1. KEY
GENERAL CHEMISTRY-II (1412)
S.I. # 19
1. Bronsted Lowry Acids and Bases
(a) Define a Bronsted Lowry acid.
(b) Define a Bronsted Lowry base.
B.L Acid = proton donor
B.L. Base = proton acceptor
2. Define conjugate acids and bases.
Conjugate acids are formed by adding a proton to the base
Conjugate bases are formed by removing a proton from the acid
3. Give the conjugate base of the following Bronsted Lowry acids:
a) HIO3 IO3-
b) NH4+ NH3
c) H2PO4- HPO42-
d) HC7H5O2 C7H5O2-
4. Give the conjugate acids of the following Bronsted Lowry bases:
a) CN- HCN
b) O2- OH-
c) HPO42- H2PO4-
d) C2H5NH2 C2H5NH3+
5. Designate the Bronsted-Lowry acid and base on the left sie of each equation and
also designate the conjugate acid and base on the right side.
a) HBrO (aq) + H2O (l) H3O+ (aq) + BrO-(aq)
BL acid BL base C.acid C.base
b) HSO4-(aq) + HCO3- (aq) SO42- (aq) + H2CO3 (aq)
BL acid BL base C.base C.acid
c) HSO3- (aq) + H3O+ (aq) H2SO3 (aq) + H2O (l)
BL base BL acid C.acid C.base
2. KEY
6. The stronger an acid, the __weaker_ is its __conjugate_-__base__
The stronger a base, the ___weaker__ is its ___conjugate__-___acid __
See Figure 16.4 for relative strengths of some conjugate acid-base pairs.
7. a) If the base in the forward reaction is a stronger base than the conjugate base,
the equilibrium will:
lie to the right or favor the side with the conjugate base
b) If the conjugate base of the forward reaction is a stronger base than the base,
the equilibrium will:
lie to the left or favor the side with the weak base
c) what is the rule for determining the which direction the equilibrium reaction
favors?
In every acid-base reaction the position of the equilibrium favors transfer
of the proton to the stronger base. Or the position of the equilibrium favors the reaction
of the stronger acid and the stronger base to form the weaker acid and the weaker base.
8. a) Write the auto ionization process for water
b) Write the-ion product constant for water
a) H-O-H + H-O-H [ H-O-H ]+ + OH-
|
H
Or H2O(l) H+ (aq) + OH- (aq)
b) Kw = [H3O+][OH-] = [H+][OH-] = 1.0x10-14 (at 25°C)
![KEY
6. The stronger an acid, the __weaker_ is its __conjugate_-__base__
The stronger a base, the ___weaker__ is its ___conjugate__-___acid __
See Figure 16.4 for relative strengths of some conjugate acid-base pairs.
7. a) If the base in the forward reaction is a stronger base than the conjugate base,
the equilibrium will:
lie to the right or favor the side with the conjugate base
b) If the conjugate base of the forward reaction is a stronger base than the base,
the equilibrium will:
lie to the left or favor the side with the weak base
c) what is the rule for determining the which direction the equilibrium reaction
favors?
In every acid-base reaction the position of the equilibrium favors transfer
of the proton to the stronger base. Or the position of the equilibrium favors the reaction
of the stronger acid and the stronger base to form the weaker acid and the weaker base.
8. a) Write the auto ionization process for water
b) Write the-ion product constant for water
a) H-O-H + H-O-H [ H-O-H ]+ + OH-
|
H
Or H2O(l) H+ (aq) + OH- (aq)
b) Kw = [H3O+][OH-] = [H+][OH-] = 1.0x10-14 (at 25°C)](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)