1. 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.
2. Define conjugate acids and bases.
3. Give the conjugate base of the following Bronsted Lowry acids:
a) HIO3
b) NH4+
c) H2PO4-
d) HC7H5O2
4. Give the conjugate acids of the following Bronsted Lowry bases:
a) CN-
b) O2-
c) HPO42-
d) C2H5NH2
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)
b) HSO4-(aq) + HCO3- (aq)  SO42- (aq) + H2CO3 (aq)
c) HSO3- (aq) + H3O+ (aq)  H2SO3 (aq) + H2O (l)

2. 6. The stronger an acid, the ____________ is its _____________-_______________
The stronger a base, the ______________ is its ________________-_________ __
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:
b) If the conjugate base of the forward reaction is a stronger base than the base,
the equilibrium will:
c) what is the rule for determining the which direction the equilibrium reaction
favors?
8. a) Write the auto ionization process for water
b) Write the-ion product constant for water