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A neutralization reaction is a type of double replacement reaction. A neutralization reaction occurs when an acid reacts with an equal amount of a base. This reaction usually produces a salt. One example, hydrochloric acid reacts with disodium iron tetracarbonyl to produce the iron dihydride: 2 HCl + Na 2 Fe(CO) 4 → 2 NaCl + H 2 Fe(CO) 4
Animation of a strong acid–strong base neutralization titration (using phenolphthalein).The equivalence point is marked in red. In chemistry, neutralization or neutralisation (see spelling differences) is a chemical reaction in which acid and a base react with an equivalent quantity of each other.
Alkalimetry and acidimetry are types of volumetric analyses in which the fundamental reaction is a neutralization reaction. They involve the controlled addition of either an acid or a base (titrant) of known concentration to the solution of the unknown concentration (titrate) until the reaction reaches its stoichiometric equivalence point.
Although this is a reaction solely of the dissociated ions in solution, it is sometimes referred to as a double displacement reaction: [1] Pb(NO 3) 2 + 2 KI → 2 KNO 3 + PbI 2. At higher temperature, this substance easily re-dissolves by dissociation to its colorless ions. The actual change (net ionic equation) is thus:
In neutralization reactions, basic oxides reacts with an acid to form salt and water: Magnesium oxide reacts with hydrogen chloride (acid) to produce magnesium chloride (salt) and water: MgO + 2 HCl → MgCl 2 + H 2 O; Sodium oxide reacts with hydrogen chloride (acid) to produce sodium chloride (salt) and water: Na 2 O + 2 HCl → 2 NaCl + H 2 O
Reaction with carbon dioxide gives barium carbonate. Its aqueous solution, being highly alkaline, undergoes neutralization reactions with acids. It is especially useful on reactions that require the titrations of weak organic acids. Thus, it forms barium sulfate and barium phosphate with sulfuric and phosphoric acids, respectively.
In general, the reaction is exothermic, but, e.g., the formation of mercuric oxide (HgO) is endothermic. The charge of the resulting ions is a major factor in the strength of ionic bonding, e.g. a salt C + A − is held together by electrostatic forces roughly four times weaker than C 2+ A 2− according to Coulomb's law , where C and A ...
This continues until the equivalence point is reached, at which one obtains a solution of sodium chloride, NaCl. If more base is added, an increase in conductivity or conductance is observed, since more ions Na + and OH − are being added and the neutralization reaction no longer removes an appreciable amount of H +. Consequently, in the ...