Definition Of Classification Of Acids And Bases

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: