2.What is autoionization, and how is it important for water?
3.Name the three non-covalent forces discussed in this module.
4.What type of non-covalent interaction is known as the strongest
dipole-dipole force?
5.Would the following be a hydrogen donor or acceptor? Or both?
6.How does the strength of London forces change with increasing
molecular weight? Explain briefly.
7.Calculate the pH of a solution containing 0.12 M of OH– .
8.If a solution contains 0.00023M of H+, then what is the OH –
concentration?
9.If a solution contains 1.67 x 10-8 M OH – , then what is H +
concentration?
10.A solution contains H+ at a concentration of 1.67 x 10-6 M. Is
the solution acidic, basic, or neutral? Explain briefly.
11.What is the concentration, in M, of water as a pure liquid?
12.Define Keq and K w .
13.Identify the acid, conjugate base, and proton in the following reaction.
14.A buffer system has a pKa of 8.5. What is its effective buffering range?
15.A buffer system has [H +] = 1.2 x 10 -6 , [A – ] = 1.2 x 10 -6 , and [HA] = 3.2 x
10 -5 . What is its corresponding Ka value?
16.A buffer system has [H +] = 1.2 x 10 -6 , [A – ] = 1.2 x 10 -6 , and
[HA] = 3.2 x 10 -5 . What is its corresponding Ka value?
17.Ice melts at room temperature. What is the sign for
Δ
G in this reaction?
18.Butane combusts in the air by the following reaction:
C 4 H 10 (l) + 6.5 O2 (g)
⟶
4 CO 2 (g) + 5 H 2 O (g)
What is the sign (+ or -) of
Δ
G,
Δ
H, and
Δ
S in this reaction?
19.
What is the role of ATP in helping a non-spontaneous reaction
occur?
