Chemical Equilibrium

Question 1

delta G is negative or K >1

Answer 1

reaction is spontaneous

Question 2

Le Châtelier’s Principal

Answer 2

Equilibrium is re-established

Question 2

Q > K

Answer 2

reaction goes to the reactants

Question 3

Complex Ions

Answer 3

Useful in separations
– Complexed metals become
more organic soluble

Question 4

Brønsted-Lowry Acids

Answer 4

proton donor

Question 5

Brønsted-Lowry Bases

Answer 5

proton acceptor

Question 6

Autoprotolysis

Answer 6

refers to proton transfer in
protic solvents like water:
H2O(l) ↔ H+ + OH-

Question 7

Strong acids: HCl, HNO3, H2SO4

Answer 7

completely dissociate in
water (except under higher concentrations)
HX(aq) → H+ + X- (no HX(aq) exists)

Question 8

Weak Acids

Answer 8

Most have H that can dissociate
HX(aq) ↔ H+ + X- (HX(aq) exists)
Example: HNO2 ↔ H+ + NO2-

Question 9

Strong Bases

Answer 9

completely dissociate to give OH-
in water
– Examples: KOH(s) → K+ + OH- (No KOH(aq))
Ca(OH)2 (s) → Ca2+ + 2OH-

Question 10

Weak Bases

Answer 10

react partially in water to give OH
- NH3(aq) + H2O(l) ↔ NH4+ + OH-
- strength of weak base given by Kb for above reaction

Question 11

Ionic Compounds in Water

Answer 11

anions usually only react as bases
- cations may react as acids

Question 12

Polyprotic Acids

Answer 12

Release more than 1 H+ per molecule
Examples: H2SO4, H3PO4, H2C2O