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IB Chem Acids SL

QuestionAnswer
Arrhenius acid Release H+ ions
Bronsted Lowry acid H+ donor
Amphoteric can act as either an acid or a base
Amphiprotic a type of amphoteric substance that specifically can act as either an acid or base by accepting or donating hydrogen ions
Acid + base --> salt + water
Acid + metal --> salt + hydrogen
Acid + metal carbonate --> salt + water + carbon dioxide
Strong acids and bases completely dissociate (split up) into ions in aqueous solution
Weak acids and bases partially dissociate into ions in aqueous solution
Acid + metal oxide --> salt + water
Hydronium ion H3O+
Arrhenius base Release OH- ions
Bronsted Lowry base H+ acceptor
Conjugate acid base pair 2 chemical species with one proton difference
Hydrogen ion concentration and pH conversion formula [H+] = 10^-pH
Conversion between pH and pOH (one not in data booklet) pKw = 14 = pH + pOH
Equivalence point The stoichiometric point - volume where the solution has been neutralised.
End point The pH where the indicator colour change is detectable to the human eye.
Created by: andrewweng0406
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