vapours are unstable and spontaneously return to the Saturated state.

Factors Affecting Saturated Solution:

The amount of solute that can be dissolved to form a Saturated Solution in a solvent depends on a variety of factors. The most prominent considerations are:

Temperature: With temperature, the solubility decreases. For example, salt can be dissolved in hot water much more than in cold water.

Pressure: Increasing pressure in solution can force more solute. This is widely used to remove liquid gases.

Chemical Composition: Solubility affects the nature of the solute and solvent and the involvement of other contaminants in a solution. For instance, in water, you can dissolve much more sugar than salt. Ethanol and water are mutually completely soluble.

Types of Saturation:

When solid solute (substance or particles) and liquid solvent are mixed, the only possible reactions are dissolution and crystallisation.

There are three types of saturation. They are:

• Saturated Solution: It is a solution where the maximum amount of solute is, so much so that if there was any more, it would not dissolve.

• Unsaturated Solution: It is a solution where the solute concentration is lesser than its corresponding equilibrium solubility. This means that the amount of solute is in lesser amounts than the maximum value until the solution reaches its saturation level. 

• Supersaturated Solution: It contains more dissolved solute than required for making a Saturated solution. It is formed by heating a Saturated solution, then adding more solute, and then cooling it down. The excess dissolved solute crystallises with the seeding of supersaturated solution with crystals of the solute.
  

How to Make a Saturated Solution

There’s more than one way to make the Saturated Solution. You may be able to prepare it from scratch, saturate an unsaturated solution, or cause a supersaturated solution to remove any product.

Until it stops dissolving, add solute to the liquid.

Evaporate the solvent until it becomes saturated from the solution. Once the solution begins to crystallise or precipitate it will saturate the solution.

Add a seed crystal to a super – Saturated Solution so that extra solvent will grow onto the crystal, leaving the solution Saturated.

Examples of Saturated Solutions

• Soda is a source containing soluble carbon dioxide in water. Therefore carbon dioxide gas produces bubbles when the pressure is released.

• Adding chocolate powder to milk produces a Saturated Solution so it prevents dissolving.

• When molten butter or oil, salt can be applied to the stage where the salt grains avoid dissolving and create a Saturated Solution.

• A Saturated Solution can be produced if you give sufficient sugar to your coffee or tea. You’ll know when the sugar starts dissolving, you’ve reached the saturation point. Hot tea or coffee helps you absorb a lot more sugar than you can add to a cold drink.

• To form a Saturated Solution, sugar can be applied to the vinegar.

Therefore, these are everyday examples of Saturated Solutions.

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Natural fibres are obtained from plants and animals. Cotton, jute and flax are all plant fibres. While wool and silk are animal fibres. We get silk from silk moths or ‘silkworms.’ The rearing of silkworms for obtaining silk is called ‘sericulture’. Thus, meaning of sericulture or silk farming is the cultivation of silkworms or silk moths to produce silk. Sericulture is a very old occupation in India. India is the 2nd largest producer of silk in the world after China and Karnataka is the largest producer of silk in India.

Methods of Sericulture 

We get silk fibre from silk-worm cocoon. Rearing of silkworm for its silk cocoon to get silk fibre is very ancient. According to one legend, the story of silk began in 2640 BC. Si-Ling-Chi, a Chinese Empress, was walking around her garden while sipping a cup of tea when the cocoon of a silkworm fell into her cup. The cocoon soon began to unravel revealing a long silken fibre. When she looked up, she saw a Mulberry tree with several other cocoons hanging from it and a number of silkworms crawling around. This led her to conclude that the cocoon had come from the silkworm caterpillars. 

For 2500 years, the Chinese kept the art of making silk to themselves. They sold silk fabric but refused to reveal the secret of how the fabric was made. In spite of their secrecy, the knowledge of how to make silk reached Korea and India in 200 BC and 140 BC respectively. 

Various methods of sericulture are used for the production of silk from silkworm. Modern method of sericulture involves use of modern rotary mountage or chandrike, specific rearing house, silkworm hybrid etc. while traditional method involves collecting cocoons of silkworm on circular bamboo frame. Here we are illustrating method of sericulture by following six steps – 

Step 1. Raising silkworms and harvesting cocoons 

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Female silkworm lays eggs on the leaf of mulberry tree. Eggs hatch about 10 days after they are laid. As the eggs hatch, they form worm like larvae. This stage of the silkworm’s lifecycle lasts for about 24-33 days. At an age of between 20 and 33 days, the appearance of the silkworm will change and it will turn yellowish and translucent. This indicates that they are ready to build a net of silk around them which is actually a liquid protein secreted from the head of silk moth or caterpillar. This silk is used as an anchor from which the worm swings back and forth to draw a long continuous fibre and build the cocoon. The fibre can be as long as 1 kilometre. Silkworms can take up to 48 hours to build a complete cocoon. At this stage silkworms are transferred in circular bamboo tray to get uniformly shaped cocoons and its easier to collect from this tray. 

Step 2. Silk thread extraction 

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Now these fresh cocoons are ready to take them out into reeling pot. Each cocoon consists of many yards of silk thread. It is important to preserve the length of silk thread. For this cocoons are placed in boiling water to kill chrysalis and for easy unwinding of the delicate thread. 

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Silk thread 

Step 3. Dyeing of silk 

Before dyeing threads are washed and sericin (a type of gum) is removed from the silk thread. 

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In traditional method of dyeing Silk thread, silk thread bundle is soaked in dye pots containing hot mixture of indigo leaves for several times over many days to get the perfect colour and quality. Now a day’s modern commercial methods are used for dyeing silk threads. In these methods’ synthetic indigo and other various colour are used for dyeing. 

Step 4. Spinning of silk 

After dyeing, spinning of silk thread takes place. We are using spinning wheels for this purpose from ancient times. Still spinning wheels are used for unwinding the dyed silk threads. Although many new techniques have been introduced for spinning of silk threads. 

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Step 5. Weaving of silk thread 

After spinning weaving of silk thread takes place. Weaving is converting wrap into a fabric by interlacing threads at right angles. A loom is used for this purpose. Now a day’s many types of machines are available for weaving of silk threads.  

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Step 6. Binding (ikat) of silk 

Many differing patterns are made on silk fabric and used to make sarees, shawls etc. There are many types of ikat such as wrap ikat, weft ikat, double ikat and pasapalli ikat. 

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If you want to know more about silk fibre and silkworms, then download app and get many more such articles as your ease on your mobile phone. You can register yourself at website as well to get free PDFs of NCERT Solutions of all subjects and study material. 

What is Silicon Dioxide? 

Silicon Dioxide is a natural compound of oxygen and silicon, found mostly in the sand. It is also known as Silica, composed of silicon and oxygen, having chemical formula [SiO_{2}], or silicon dioxide. There are various forms of Silica, and all silica forms are identical in chemical composition but contain different atom arrangements. 

Silica has three primary crystalline varieties, quartz, tridymite, and cristobalite. Silica dust from fine particulate quartz rock causes a long-term progressive lung injury, silicosis. ([NCIO_{4}]). The [SiO_{2}] chemical name is Silicon Dioxide.

Silica compounds are further divided into amorphous Silica (a-silica or non-crystalline Silica) and crystalline (or c-silica).

c-Silica compounds have structures with repeating patterns of both silicon and oxygen.

a-Silica chemical structures are more randomly linked to that of c-silica. 

All silica forms are odourless solids composed of silicon and oxygen atoms obtained as transparent to grey in its crystalline or amorphous powdered form. Silica particles get suspended in air and form non-explosive dust. Silica can be combined with oxides and other metallic elements for the formation of silicates.

[SiO_{2}] Structure 

Silicon dioxide is otherwise called silicon (IV) oxide.

There exist three different silicon dioxide crystal forms. The easiest one to draw and remember depends on the diamond structure.

The crystalline silicon has a similar structure as diamond. To turn it into silicon dioxide, all we are supposed to do is modify the silicon structure by adding some oxygen atoms.

The simple [SiO_{2}] structure is represented in the following way.

If we notice properly, each silicon atom is bridged to its neighbour by an oxygen atom. Remember that this is just a tiny part of a giant [SiO_{2}] structure that extends on all three dimensions.

Silicon Dioxide Properties

The basic [SiO_{2}] properties of both physical and chemical are given below.

Physical Properties of [SiO_{2}]

Silicon dioxide is transparent to grey, crystalline, odourless, or an amorphous solid. They have melting and boiling points as 1713º C and 2950º C, respectively. The density is about 2.648 g/cm3. It is insoluble in both acid and water and soluble in hydrofluoric acid. Its molecular weight is about 60.08 g/mol.

Chemical Properties of [SiO_{2}]

Silicon dioxide is not a very reactive compound because the polarity of the molecule is zero. The ‘Si’ forms two double bonds with the oxygen. Therefore, it’s a very stable molecule. Moreover, it has high dielectric strength, so that it is used as an insulator and semiconductor.

Production of Silicon Dioxide

The acidification sodium silicate solutions obtain precipitated Silica or amorphous Silica. Its gel is washed and dehydrated to make colourless microporous Silica. The reaction involving a trisilicate along with sulfuric acid is provided below.

[Na_{2}Si_{3}O_{7} + H_{2}SO_{4} rightarrow 3SiO_{2} + Na_{2}SO_{4} + H_{2}O]

Silicon Dioxide Reactions

Silica is converted into silicon by reducing carbon.

When fluorine reacts with silicon dioxide, it produces [O_{2}] and [SiF_{4}].

Silicon dioxide also reacts with hydrofluoric acid to form hexafluorosilicic acid ([H_{2}SiF_{6}]).

[SiO_{2} + 6HF rightarrow H_{2}SiF_{6} + 2H_{2}O]

Preparation of Silicon Dioxide

Most of the silicon dioxide is extracted even from quartz mining, it can also be prepared using acid neutralisation of an aqueous alkali metal – silicate solution. This kind of method is known as a wet process and forms amorphous [SiO_{2}] particles.

[Na_{2}Si_{3}O_{7} + H_{2}SO_{4} rightarrow 3SiO_{2} + Na_{2}SO_{4} + H_{2}O]

The other methods form pyrogenic Silica, having silanes combustion like silicon tetrachloride, in an oxygen-hydrogen burner. These are the fine particle product aggregates of 100 – 400 nm in diameter.

[SiCl_{4} + 2H_{2} + O_{2} rightarrow SiO_{2} + 4HCl]

Applications of Silicon Dioxide

Silica exists as fluffy, and white powders produced through a wet process, yielding a thermal route, Silica, or silica gel, yielding a pyrogenic (fumed) silica.

In powdered foods, the Silica clings to the food particles and prevents them from clumping. Doing this allows powdery products to remain free-flowing, and to separate other products easily.

Also, Silicon dioxide functions as a defoaming agent, conditioning agent, carrier, chill proofing agent in malt beverages like beer and filter aid.

Besides, it is used in material manufacture like paper and adhesives for food-packaging materials.

As per the U.S. FDA regulation’s direct additive, the SAS levels cannot exceed 2% by the food weight, and as an indirect additive, it can be used only in the required amount to produce the intended functional effect.

Silicon Dioxide Uses

There is various Silicon dioxide used in electronic, chemical, and pharmaceutical industries. In the chemical industry, it is used in the production of adhesives and sealants, adsorbents, ceramic, porcelain, corrosion inhibitors, anti-adhesives, dyes, and paint additives. In addition, silicon dioxide production occurs in agricultural chemicals. Coming to pharmaceutical industries, it helps as an additive of food and medicines to absorb water. For telecommunication, [SiO_{2}] is the main component of optical fibres. Silicon dioxide is extensively used as a precursor to obtaining glass and silicon by the reaction given below.

[SiO_{2} + 2C rightarrow Si + 2CO]

Furthermore, Silicon dioxide is also used in the construction industry to produce concrete. Used in hydraulic fracturing in its crystalline form, and in glass production, as a Sedative, production to produce elemental silicon, as an anti-caking agent in powdered foods such as spices, as a fining agent in beer, juice, and wine, in pharmaceutical tablets, and in toothpaste to remove the tooth plaque.

Health Hazards

Orally Silica is non-toxic when ingested. According to a study report conducted in 2008, the higher the rates of Silica in water, the lower the likelihood of dementia. As a result, the dosage was raised to 10 mg/day of silica in drinking water as the incidence of dementia reduced. When silica dust of finely divided crystalline is inhaled, it may lead to lung cancer, bronchitis, or silicosis, because of the lodging of dust in the lungs. Also, when fine particles of Silica are inhaled in excessive quantities, it increases the risk of lupus and rheumatoid arthritis.

Sodium Acetate is a chemical compound, comprising one Sodium (Na) atom, two oxygen (O) atoms, two carbon (C) atoms, and three hydrogens (H) atoms. It is a sodium salt of acetic acid or Sodium acetate anhydrous (i.e., lacking water of hydration) or Sodium Ethanoate. It is easily soluble in water and alcohol and is hygroscopic in nature. It is usually odourless but when heated till decomposition it smells like vinegar or acetic acid.

 

Chemical Formula: CH3COONa.

 

Uses of Sodium Acetate

• It is generally used in the textile industry.

• It is used in hot ice, heating pads, and hand warmers.

• It is used as a disinfectant.

• It is used as a buffering agent in the cosmetics industry in a variety of personal care products.

• It acts as a concrete sealant.

• It can be used as a buffer with acetic acid to keep a relatively constant pH at 881.4 °C.

• It is used as an additive in food industries, as a preservative that prevents bacteria formation in a wide range of food.

 

Properties of Sodium Acetate

 

Preparation Method

Sodium acetate can be prepared with the help of baking soda and vinegar. (It is advised to wear safety goggles as the splashing can happen and it will cause irritation in the eyes, skin, and respiratory system. If inhaled directly, it can cause inflammation of the lungs and throat).

 

Steps

• Add one spoonful of baking soda to a glass container and slowly add vinegar, being careful not to create too much foam, Keep adding vinegar while stirring the mixture.

• Once the mixture stops bubbling, you can stop adding vinegar as all of the sodium bicarbonate has been converted to sodium acetate and carbon dioxide.

• To separate out the sodium acetate from water, boil the solution until you hear a popping sound. At this point, crystals will be formed. When you get this supersaturated sodium acetate solution, cool the solution to room temperature, and a translucent gel will be formed.

• Scrape the gel into a bowl with a coffee filter, which will absorb the remaining water, Break the pieces and put them on another coffee filter to finish the drying process, creating sodium acetate powder. 

 

Reactions Involved : 

[CH_3COOH  +  NaHCO_3    rightarrow    CH_3COONa   +   H_2CO_3]

Acetic Acid     Baking Soda                Sodium Acetate   Carbonic Acid

 

[H2_CO_3                 rightarrow        H_2O  +  CO_2 ]

Carbonic Acid                   Water    Carbon Dioxide

 

Did You know?

Sodium acetate is also used as a deicer (the process of removing ice) in parking garages. The compound is preferred over Sodium chloride because sodium chloride corrodes steel rods buried in concrete and sodium acetate does not corrode. There are several other uses of sodium acetate.

 

What happens when Sodium Acetate is heated?

Answer: When Sodium acetate is heated above 58 °C, sodium acetate loses its hydration capacity and starts to dissolve in that steam. The process is exothermic in nature.

 

Note:

Acidic Buffers: It is a combination of the weak acid and its salt with a strong base (Conjugate base).

 

Eg: HCOOH / HCOONa

       CH3COOH / CH3COONa

       H2CO3  / NaHCO3

 

Basic Buffers: It is a combination of a weak base and salt with a strong acid (Conjugate acid).

 

Eg: NH3 / NH4Cl

       NH4OH / NH4Cl

 

Sodium acetate can cause mild irritation to the eyes, skin, and respiratory system. If inhaled directly, it can cause inflammation of the lungs and throat.

 

Applications of Sodium Acetate 

Sodium acetate is a compound used in various industries in the manufacturing of different products. Below are some of the applications of sodium acetate. 

Sodium acetate can be used as a carbon source to cultivate bacteria. This chemical compound also helps in increasing yields while extracting DNA by ethanol precipitation.  

Sodium acetate is a chemical compound widely used in the textile industry to remove calcium salts, which improves the quality of the finished fabric. Apart from this, it is used as a pickling agent in the production of synthetic rubber.  

Sodium acetate adds a salty flavour to different types of food items. It acts as a preservative to improve the flavour and quality of the food such as meat, poultry, etc. During food processing, sodium acetate regulates the pH level. 

Sodium acetate is used in heating pads and warmers. This compound can melt at  58.4°C dissolving in the water of crystallisation. Once the sodium acetate crystal is heated past its melting point, the aqueous solution will become supersaturated. This solution can cool down to room temperature without forming any crystals. 

Sodium acetate injections are commonly used to treat or prevent hyponatremia. In this
condition, there is a lack of sodium in the patient’s blood. With sodium acetate injection, the level of sodium in the blood can be increased and improve the patient’s condition.  

Instead of methanol, sodium acetate is used in water treatment as an environmentally-friendly compound. It can be used to prevent or lessen the damage caused by water to the concrete. 

Sodium acetate is used in the manufacturing of cosmetic products as a buffering agent to neutralise the pH levels and improve the quality of these products.  

Learn about Sodium Acetate

Learning about Sodium Acetate – Definition, Use, Preparation, and Reactions requires a lot of your time and attention. Sodium acetate is a chemical compound, which can be used for multiple purposes. For example, sodium acetate acts as a buffering agent in personal care products. To learn everything about sodium acetate, you can follow the tips mentioned below:

• You can start learning about sodium acetate from your chemistry textbook to get an idea of what this chemical compound is and how it is prepared. 

• Refer to ’s website and find the best study materials to learn the concept of sodium acetate. Here, you can learn the preparation, uses, and structure of sodium acetate and enhance your knowledge. 

• Use different reference books and guides of chemistry to gain more knowledge about sodium acetate and improve your understanding of the concept. 

• Go through the steps of preparation of sodium acetate thoroughly and also learn about the materials you need to prepare it. 

• Learn how sodium acetate reacts with other chemical compounds and is used in various industries for different purposes. 

• After learning about sodium acetate, you should start attempting questions to practice and test your knowledge to check whether you have understood the concept or not.