Definition Of Classification Of Acids And Bases
Acids and bases can be classified as organic and inorganic
More About Classification of Acids and Bases
- Some of the more common organic acids are: citric acid, carbonic acid, hydrogen cyanide, salicylic acid, lactic acid, and tartaric acid
- Some examples of organic bases are: pyridine and ethylamine
- Some of the common inorganic acids are: hydrogen sulfide, phosphoric acid, hydrogen chloride, and sulfuric acid
- Some common inorganic bases are: sodium hydroxide, sodium carbonate, sodium bicarbonate, calcium hydroxide, and calcium carbonate
- Acids, such as hydrochloric acid, and bases, such as potassium hydroxide, that have a great tendency to dissociate in water are completely ionized in solution are called strong acids or strong bases.
- Acids, such as acetic acid, and bases, such as ammonia, that are reluctant to dissociate in water are only partially ionized in solution; they are called weak acids or weak bases
- Strong acids in solution produce a high concentration of hydrogen ions, and strong bases in solution produce a high concentration of hydroxide ions and a correspondingly low concentration of hydrogen ions
- The hydrogen ion concentration is often expressed in terms of its negative logarithm, or pH. Strong acids and strong bases make very good electrolytes
- The solutions of strong acids and bases readily conduct electricity
- Acids have Sour taste, are corrosive, change litmus from blue to red, become less acidic when combined with alkalies
- Alkalies (Bases), feel slippery, change litmus from red to blue, become less alkaline when combined with acids
- Any substance that ionizes when it dissolves in water to give the H+ ion is an acid as per Arrhenius definition
Applications:
- Any substance that ionizes when it dissolves in water to give the OH- ion is a base
- HCl → H++Cl-
- NaOH →Na++OH-
- The Arrhenius theory can only classify substances when they are dissolved in water since the definitions are based upon the dissociation of compounds in water
- It does not explain why some compounds containing hydrogen such as HCl dissolve in water to give acidic solutions and why others such as CH4 do not
- According to Lowry Bronsted concept acids are substances that donate protons and bases are substances that can accept protons
- A conjugate acid base pair differs by a proton
- An acid donates a proton and a base accepts it. The base formed from an acid by donation of a proton is called conjugate base of that acid
- Acid1 base2 acid2 base1
- According to Lewis concept an acid is a substance that can accept electron pair and a base is a substance that can donate electron pair
- Examples of Lewis acids:
