Importance of pH in Everyday Life: An Introduction
The pH measures how acidic/basic is a given solution. Its range is going from 0 - 14, with 7 being neutral. If the pH is less than 7 shows acidity, while a pH greater than 7 shows a base. It is actually a degree of the relative quantity of free hydrogen and hydroxyl ions within the solution. It is equal to −log10 c; where c is the hydrogen ion concentration in moles per litre. Water that has greater free hydrogen ions is acidic, while water that has greater free hydroxyl ions is basic. Since pH may be affected by chemical substances within the water, pH is an essential indicator of water which is converting chemically.
The Theory of pH & Its Discovery
The pH is stated in "logarithmic units". Each range represents a 10-fold change within the acidity/basicity of the water. Water with a pH of 5 is ten times greater acidic than water having a pH of 6. It is an essential amount that displays the chemical situation of a solution. The pH can manage the supply of nutrients, biological functions, microbial activity, and the behaviour of chemicals.
The theory of pH was first added through the Danish chemist Soren Peder Lauritz Sorensen at the Carlsberg Laboratory in 1909 and revised to the present-day pH in 1924 to deal with definitions and measurements in phrases of electrochemical cells. In the primary papers, the notation had H• as a subscript to the lowercase p, thus: pH•.
The actual meaning of the letter p in "pH" is disputed, as Sorensen did not give an explanation for why he used it. Sorensen describes a manner of measuring pH using potential differences, and it represents the negative energy of 10 within the concentration of hydrogen ions. The letter p should stand for the French puissance, German Potenz, or Danish potens, which means "power", or it can mean "potential". All the phrases for those beginning with the letter p in French, German, and Danish—all languages Sorensen posted in: Carlsberg Laboratory became French-speaking, German became the dominant language of clinical publishing, and Sorensen became Danish.
pH in Our Digestive System
The pH of our belly is vital to the digestion of many nutrients and acts like the first line of protection in opposition to harmful microorganisms and viruses. The belly is a reservoir of robust acid, with a far lower pH than in other parts of our digestive system. Gastric juice or belly acid is a digestive fluid formed within the stomach lining. It is acidic as the protein-digesting enzymes of the belly including pepsin do not work properly within the primary medium so the pH is maintained from 1.5 – 3.5 within the belly. So, the pH is usually around 2.
The stomach is pretty acidic and enables the breakdown of meals for simpler digestion. This allows your body to soak up nutrients without difficulty as food transfers via your digestive tract. In order to break down the whole thing from meat too tough, fibrous plants, belly acid needs to be more acidic.
As we recognize our belly produces gastric juice which incorporates a huge quantity of hydrochloric acid (pH approximately 1.4). The acid does not damage the stomach wall due to the protective mucus layer, however, it kills germs and microorganisms which input into our digestive system together with food, therefore in a manner it protects us from illnesses and helps in the digestion process. Sometimes more acid is produced within the belly because of overeating, consuming highly spiced meals or because of abnormal food habits. This stage is known as acidity which causes gastritis. To get comfort from this pain, one needs to take antacids. These include bases to neutralise the extra acids. Examples- Magnesium hydroxide (milk of magnesia). Mg (OH)2 or Aluminium hydroxide.
Importance of pH Scale
The pH scale is measurable to a set of standard solutions whose pH is installed through worldwide agreement. Primary pH preferred values are observed by the use of a concentration cellular with transference, by measuring the ability difference between a hydrogen electrode and a standard electrode which includes the silver chloride electrode. The pH of aqueous solutions may be measured with a glass electrode and a pH meter, or a colour-changing indicator. Measurements of pH are essential in chemistry, agronomy, medicine, water treatment, and lots of different applications.
Examples of Bases in Everyday Life
Sodium Bicarbonate - Baking Soda
Soap (A mild base)
Oven Cleaner
Drain Cleaner
Toothpaste
Bleach
Ammonia (Sometime found in hair products or cleaning products)
Washing Powder
Cement
Calcium Hydroxide - Slaked lime
A lot of cleaning products are bases.
Examples of Acids in Everyday Life
Hydrochloric Acid (HCl) Hydrochloric acid is a strong acid which is found inside our body in gastric juice.
Acetic Acid for example vinegar.
Ascorbic or Citric Acid.
Carbonic Acid.
Sulphuric Acid.
Tartaric Acid
Interesting Facts
Currently, in chemistry, the p stands for "decimal logarithm of", and is likewise used within the word pKa, used for acid dissociation constants and pOH, the same for hydroxide ions.
Any aqueous solution can be classified as an acid, base, or neutral. Oils and some other non-aqueous liquids are either acids or bases.
Combining a base with an acid neutralizes the acid.
Stomach acid stimulates the inactive enzymes secreted in the belly which helps in the chemical digestion of meals.
Key Features
The pH stands for the potential of hydrogen.
For the sign p, Sorensen recommends the name 'hydrogen ion exponent' and the image pH•. Then, for the hydrogen ion exponent (pH•) of a solution, the negative range of the Briggsian logarithm of the associated hydrogen ion normality factor is to be understood.
FAQs on Importance of pH in Everyday Life
1. What is the pH scale and what is its importance in everyday life?
The pH scale is a measure of how acidic or basic a substance is, ranging from 0 (very acidic) to 14 (very basic), with 7 being neutral. Its importance in everyday life is immense as it affects many biological and chemical processes. For example, it determines the proper functioning of our digestive system, the health of soil for agriculture, and even prevents tooth decay.
2. How does pH play a crucial role in our digestive system?
Our stomach produces hydrochloric acid (HCl), creating a highly acidic environment with a pH between 1.5 and 3.5. This low pH is crucial for two main reasons: it activates the enzyme pepsin to digest proteins and it kills most harmful bacteria and viruses that enter with food. When excess acid is produced, it leads to a condition called acidity, which is neutralised by taking antacids (mild bases).
3. What is the connection between the pH in our mouth and tooth decay?
Tooth decay begins when the pH in the mouth falls below 5.5. Bacteria present in our mouth break down sugar and leftover food particles to produce acids. This acid corrodes the tooth enamel, which is made of calcium phosphate, the hardest substance in the body. Using toothpaste, which is generally basic, helps to neutralise the excess acid and prevent tooth decay.
4. Why is it important for farmers to monitor the pH of the soil?
The pH of the soil is vital for plant health because it affects the availability of essential nutrients. Most plants thrive in soil that is close to neutral (pH 7). If the soil is too acidic or too alkaline, it can lock up nutrients, making them unavailable for the plants to absorb, leading to poor growth. Farmers test soil pH and treat it with substances like lime (calcium hydroxide) to reduce acidity or gypsum to reduce alkalinity, ensuring optimal crop yield.
5. How do some animals and plants use acids and bases for self-defence?
Many living organisms use pH for protection. For example, when a bee stings, it injects an acidic liquid (methanoic acid) into the skin, causing pain and irritation. Applying a mild base like baking soda can provide relief. Similarly, the stinging hair of the nettle plant injects methanoic acid. Traditionally, the leaf of a dock plant, which often grows nearby and is basic in nature, is rubbed on the affected area to neutralise the sting.
6. Why does our stomach not get damaged by the highly acidic hydrochloric acid it produces?
Although the hydrochloric acid in our stomach is strong enough to dissolve metals, the stomach itself is protected from harm. This is because the inner lining of the stomach secretes a thick layer of mucus. This protective mucus layer acts as a barrier, preventing the corrosive acid from coming into direct contact with and damaging the stomach walls.
7. What are some common examples of acidic and basic substances found in a typical household?
Many common household items can be classified by their pH.
- Common Acids: Vinegar (acetic acid), lemon juice (citric acid), and battery acid (sulphuric acid).
- Common Bases: Baking soda (sodium bicarbonate), soap, drain cleaner (sodium hydroxide), and toothpaste.
8. If acid rain has a pH of around 5.6, why is it considered harmful when it's only slightly acidic?
The pH scale is logarithmic, meaning each whole number change represents a tenfold change in acidity. Pure water has a neutral pH of 7. Rainwater with a pH of 5.6 is about 25 times more acidic than pure water. This slight-sounding change is significant enough to harm aquatic life by altering the pH of lakes and rivers, damage forests by leaching nutrients from the soil, and corrode buildings and statues made of limestone or marble.
