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acids & bases

chemistry

QuestionAnswer
Arrhenius Theory (AT) Acids An acid dissociates in water to produce H+ ions
AT Bases A bases dissociates in water to produce OH- ions
Alkali An alkali is a base that is soluble in water
Two problems with Arrhenius theory Acids ? 1. Allowed the existence of independent H+ ions, that is nit true. The H+ ions react with water to form H3O+ ( hydronium Ion) 2. Based definitions to reactions occurring in polar water, so non-polar water organic solvents were excluded
Problem with Arrhenius Theory Bases? Excluded common bases such as NH3 ( ammonia)
Monobasic acid A mono basic acid produces one H+ ion in solution e.g. HCl and HNO3
Dibasic acids A dibasic acid produces two H+ ions in solution e.g H2SO4
Tribasic Acid A tribasic acid produces three H+ ions in solution e.g H3PO4
Bronsted-Lowry Theory ( BL) ---> Acids An acid is a proton (H+) donor
(BL) Base A base is a proton (H+) acceptor
Amphoteric /Amphiprotic A substance that can act as both an acid and a base
Conjugate pairs Two species that differ by one proton (H+ ion )
Conjugate acid a base plus a H+ ion
Conjugate base An acid minus a H+ ion
dissociation When acids are placed in solutions they split up into their ions, hydrogen ions and anions
Monobasic acid will have one equation for their dissociation
Dibasic acids will have two equations for their dissociation
Tribasic Acid will have three equations for their dissociation
Created by: user-1973937
 

 



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