Difference between Strong and weak Acids and Bases

Strong Acids:

Strong acids are substances that completely dissociate (100%ionize) in water, meaning they release all their hydrogen ions (H^+) into the solution.

This results in a high concentration of H^+ ions and a very low pH.

Examples:

 * Hydrochloric acid (HCl) - found in stomach acid

 * Sulfuric acid (H2SO4) - used in car batteries and industrial processes

 * Nitric acid (HNO3) - used in the production of fertilizers and explosives

 * Hydrobromic acid (HBr)

 * Hydroiodic acid (HI)

 * Perchloric acid (HClO_4)

 * Chloric acid (HClO_3)

Weak Acids:

Weak acids are substances that only partially dissociate (below 100%ionize) in water. 

They release only a small fraction of their hydrogen ions (H^+) into the solution, establishing an equilibrium between the undissociated acid molecules and their ions.

This leads to a lower concentration of H^+ ions and a higher pH compared to strong acids of the same concentration.

Examples:

 * Acetic acid (CH_3COOH) - the main component of vinegar

 * Citric acid (C_6H_8O_7)

 * Carbonic acid (H2CO3)

 * Hydrofluoric acid (HF)

 * Phosphoric acid (H3PO4)

 * Formic acid (HCOOH)

 * Nitrous acid (HNO2)

 * Sulfurous acid (H2SO3)

Strong Bases:

Definition: A strong base is a base that completely dissociates or ionizes in water to produce a large amount of hydroxide ions (OH^-). This means that virtually all of the base molecules break apart into their constituent ions when dissolved in water. They are strong electrolytes.

Characteristics:

 * They fully ionize in solution.

 * They have a high concentration of OH^- ions in solution.

 * They react completely with water, deprotonating it to the fullest extent possible.

Examples:

Most strong bases are the hydroxides of Group 1 (alkali metals) and Group 2 (alkaline earth metals) elements.

 * Lithium hydroxide (LiOH)

 * Sodium hydroxide (NaOH) - commonly known as caustic soda

 * Potassium hydroxide (KOH) - commonly known as caustic potash

 * Rubidium hydroxide (RbOH)

 * Cesium hydroxide (CsOH)

 * Calcium hydroxide (Ca(OH)_2) - also known as slaked lime (though its solubility is lower than Group 1 hydroxides, what does dissolve still fully ionizes)

 * Strontium hydroxide (Sr(OH)_2)

 * Barium hydroxide (Ba(OH)_2)

Weak Bases:

Definition: A weak base is a base that only partially dissociates or ionizes in water, producing a relatively small amount of hydroxide ions (OH^-). When a weak base is dissolved in water, an equilibrium is established between the undissociated base molecules and their ions. They are weak electrolytes.

Characteristics:

 * They only partially ionize in solution.

 * They produce a small concentration of OH^- ions in solution.

 * The reaction with water is reversible, and the equilibrium lies predominantly towards the undissociated base.

Examples:

Many weak bases are molecular compounds that react with water to accept a proton, forming hydroxide ions.

 * Ammonia (NH_3) 

 * Methylamine (CH_3NH_2)

 * Aniline (C_6H_5NH_2)

 * Pyridine (C_5H_5N)

 * Trimethylamine (N(CH_3)_3)

 * Aluminum hydroxide (Al(OH)_3)

 * Lead hydroxide (Pb(OH)_2)

 * Copper hydroxide (Cu(OH)_2)

 * Zinc hydroxide (Zn(OH)_2)