10 Examples of Acids

The acids are all chemical compounds that produce a pH less than 7. They are characterized by release hydrogen ions (H+) when they are dissolved in water, that is, in aqueous solution. Depending on the acid, it will be the concentration of these H+ ions that is reached in that medium, and therefore the pH value that is detected. Its chemical behavior is described in three theories called Acid-Base TheoriesWhat are they:

• Arrhenius theory
• Brönsted–Lowry theory
• Lewis theory

Arrhenius theory

According to Arrhenius, acids are all chemical species capable of release a hydrogen ion (H+) when they are dissolved in water, and thus increase the concentration of these ions, accompanying those of water (H2O), separated into hydrogen H+ and hydroxyl OH–. The pH of the solution can be measured with litmus paper, the color of which after immersion will indicate the value.

Brönsted–Lowry theory

According to Brönsted and Lowry, acids are the substances capable of giving up protons in a chemical reaction. A proton is practically the same as a hydrogen ion H+. This theory is also called Proton exchange theory. Although it may seem identical to the Arrhenius Theory, it is distinguished by the fact that it also covers ammonia NH3, for example.

Ammonia does not have a hydracid, oxyacid, or organic acid chemical structure. chemically it is amphoteric, that is, it behaves as both an acid and a base. It can donate protons to form amines, or receive them to form the ammonium ion NH4+, which later joins the hydroxyl of water (OH–) and forms ammonium hydroxide NH4OH.

Lewis theory

According to Lewis, it is called acid Any substance capable of receiving electrons during a chemical reaction. In other words, it is the substance that is reducedand that by his action oxidizes others. Your participation will be responsible for reducing the pH to values ​​below 7. It does not necessarily have to have a molecule of hydracid, oxyacid or organic acid.

types of acids

Acids are classified according to their nature into inorganic and organic, but it is within these broad categories that the three types are located, remaining as follows:

• Inorganic acids: hydracids, oxyacids.
• Organic acids: carboxylic acids.

Hydracids

Hydrocids are ionic compounds formed by hydrogen (H+) and an anion which can belong to the oxygen family or to the halogens. Are the most reactive and they attack metals to form their binary salts, releasing H2 hydrogen gas into the environment. This phenomenon is a kind of corrosionwhich degrades metals and renders them useless for mechanical purposes.

Some examples of hydrocids are:

• HF hydrofluoric acid
• HCl hydrochloric acid
• Hydrobromic acid HBr
• Hydrogen sulfide H2S
• Selenhydric acid H2Se
• Hydrocyanic acid HCN

oxyacids

Oxyacids are ionic compounds formed by hydrogen (H+) and an anion formed by a nonmetal and oxygen, also called radical. They are slightly less reactive than the hydrocids, and when they come into contact with metals, they aggressively attack them to form an oxysalt and release hydrogen H2 gas into the environment. It is the same mechanism as with the previous ones.

Some examples of oxyacids are:

• Nitric acid HNO3
• Perchloric acid HClO4
• Carbonic acid H2CO3
• sulfuric acid H2SO4
• Boric acid H3BO3
• Phosphoric acid H3PO4

Carboxylic acids

Carboxylic acids are organic compounds formed by a hydrocarbon chain (with C–C and C–H covalent bonds) and a carboxyl group (–COOH). They are much less reactive than the other types of acid, and they do not reduce the pH too much, staying at values ​​between 6 and 5. They dissociate in water with a considerably slower speed.

Some examples of carboxylic acids are:

• Formic acid HCOOH
• Acetic acid CH3COOH
• Propionic acid CH3CH2COOH
• Butyric acid CH3CH2CH2COOH
• Pentanoic acid CH3CH2CH2CH2COOH
• Hexanoic acid CH3CH2CH2CH2CH2COOH

Characteristics of acids

All substances referred to as acid are distinguished by the following characteristics:

• They chemically attack metals producing salts and hydrogen gas H2.
• They dissociate in water, releasing H+ hydrogen ions.
• They generate a pH less than 7 in aqueous solution.
• They chemically counteract the bases, producing a neutralization reaction between them. The products are water and a salt.
• They can be in a gaseous or liquid state.

most important acids

1. Nitric Acid HNO3:It is a liquid compound that is obtained from the mixture of nitrogen peroxide and water, thus obtaining a highly toxic and corrosive acid mixture.
2. Hydrochloric Acid or Muriatic HCL: It is highly corrosive, it is used industrially and the digestive system also produces it for the degradation of food, it is a liquid solution of hydrogen chloride.
3. Phosphoric Acid H3PO3: It is usually obtained from carbon dioxide, and is involved in various metabolic functions.
4. Citric Acid C6H😯7:It is an organic acid that is involved in various metabolic functions and is abundant in various foods of plant origin (especially citrus fruits), from which the body can acquire it when eating.
5. Sulfuric Acid H2SO4:It is highly corrosive, which is why it is widely used in industry and in tasks such as unclogging drains, as well as for the synthesis of other acids, and in the refining processes of various metals.
6. Boric Acid H3BO3: Boric acid arises after the reaction of sodium tetrabirate decahydrate, with an inorganic acid (commonly with hydrochloric acid). It is often used as an insecticide, antiseptic and for food preservation.
7. Acetyl Salicylic Acid C8H6O4:It is one of the acids that have clinical functions, acetylsalicylic acid is aspirin, it is used to treat pain, fever and for other medical uses.
8. Acetic Acid C2H4O2: It is the one that is formed when the fermentation of the sugars that formed alcohol is too much, acetic acid is vinegar and has a sour taste.
9. Lactic Acid C3H6O3:It is one of the organic acids that the body itself produces, for example after making physical efforts after the processes of metabolizing carbohydrates, since this acid is also found in substances such as milk (hence the name).
10. Benzoic Acid C6H5-COOH:It is used for food preservation, perfumery, and other industrial uses. It usually occurs in a solid state in the form of salts, since its dissolution in water is very slight (unless it is hot, when its solubility increases).

More than 40 examples of acids

Examples of hydrocids

1. HF hydrofluoric acid
2. HCl hydrochloric acid
3. Hydrobromic acid HBr
4. Hydroiodic acid HI
5. Hydrogen sulfide H2S
6. Selenhydric acid H2Se
7. Hydrotelluric acid H2Te
8. Hydrocyanic acid HCN

Examples of oxyacids

1. Nitric acid HNO3
2. Hypochlorous acid HClO
3. Chlorous acid HClO2
4. Chloric acid HClO3
5. Perchloric acid HClO4
6. Carbonic acid H2CO3
7. sulfurous acid H2SO3
8. sulfuric acid H2SO4
9. Boric acid H3BO3
10. Phosphorous acid H3PO3
11. Phosphoric acid H3PO4
12. permanganic acid HMnO4
13. Hypobromous acid HBrO
14. bromous acid HBrO2
15. Bromic acid HBrO3
16. Perbromic acid HBrO4
17. Hypoiodous acid HIO
18. Iodous acid HIO2
19. Iodic acid HIO3
20. periodic acid HIO4

Examples of organic acids

1. Formic acid HCOOH
2. Acetic acid CH3COOH
3. Propionic acid CH3CH2COOH
4. Butyric acid CH3CH2CH2COOH
5. Pentanoic acid CH3CH2CH2CH2COOH
6. Hexanoic acid CH3CH2CH2CH2CH2COOH
7. Heptanoic acid CH3CH2CH2CH2CH2CH2COOH
8. Octanoic acid CH3CH2CH2CH2CH2CH2CH2COOH
9. Nonanoic acid CH3CH2CH2CH2CH2CH2CH2CH2COOH
10. Decanoic acid CH3CH2CH2CH2CH2CH2CH2CH2CH2COOH
11. Undecanoic acid CH3(CH2)9COOH
12. Dodecanoic acid CH3(CH2)10COOH
13. Tridecanoic acid CH3(CH2)11COOH
14. Tetradecanoic acid CH3(CH2)12COOH
15. Pentadecanoic acid CH3(CH2)13COOH
16. Hexadecanoic acid CH3(CH2)14COOH
17. Heptadecanoic acid CH3(CH2)15COOH
18. Octadecanoic acid CH3(CH2)16COOH
19. Nonadecanoic acid CH3(CH2)17COOH
20. Eicosanoic acid CH3(CH2)18COOH

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