Notes #39 Flashcards
how were acids and bases recognized before modern analytical tool?
chemical properties
acids
-sour taste
-react w/metals to produce hydrogen gas (H2)
-react w/carbonates to produce CO2
bases
-bitter taste
-feel slippery when mixed w/H2O
-opposite of acid, causes acids to lose their acedic properties when mixed with them
describing acids and bases
Arrhenius model for ^
acid release H+ ions in solution
HCl -> H+ Cl-
bases release OH- in solution
NaOH -> Na+ + OH-
this could not explain others, like ammonia NH3+ (a base).
Bronsted Lowry acid
-explains a wide range of acids and bases
-acids are protons (H+ ions) donors
-bases are protons acceptors
1) conjugate acids
2) conjugate bases
1) the substance resulting from accepting the protons
(has properties of an acid)
2) the substance resulting from losing the protons
(has properties of an base)
Water is referred to _____ substance because it can act as both an ____ and ____.
Water is referred to amphoeric substance because it can act as both an acid and base.
Why is there a double arrow?
It can go both ways! 😁
Weak acids
Backward reaction is much stronger
-most weak acid does not dissociate into ions
-poor conductor of electricity
-forms a very strong conjugate base
Strong acid
Forward reaction
strong acids dissociate almost all
good conductor of electricity in
aqueous solution
Forms a very weak conjugate base
The 6’S Acids
HClO4
HCl
HBr
HI
HNO3
H2SO4
The 6’S Bees
LiOH
NaOH
KOH
CA(OH)2
Sr(OH)2
Ba(OH)2
Mostly dissociate into ions:
strong acid and strong base
Most of the compound does not dissociate:
weak acid and weak base
The conjugate acid is barely formed and mostly dissociate is:
weak base
