Soap:- Cleansing Agent

Soap:- Cleansing agent

Fatty acid and an alkali metal hydroxide react chemically to produce soap, a cleaning agent. A fatty acid reacts chemically with an alkali metal hydroxide such as sodium hydroxide or potassium hydroxide, to create soap, a cleaning agent. Because of its exceptional capacity to enclose oil particles, soap has the special power to disperse them in water and make them simple to rinse away. Since ancient times, soap has been used as a washing agent, a mild antibacterial, and an ingestible remedy for some poisonings. 

The general chemical formula for soap is RCOOX. The X on the periodic table of elements stands for an alkali metal, which is an element found in the first column. The R stands for a chain of hydrocarbons made up of anywhere between 8 and 22 linked carbon atoms that are encircled by hydrogen atoms. 

Features And Applications Of Soap

Soaps have good biodegradability and are great cleaning agents. The propensity of the carboxylate ion to react with Ca+ and Mg+ ions in hard water is a significant problem that limits their general use. The end result is a salt that is not water-soluble and can settle on clothing and other surfaces. Hard water plaques also cause rings in sinks and bathtubs and bleach fabric colors. The inefficiency of soaps in acidic environments is another drawback. In these situations, soap salts are inefficient as cleaning agents because they do not separate into their individual ions. Although soaps are usually used for cleaning, they also work well as ingestible antidotes for heavy metal or mineral acid poisoning as well as mild antiseptics. Polishes, inks, paints, and lubricating oils all utilize special metallic soaps as additions since they are manufactured from soap and heavier metals.

How Does Soap Work?

On our hands, soap eliminates germs rather than killing them.

The molecules of soap are uniformly distributed in a solution of soap and water. However, because the hydrocarbon ions in the soap are attracted to one another and aggregate into spheres known as micelles, this system is not a real solution. The hydrophilic heads of the molecules remain on the exterior of these micelles to interact with water, while the water-incompatible molecular tails are inside these micelles. Oil is absorbed by these micelles as tiny particles when it is added to this environment. After that, it can be rinsed off. Use soap and be thorough when washing your hands for the best results. Create a lather because, according to the Centers for Disease Control and Prevention, the friction helps remove debris and oils from your skin (CDC). Depending on how dirty your hands are, you should scrub for whatever long it takes to sing "Happy Birthday" twice, which is often at least 20 seconds, according to health experts. Don't forget to scrape between your fingernails as well. Germs love that spot; it's good real estate. After washing, make sure to towel- or air-dry your clothes. There is no established optimal procedure for drying, however, the CDC notes that moist hands are more likely to spread germs than dry ones.

In water, soap partially separates into its component ions since it is a salt. The RCOO- is the soap molecule's active ion. This ion's two ends exhibit diverse behaviors. The hydrophilic (loving water) carboxylate end (-COO-) is referred to as the "head" of the ion. The "tail" of the molecule refers to the lipophilic (oil-loving) hydrocarbon part. The distinctive surface and solubility properties of soaps and other surfactants are the results of their particular molecular structure. The molecules of soap are uniformly distributed in a solution of soap and water. However, because the hydrocarbon ions in the soap are attracted to one another and aggregate into spheres known as micelles, this system is not a real solution. The hydrophilic heads of the molecules remain on the exterior of these micelles to interact with water, while the water-incompatible molecular tails are inside these micelles. Oil is absorbed by these micelles as tiny particles when it is added to this environment. After that, it can be rinsed off.

Is soap that is antibacterial even better? 

Ingredients like triclosan or triclocarban, which are hydrophobic compounds that can penetrate bacterial cell walls and kill the bacteria, are added to antibacterial soaps. Although it may sound amazing, research has revealed that antibacterial soaps are not any more successful at eradicating bacteria than normal soaps. Antibacterial soaps were no longer permitted to be promoted to the general public after an FDA rule was announced in 2016. Consumers might believe that antibacterial washes are more efficient at halting the transmission of germs, but there is no scientific proof to support this, according to Dr. Janet Woodcock, head of the FDA's Center for Drug Evaluation and Research (CDER).

Corrosion, Rusty Iron!

One of the most common phenomena we see in our daily lives is corrosion. You've probably noticed that some iron objects are covered with an orange or reddish-brown colored layer at some point. The formation of rust on iron is perhaps the most well-known example of corrosion. When iron is exposed to oxygen and water, it rusts (oxidizes). Corrosion is commonly defined as the electrochemical degradation of metals. Corrosion can be seen in the formation of rust on iron, tarnish on silver and the blue-green patina that develops on copper. 

In general, corrosion is a process that converts refined metals into more stable compounds such as metal oxides, metal sulfides, or metal hydroxides. Similarly, iron rusting involves forming iron oxides due to the action of atmospheric moisture and oxygen. When we look at the science behind corrosion, we can say that it is a spontaneous/irreversible process in which metals transform into more stable chemical compounds such as oxides, sulfides, hydroxides, and so on. In this post, we will delve deeper into the concept of corrosion and understand its various factors such as its meaning, types, prevention, and more.

What exactly is corrosion? 

It is essentially defined as a natural process that causes pure metals to transform into undesirable substances when they react with substances such as water or air. This reaction causes metal damage and disintegration, beginning with the exposed portion of the metal and spreading to the entire bulk of the metal. Corrosion is typically an unfavorable phenomenon because it interferes with the desirable properties of the metal. Iron, for example, is known to have high tensile strength and rigidity (especially alloyed with a few other elements). Rusting, on the other hand, causes iron objects to become brittle, flaky, and structurally unsound. Corrosion, on the other hand, is a diffusion-controlled process that occurs primarily on exposed surfaces. As a result, in some cases, attempts are made to reduce the activity of the exposed surface and increase the corrosion resistance of a material. Passivation and chromate conversion are examples of processes used. Some corrosion mechanisms, on the other hand, are not always visible and are even less predictable.

Are All Metals Corrodible?

Metals higher in the reactivity series, such as iron and zinc, corrode easily, whereas metals lower in the reactivity series, such as gold, platinum, and palladium, do not corrode. The reason for this is that corrosion involves the oxidation of metals. The tendency to oxidize decreases as we move down the reactivity series.

Corrosion rate depends on:-

Metals are exposed to air containing gases such as CO2, SO2, SO3, and others increasing the chance of corrosion of metals. Metals exposed to moisture, particularly salt water have a high corrosion rate. The acid in the atmosphere: Acids can easily accelerate the corrosion process. As the temperature rises, so does corrosion. The nature of the first oxide layer formed also determines the corrosion rate: some oxides, such as Al2O3, form an insoluble protective layer that can prevent further corrosion. Others, such as rust, easily crumble and expose the remaining metal.

How could it affect our life?

Corrosion can have varying degrees of impact on a wide range of things. As a result, it primarily wastes natural resources. Furthermore, it can lead to dangerous situations such as building structures becoming weak and unstable, accidents caused by corroded parts, and other unwelcome failures such as cracked pipelines, bridge collapses, transport vehicle crashes, and other disasters. The annual global cost of metallic corrosion is estimated to be more than $2 trillion, but experts believe that proper corrosion protection could save 25 - 30% of this cost. Poorly planned construction projects can result in corroded structures that must be replaced, wasting natural resources and contradicting global sustainability concerns. Corrosion can also result in safety concerns, loss of life, additional indirect costs, and reputational damage. That's why it is critical to monitor and prevent corrosion at all costs.

Prevention:-

Corrosion is prevented by protective coatings. Metals can be protected from corrosion by applying protective coatings that act as a barrier to water and oxygen. This coating can be applied by oil greasing, painting, or electroplating with a different metal. Electroplating is accomplished through the electrolysis process. Electrolysis allows for the application of a thin layer of metal to an object. The object is at the cathode, and the plating metal is at the anode. The electrolyte is made up of plating metal ions. Aluminium oxide shields the metal. Aluminium oxide is a coating that is applied to aluminum. This oxide layer on the surface of aluminium protects the metal from further corrosion. Electroplating has a variety of applications. Metals are less likely to corrode or be damaged when they are electroplated. It also enhances the aesthetics and appearance of metals, such as silver-plated cutlery.