Acids And Bases Flashcards
Arrhenius’ definition of an acid
A substance that dissociates in water to produce hydrogen ions
Arrhenius’ definition of a strong acid
A substance that almost completely dissociates in water to produce hydrogen ions
Arrhenius’ definition of a weak acid
A substance that only slightly dissociates in water to produce hydrogen ions
Arrhenius’ definition of a base
A substance that dissociates in water to produce s hydroxide ion
Arrhenius’ definition of a strong base
A substance that almost completely dissociates in water to produce hydroxide ions
Arrhenius’ definition of a weak base
A substance that only slightly dissociates in water to produce hydroxide ions
Monobasic
Only produces one hydrogen ion
Dibasic
Produces two hydrogen ions
Tribasic
Produces three hydrogen ions
Since hydrogen ions are bare protons ….
It makes a covalent bond or dative covalent bond
Shortcomings to Arrhenius’ definition of an acid and a base
Ammonia, benzene, methylbenzene and other solvents are not included
Not all acid-base reactions requires water
H3O+ not H+ ions exist in the solution
Brønsted-Lowry’s definition of an acid
Proton donor
Brønsted-Lowry’s definition of a base
Proton acceptor
Brønsted-Lowry’s definition of a weak acid
Poor proton donor
Brønsted-Lowry’s definition of a strong acid
Good proton donor
Brønsted-Lowry’s definition of a strong base
Good proton acceptor
Brønsted-Lowry’s definition of a weak base
Poor proton donor
Arrhenius’ vs Brønsted-Lowry’s definition theory
Linited reactions in Arrhenius’ theory (only in water)
Brønsted-Lowry theory includes gaseous reactions
Arrehius’ theory is limited to bases producing hydroxide ions
Brønsted-Lowry theory broadens the ranges of acids and bases. (More inclusive)
Arrhenius’ theory never considers hydronium ions
Conjugating from acid to base
Remove H
Removd proton or + a minus sign
Conjugate base to acid
+ H
Include a +
