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WorksheetsCeutics Exam 2 - Ionic Equilibria Pavuluri
Total questions: 78
Worksheet time: 39mins
Name
Class
Date
1.
The physiochemical properties of a drug does not depend on a drug's molecular structure
a)
true
b)
false
2.
Physiochemical properties influence the drug's physical, chemical, and biological performance
a)
true
b)
false
3.
Ionization is a process by which an inorganic or organic compound dissociates into two or more ions when dissolved in aqueous solvent
a)
true
b)
false
4.
Ionization does not play an important role in the physiochemical property of a drug
a)
true
b)
false
5.
What is the most acidic part of the body
a)
stomach
b)
duodenum
c)
jejunum & ileum
d)
plasma
e)
colon
6.
What part of the GI has the longest transit time for ingested items
a)
stomach
b)
duodenum
c)
jejunum & ileum
d)
plasma
e)
colon
7.
In the ionized form, aqueous solubility
a)
increases
b)
decreases
c)
remains unchanged
8.
In the unionized form, aqueous solubility
a)
increases
b)
decreases
c)
remains unchanged
9.
In the ionized form, lipid solubility
a)
increases
b)
decreases
c)
remains unchanged
10.
In the unionized form, lipid solubility
a)
increases
b)
decreases
c)
remains unchanged
11.
In the ionized form, the passage of drugs through a lipid membrane (permeability)
a)
increases
b)
decreases
c)
remains unchanged
d)
non-permeable
12.
In the unionized form, the passage of drugs through a lipid membrane (permeability)
a)
increases
b)
decreases
c)
remains unchanged
d)
non-permeable
13.
Most drugs are
a)
strong acids
b)
strong bases
c)
weak electrolytes
d)
unionized
e)
neutral
14.
Extent of ionization depends on the ___ and the ___ of the surrounding environment
a)
strength of ionizable functional group
b)
pH
c)
strength of bonds
d)
pOH
e)
size of neutral functional groups
15.
Properties of ionized form a drug are dramatically different from the unionized form
a)
true
b)
false
16.
pH of body fluids range from
a)
1 to 14
b)
1 to 10
c)
1 to 8
d)
3 to 10
e)
3 to 8
17.
What is a substance that is dissolved in a solvent
a)
solute
b)
electrolyte
c)
non-electrolyte
18.
What are substances that ionize to positive ions and negative ions in aqueous solution
a)
solute
b)
electrolyte
c)
non-electrolyte
19.
Electrolytes in aq solution exhibit properties such as
a)
anomalous colligative properties when compared with non-electrolytes
b)
conduct electricity
c)
show rapid chemical reactions when compared to non-electrolytes
d)
do not ionize
e)
do not conduct an electric current
20.
Which substance can completely ionize in aq solution
a)
strong electrolytes
b)
weak electrolytes
21.
Which substance can only partially ionize in aq solution at most concentrations and ionize completely at infinite dilutions
a)
strong electrolytes
b)
weak electrolytes
22.
Which electrolyte type's ionization is pH independent
a)
strong electrolytes
b)
weak electrolytes
23.
Which electrolyte type's ionization is pH dependent
a)
strong electrolytes
b)
weak electrolytes
24.
What solvents are capable of accepting protons from the solute
a)
protophilic solvents
b)
protogenic solvents
c)
amphiprotic solvents
d)
aprotic solvents
25.
What solvents are proton donating compounds
a)
protophilic solvents
b)
protogenic solvents
c)
amphiprotic solvents
d)
aprotic solvents
26.
What solvents act as both proton acceptors and proton donors
a)
protophilic solvents
b)
protogenic solvents
c)
amphiprotic solvents
d)
aprotic solvents
27.
What solvents do not accept or donate protons and are neutral
a)
protophilic solvents
b)
protogenic solvents
c)
amphiprotic solvents
d)
aprotic solvents
28.
Substances that do not contain hydrogen cannot be classified as acids and bases
a)
true
b)
false
29.
Acids are
a)
proton donors
b)
proton acceptors
30.
Bases are
a)
proton donors
b)
proton acceptors
31.
Weak acids are
a)
unionized
b)
undissociated
c)
ionized
d)
dissociated
32.
Conjugate bases are
a)
unionized
b)
undissociated
c)
ionized
d)
dissociated
33.
Weak bases are
a)
unionized
b)
undissociated
c)
ionized
d)
dissociated
34.
Conjugate acids are
a)
unionized
b)
undissociated
c)
ionized
d)
dissociated
35.
Glibenclamide is an antidiabetic drug that is a weak acidic drug with a pKa of 6.8. Which form of the conjugate acid-base pair of Glibenclamide is charged?
a)
conjugate-acid form
b)
conjugate-base form
c)
unionized form
d)
free form
36.
Glibenclamide is an antidiabetic drug that is a weak acidic drug with a pKa of 6.8. What charge would the ionized form be
a)
positive
b)
negative
37.
The stronger the acid<br />
a)
the weaker its conjugate base
b)
the weaker its conjugate acid
38.
The stronger the base<br />
a)
the weaker its conjugate base
b)
the weaker its conjugate acid
39.
Water can act as a acid or a base
a)
true
b)
false
40.
According to the law of mass action, the rate of reaction is directly
a)
proportional to the concentration of reactants
b)
unrelated to the concentration of reactants
c)
proportional to the products
d)
unrelated to the concentration of reactants
41.
Kw =
a)
[H+][OH-]
b)
[H+]
c)
[OH-]
d)
[H+]^2 * [OH]
42.
Kw =
a)
10^-7
b)
10^-14
c)
7
d)
14
e)
-14
43.
pKw =
a)
10^-7
b)
10^-14
c)
7
d)
14
e)
-14
44.
pH =
a)
-log[OH-]
b)
-log[H+]
c)
10^[H+]
d)
10^[OH-]
45.
[H+] =
a)
-log[pOH]
b)
-log[pH]
c)
10^-pH
d)
10^-pOH
46.
When pH decreases
a)
hydrogen ion concentration increases
b)
hydroxyl ion concentration increases
47.
pKw =
a)
pH + pOH
b)
pH^2
c)
pKa + pKb
d)
14
e)
7
48.
What are some characteristics of the ionization of electrolytes for strong acids and bases
a)
ionize completely in aq solution
b)
is pH independent
c)
reverse reactions occur to a very small extent in concentrated solution
d)
equilibrium always shifts completely to the right in dilute solutions
e)
conjugates are weak
49.
What are some characteristics of the ionization of electrolytes for weak acids and bases
a)
partially ionized at some pH
b)
extent of ionization is pH dependent
c)
equilibrium shifts to the left
d)
weak acids and bases have weak tendancy to ionize
e)
conjugates are stronger
50.
What is Ka
a)
ionization constant of the weak acid
b)
acidic dissociation constant
c)
acidity constant
d)
ionization of the weak base
e)
basic dissociation constant
51.
Ka =
a)
([H+][A-]) / [HA]
b)
[HA] / ([H+][A-])
c)
([H+] + [A-]) / [HA]
d)
[HA] / ([H+] + [A-])
52.
pKa =
a)
-log(Ka)
b)
-log(H+)
c)
-log(Kw)
d)
-log(OH-)
53.
The higher the Ka, the lower the pKa of a compound
a)
the stronger the weak acid
b)
the stronger the weak base
c)
the weaker the weak acid<br />
d)
the weaker the weak base<br />
54.
What is the equation for calculating the pH of a weak acid or the pH of the salt of a weak base and strong acid
a)
pH = 1/2pKa - 1/2log[C]
b)
pH = pKa + log([Salt] / [Acid])
c)
pH = pKa + log([ionized] / [unionized])
d)
pH = 1/2pKw + 1/2pKa + 1/2log[C]
e)
pH = pKa + log([Base] / [Salt])
55.
What is the Henderson Hasselbach equation for weak acid and acid buffer (conjugate base)
a)
pH = 1/2pKa - 1/2log[C]
b)
pH = pKa + log([Salt] / [Acid])
c)
pH = pKa + log([ionized] / [unionized])
d)
pH = 1/2pKw + 1/2pKa + 1/2log[C]
e)
pH = pKa + log([Base] / [Salt])
56.
Kb =
a)
([BH+][OH-]) / [B]
b)
[B] / ([BH+][OH=])
c)
([BH+] + [OH-]) / [B]
d)
[B] / ([BH+] + [OH-])
57.
pKb =
a)
-log(Kb)
b)
-log(H+)
c)
-log(Kw)
d)
-log(OH-)
58.
The higher the Kb, the lower the pKb of a compound
a)
the stronger the weak acid
b)
the stronger the weak base
59.
The higher the Ka
a)
the lower the pKa
b)
the higher the pKa
c)
the stronger the acid<br />
d)
the weaker the acid<br />
60.
The higher the Kb
a)
the lower the pKb
b)
the higher the pKb
c)
the stronger the base<br />
d)
the weaker the base
61.
What is the equation for calculating the pH of a weak base or salt of weak acid and strong base
a)
pH = 1/2pKa - 1/2log[C]
b)
pH = pKa + log([Salt] / [Acid])
c)
pH = pKa + log([ionized] / [unionized])
d)
pH = 1/2pKw + 1/2pKa + 1/2log[C]
e)
pH = pKa + log([Base] / [Salt])
62.
What is the Henderson Hasselbach equation for weak base and basic buffer (conjugate acid)
a)
pH = 1/2pKa - 1/2log[C]
b)
pH = pKa + log([Salt] / [Acid])
c)
pH = pKa + log([unionized] / [ionized])
d)
pH = 1/2pKw + 1/2pKa + 1/2log[C]
e)
pH = pKa + log([Base] / [Salt])
63.
What type or reaction creates a salt
a)
combustion reaction
b)
acid base reaction
c)
single displacement reaction
d)
neutralization reaction
64.
When a salt is added to water, the solution can be
a)
acidic
b)
neutral
c)
alkaline
65.
What are the different kinds of salt
a)
strong acid + strong base
b)
strong acid + weak base
c)
weak acid + strong base
d)
weak acid + weak base
66.
What are characteristics of salts of strong acid and strong base
a)
they do not undergo hydrolysis
b)
H+ and OH- ions remain unchanged in the solution
c)
hydrolyzes to a greater extent than the other three classes of salts
d)
pH of the solution depends on the strength of the acid and base
e)
if the strength of the acid and base is the same, the solution is neutral
67.
What are characteristics of salts of weak acid and weak base
a)
they do not undergo hydrolysis
b)
H+ and OH- ions remain unchanged in the solution
c)
hydrolyzes to a greater extent than the other three classes of salts
d)
pH of the solution depends on the strength of the acid and base
e)
if the strength of the acid and base is the same, the solution is neutral
68.
What are characteristics of salts of strong acid and weak base
a)
have an acidic pH in water
b)
salt is completely ionized in aq solution
c)
have an alkaline pH in water
d)
do not undergo hydrolysis
e)
hydrolyzes to a greater extent than the other three classes of salts
69.
What are characteristics of salts of weak acid and strong base
a)
have an acidic pH in water
b)
salt is completely ionized in aq solution
c)
have an alkaline pH in water
d)
do not undergo hydrolysis
e)
hydrolyzes to a greater extent than the other three classes of salts
70.
If you take a salt of a strong acid + weak base, which equation would you use to find pH and what would the pH be
a)
pH = 1/2pKa - 1/2log[C]
b)
acidic pH
c)
basic pH
d)
pH = 1/2pKw + 1/2pKa + 1/2log[C]
e)
neutral pH
71.
If you take a salt of a strong base + weak acid, which equation would you use to find pH and what would the pH be
a)
pH = 1/2pKa - 1/2log[C]
b)
acidic pH
c)
basic pH
d)
pH = 1/2pKw + 1/2pKa + 1/2log[C]
e)
neutral pH
72.
What are some examples of strong acid + weak base salts
a)
HCl
b)
Iodide
c)
Sulfate
d)
Phosphate
e)
Na
73.
What are some examples of strong base + weak acids
a)
Na
b)
K
c)
Mg
d)
Iodide
e)
Sulfate
74.
Weak acids is more ionized or more soluble in aq solvents when pH is ___ than its pKa
a)
higher
b)
lower
c)
equal
75.
Weak base is more ionized or more soluble in aq solvents when pH is ___ than its pKa
a)
higher
b)
lower
c)
equal
76.
Small changes in pH (within 2 units) near pKa results in ____ changes in % ionized and unionized
a)
large
b)
small
c)
non-existent
77.
Weak acid is almost completely ionized when pH is __ units higher than its pKa
a)
1
b)
2
c)
3
d)
4
78.
Weak base is almost completely ionized when pH is __ units lower than its pKa
a)
1
b)
2
c)
3
d)
4
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