They have a high pK a or pH value with moderate electrical conductivity property and weak electrolyte compare to strong acid.Įxamples of a weak acid – Hydrogen cyanide(HCN), Ammonium ion(NH 4 +), Phosphoric acid(H 3PO 4), HF, HCOOH, H 2CO 3, etc. The presence of water solution is a must for knowing the acidic nature of substance according to Arrhenius theory.Įxamples of strong acids: Hydrochloric acid(HCl), Sulfuric acid(H 2SO 4), Nitric acid(HNO 3), HBr, HI, etc.Īnd weak acid is a compound that partially dissociates which means not all moles of weak acid dissociate in a solution to give H + ion or they are not 100 % ionized in a solution and give only a low amount of hydrogen ions. ![]() OH –, NaOH, NH 3, H 2O, etc.īut Arrhenius’s theory said a substance is an acid when it loses the proton on dissolving in an aqueous solution. ![]() Note:- Bronsted-Lowry theory is not limited to an aqueous solution, this theory state that a substance is said to be Bronsted-Lowry acid when it donates the proton to other reacting species, the reacting species should be base or very less acidic in nature because according to this theory-Ī substance can function as an Bronsted-Lowry acid only in the presence of a base. Therefore, we can say, in the above reaction, CH 3COOH acts as Bronsted-Lowry acid because of proton donating ability, and H 2O acts as a Bronsted-Lowry base because of proton accepting ability. The final aqueous solution of CH 3COOH contains H 3O + ions and a conjugate base(CH 3COO -). ![]() As you see in the above reaction, CH 3COOH liberates or donates the one H + ion to the water molecule and itself makes a conjugate base (CH 3COO -).
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