1. No category

MULTIPLE CHOICE SAMPLE TEST FOR THE SEMIFINAL EXAM
1. What is the highest possible Ag+-concentration in a solution containing 0.001 M Cl-?
(Ksp of AgCl=10-10)
A: lO-1 M
B: 10-2 M
C: 10-7 M
D: 10-5 M
E:10-3 M
2. Which of the following statement(s) is/are true?
1. Precipitation is expected to occur if the ion product is greater than the Ksp.
2. Precipitation is expected to occur if the ion product is smaller than the Ksp.
3. The solubility of an ionic compound decreases by the addition ofa soluble salt that supplies
a common ion.
4. The solubility of an ionic compound increases by the addition ofa soluble salt that supplies
a common ion.
5. The solubility of salts could be calculated from the value of the solubility product.
A: 2,4,5
B: 1,3,5
C: 2,3,5
D: 1,4,5
E:l,3
3. Select the compound(s) from the list below that decrease(s) the dissociation of
phosphoric acid, when added in 0.01 M concentration to a 0.01 M phosphoric acid
solution !
1. NaOH 2. Na2SO4
3. Na2CO3
A: 4
C:l,2
B:2,4
4. H2SO4
D:3,4
E:l,3
What is the pH of a 0.01 N acid solution whose ionization constant is 1.7 x 10-5 ?
4.
A: 1.4
B: 1.7
C: 2.0
D: 3.4
E: 4.8
5. What is the pH of a 0.1 M sulfuric acid?
A: 1
B:-l
C:0
D:0.7
E:-0.7
6. 50 ml 0.1 M phosphoric acid is titrated with 1 N NaOH. Which of the following NaOH
additions results in the formation of a buffer?
1. 2.5 ml
A: 4,5
B:5
2. 5 ml
3. 7.5 ml
4. 10 ml
C:l,3
D:2,3
E:2,4
5. 25 ml
7. What is the pH of the solution after mixing 10 ml 0.1 M H2SO4 with 10 ml 0.1 M NaOH?
A: 0.00
B: 1.00
C: 1.30
D: 1.48
E:7.00
8. Which of the following statements is not true concerning the titration of a weak base?
1. HCl is an appropriate titrating solution.
2. The titration starts at a lower pH, compared to the titration of a strong base with the same
concentration.
3. Methyl orange or methyl red are suitable indicators.
4. At partial neutralization a buffer system is formed.
5. The equivalence point is in the basic range.
A: 5
B:3
C:l
D:2
E:4
9.
1000 ml solution of each substance listed below is diluted with 1000 ml water. In
which case(s) does this dilution shift the pH of the solution?
1. 0.1 N acetic acid
2. 0.1 M acetate buffer, pH = 5,7
3. 0.1 N hydrochloric acid
4. 0.1 M sodium chloride
A: 1,3
B: 1,3,4
C:2,4
D:l,2
E:2,3,4
10. Which of the following statements is true?
A: H3PO4 is a weaker acid than H2PO4-.
B: HPO42- is a stronger base than PO43-.
C: PO43- is a weaker base than HPO42-.
D: H2PO4- is a stronger base than HPO42-.
E: HPO42- is a weaker acid than H2PO4-.
11. An 0.1 M solution of a monoprotic acid has the pH of 3.0. What is the
degree of dissociation in this solution?
A: 0.1
B: 0.2
C: 0.02
D: 0.01
E: 0.015
12. At which of the following concentrations does H3PO4 have the highest degree of
ionization?
1. 0.1N
2. 0.01 N
3. 0.001 N
4. 1 N
5. degree of ionization is independent on the H3PO4 concentration
A: 1
B: 4
C: 3
D: 2
E: 5
13. We wish to make a solution, isotonic with blood serum, by dissolving a non-dissociating
compound (Molar mass = 180) in 110 g water. How many grams do we have to dissolve?
(The freezing point of blood serum is -0.56 °C, the molal freezing point depression (Kf) of
water is 1.85°C kg/mol.)
A: 15
B: 18
C: 12
D: 9
E: 6
14. Which of the following phenomena are colligative?
1. Freezing point depression
2. Boiling point elevation
3. Electrolytic dissociation
4. Osmotic pressure
5. Ionization of water
A: 1,2,4
B:l,3,5
C:l,3,4
D:l,3
E:3,4
15. The osmotic pressure of a solution of 0.050 g horse hemoglobin in 10.0 ml water is 1.8 x
10-3 atm at 25 °C. What is the molar mass of hemoglobin? (R= 0.0821 L x atm/K x mol)
A: 3.4xl05
B:6.8xl04
C:3.4xl04
D:9.6xl05
E:6.8xl05
16. Which of the solutions below are isotonic with the human blood plasma? (Freezing point
depression of human blood plasma is 0.56°C, the molal freezing point depression (Kf) of
water is 1,85 °C/molal.)
1. 0.30 Molal NaCl solution
2. 0.15 Molal NaCl solution 3. 0.30 Molal glucose solution
4. 0.15 Molal glucose solution 5. 0.15 Molal CaCl2 solution 6. 0.10 Molal CaCl2 solution
A: 1,2
B:2,3
C:2,3,6
0:1,4,6
E:3,4,5
17. A solution process is endothermic if...
A: the sum of the lattice energy and enthalpy change of hydration is negative.
B: the enthalpy change of hydration is higher than the lattice energy.
C: the sum of the lattice energy and the enthalpy change of hydration is zero.
D: the sum of the lattice energy and the enthalpy change of hydration is positive.
E: the enthalpy change of hydration is positive.
18. The standard enthalpy of formation ( H°f) of methanol (CH3OH) is -238.6 kJ/mol.
Calculate the combustion heat of one mole of CH3OH ! The standard enthalpies of
formation of CO2 (g) and H2O(1) are -394 kJ/mol and -285.8 kJ/mol, respectively.
(Results are expressed as kJ/mol)
A:-1300
B:-976
C:-854
D:-727
E:-1142
19. The free energy change is zero in ...
1. the state of equilibrium. 2. spontaneous reactions. 3. autocatalytic reactions.
4. atomic and ionic reactions. 5. reversible reactions.
A: 1
B: 2
C: 3
D: 4
E: 5
20. Which statements are true for the following cell?
Pt | Cl2 (1 atm) | Cl- (1 M) // MnO4- (1 M) | Mn2+ (1 M) | Pt
Standard electrode potentials:
Cl2 (g) + 2 e-> 2Cl- (aq) +1.36 V
MnO4- (aq) + 8 H+ (aq) + 5 e- -> Mn2+ + 4 O2 +1.51 V
1. Permanganate ions become reduced.
2. Cloride ions become oxidized.
3. The chlorine electrode is the negative pole. 4. The standard electromotive force is 2.87 V.
A: 1,2
B:3
C:l,2,3,4
D:l,2,3
E:l,2,4
21. Select those pairs of standard electrodes which can provide a voltaic cell with 2 V
electromotive force ! Standard potentials:
Cs++e- -->Cs = -3.00V
Mn2++2e- -->Mn = - l.OOV Cu2++2e - --> Cu = + 0.34 V
Mg2++2e--->Mg = -2.34 V Ag+ + e- --> Ag = + 0.80 V
1: Cs-Mn
A: 1,2,3,4
2: Cu-Mn
B: 1,3
3. Cu-Mg
C: 1
4. Ag-Mg
D: 3,5
Pt2+ +2e- --> Pt = + 1.20 V
5. Ag-Pt
E: l,3,5
22. Which of the following five compounds is the strongest oxidizing agent under standard
conditions? Standard electrode potentials:
ClO4-(aq) + H2O(l) + 2e- --> ClO3-aq) + 2OH-(aq) +0.17 V
ClO3-(aq) + H2O(l) + 2e- --> ClO2-(aq) + 2OH-(aq) +0.35 V
ClO2-(aq) + H2O(l) + 2e- --> ClO-(aq) + 2OH-(aq)
ClO-(aq) + H2O(l) + 2e- -->
A: Cl-
B: ClO2-
Cl-(aq) + 2OH-(aq)
C: ClO3-
+0.59 V
+0.90 V
D: ClO-
E: ClO4-
23. A concentration cell is built from hydrogen electrodes:
(-) Pt | H2 (1 atm) | H2SO4 (unknown) | | HCl (10-2 N) | H2 (1 atm) | Pt (+)
The measured electromotive force is 0.12 V. What is the pH of the H2S04 solution?
A: 4
B:3
C:2
D:2.7
E:3.3
24. What is the electromotive force in a cell, consisting of two Fe /Fe redox electrodes, if the
ratio of ion concentrations is: [Fe2+]/[Fe3+ ] = 0.1 in one, and [Fe2+]/[Fe3+] = 0.01 in the other
electrode?
A: 0.6 V
B: 0.12 V
C: 1.2 V
D: 2,l V
E: 0.06V
25. The reaction A -> B + C is characterized by the following energy profile:
E
A
reaction coordinate
Which statement is true for this reaction?
A: A catalyst would not be useful.
B: The reaction occurs spontaneously.
C: The reaction is endothermic at constant pressure.
D: The reaction is reversible.
E: The reaction liberates a large quantity of heat.
26.
1/[A]
Consider the reaction: A+B —>C
The graph shows the change of 1/[A] with time.
What is the rate expression for this reaction?
time
A: v = k [A]2
B: v = k [B]
C: v = k[A]
D: v = k [A] [ B]
E: v = k[A][B]2
27. Select the pair of compounds, that are in equilibrium with each other, and do not
constitute a resonance pair!
R
1.
-
R
C=O
R
C
-
O
C=O
-
O
CH3 — CH == CH — +CH2
O-
CH3—C
O-
O
O
3. CH3 — +CH — CH = CH2
4. CH3—C
O
-
C
R
O
-
O
+
OH
O
5. CH2 = C— COOH
CH3 — C— COOH
O
A: 4
B:l
C:2
D:5
E:3
28. Select the correct statements on the  (pi) molecular orbitals!
1.  molecular orbitals are always formed together with sigma molecular orbitals.
2.  molecular orbitals have no cylindrical symmetry around the internuclear axis.
3.  electrons are symmetrically distributed around the internuclear axis.
4. Only one  bond is possible between two atoms.
A: 1,2,3
B:2,4
C: 1,3,4
D:4
29. Which statements are true for the following pair of compounds?
COOH

HO-C-H

CH3
COOH

H-C-OH

CH3
[]D = + 3.3º
[]D = - 3.3o
1. The two compounds are enatiomers.
2. The compound on the left is the L(+) form.
3. The compound on the left is the L(-) form.
4. The compound on the left is the R-lactic acid.
5. The compound on the left is the S-lactic acid.
A: 1,2,4
B: l,2
C: 3,5
D: 2,4
E: l,2,5
E:l,2,3,4
30. The isomers of butanal include all of the following compounds except
1. 2,3-epoxybutane 2. tetrahydrofuran 3. ethyl-vinyl ether
4. dibutyl ether
A: 1
B: 2
5. 2-hydroxy-1-butene
C: 3
D: 4
E: 5
31. Which of the following compounds contain more than one chiral center?
l. malate 2. aconitate 3. tartarate 4. -amino--hydroxybutyric acid
A: 1
B:2,3
C:l,2,3,4
D:2,3,4
E:3,4
32. Which of the following IUPAC names is correct ?
CH3—CH2—C—CH2—CH3
1. 3-methenyl-pentane 2.3-ethyl-3-butene
3. 2-ethyl-l-butene
4. 1-diethyl-ethene
CH2
5. 3-methyl-pentane
A: 4
B:3
C:2
D:1
E:5
33. Which statements are true for the following compound?
CH3—CH2—CH2—Br
1. The compound can be formed from propane by UV light induced bromination, in a radical
substitution type of reaction.
2. The compound is the main product of the HBr addition to 1-propene.
3. The compound is the minor byproduct of HBr addition to 1-propene.
4. The compound can be used to produce hexane.
5. The compound easily reacts with electrophiles.
A: 1,3,5
B: 1,3,4
C:2,5
D: 1,2,4,5
E:l,3,4,5
34. In which of the following reactions will the second substitution occur
in ortho position ?
1. toluene + chlorine (FeCl3 catalyst)
2. nitrobenzene + cc. sulfuric acid
3. benzenesulfonic acid + cc. nitric acid (sulfuric acid catalyst)
4. iodobenzene + bromine (FeBr3 catalyst)
5. toluene + acetyl chloride (AlCl3 catalyst)
A: 1,2,3,4,5
B: 2,4,5
C: l,4,5
D: 1,2,3
E:2,3,4
35. Which of the following compounds contains two hetero-atoms?
A: pyrrole
B: pyran
C: pyridine D: furan
E: pyrimidine
36. What is the type of compounds that is formed upon the reaction of phenol with an
alcohol?
1. phenylalcohol
A: 1
2. phenolether 3. anhydride
B: 2
C: 3
4. phenolester 5. phenylacetale
D: 4
E: 5
37. What is the common name of the compounds containing a hydroxyl group linked directly
to the aromatic ring?
1. hydroxols 2. phenols 3. aromatic alcohols
A: 1
B: 2
C: 3
D: 4
4. enols
E:5
38. Select the proper pair(s) to the equation:
1.
R—OH ———> hemiacetal
2.
H2O
3.
R—NH2 ———> Schiff-base
5. thiols
Aldehyde + X
———> hydrate
O
CH3 - C ———> aldol
4.
H
H2N—OH ———> oxime
5.
A: 1,3
B: l
C: 2,3
D:1,2,3,4,5
E: l,2,3,4
39. Which of the following compounds contain oxo-group?
l. acetone 2. oxaloacetic acid
A: 1,2,3
B: 1,4
3. propanol
C: 1,2,3,4
4. butanol
D: 1,2
E: 3,4
40. Which are oxo compounds?
1. A carbonyl group bound to two hydrogen atoms.
2. A carbonyl group bound to a hydrogen and an alkyl group.
3. A carbonyl group bound to a hydrogen and an aryl group.
4. A hydroxyl group bound to an alkyl group.
5. A hydroxyl group bound to an aryl group.
A: 2,3
B:3,5
C: 1,2,3
D: 1,2,4
E: 4,5
———> Y
41. Which of the following compounds contain more than one chiral center?
l.citrate
A: 2,3
2. tartarate
B: 2,3,4
3. isocitrate
C: 2,4
4. 1,2-dimethylcyclohexane
D: l,2,3,4
E: 1,2
42. From the listed compounds, which are hydroxy-carboxylic acids?
l. malic acid
A: 1,3
2. acetone
B: 2,3
3. pyruvic acid
C: 1,2,3
4.citric acid 5. lactic acid
D: 3,5
E: 1,4,5
43. Which of the following statements are true?
1. Both benzene and pyridine have a symmetrical electron distribution.
2. Pyridine tends to undergo substitution type of reactions rather than addition.
3. Like benzene pyridine is miscible with most organic solvents.
4. Unlike benzene pyridine is completely miscible with water.
5. Pyridine is a weak acid.
A: 1,4,5
B: 2,3,5
C: 2,4,5
D: 1,2,3
E: 2,3,4
44. Select the pyrimidine derivatives from the following compounds ¡
OH
O
HN
O
N
N
H
O
1.
A: 4,5
OH
OH
N
N
H
HO
2.
B: 1,2,3
OH
N
HO
3.
C: 1,2,3,4,5
N
4.
D: 2,5
E: 2,3
N
O
N
H
5.
N
45. Find the incorrect pairing of name to formula:
1. H2SO4 - sulfuric acid
2. H2SO3 - sulfurous acid
3. HPO3 - metaphosphoric acid
4. HNO2 - nitric acid
5. HCl - hydrochloric acid
A: 1
B: 2
C: 3
D: 4
E: 5
46. What indicators are appropriate for complexometric titrations?
1. potassium chromate
2. eriochrome black T
3. methyl red
4. murexide
A: 2,3,4
B: 1,2,3,4
C:l,3
D:4
E: 2,4
47. Select the suitable titration method(s) for the quantitative determination of oxalic acid !
1. Iodometry
2. Permanganometry
A: 2,4
B: 4
3. Complexometry
C: 2
D: 1,3
4. Acidi-alkalimetry
E: 3,4
48. 10 ml unknown H2SO4 (Molecular mass: 98) solution reacts quantitatively with 7.25 ml
0.1 N NaOH (f=0.97). What is the w/v % concentration of the unknown solution?
A: 1.72
B:3.45
C:0.69
D:0.1725
E:0.345
49. Which of the following ligands are polydentate?
l. CNA: 2
2. EGTA
B: 2,3
3. CO
C: l,4
4. NH3
D: 1,2,3,4
E: 1,2,3
50. What is the Lugol solution?
1. solution of iodine in water 2. solution of iodine in chloroform
3. solution of iodine in KIO3 4. solution of KI in water
5. solution of iodine and KI in water
A: 1
B: 2
C: 3
D: 4
E: 5
Solutions of the multiple choice tests
1.
2.
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C
B
A
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D
C
C
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A
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E
A
B
C
D
D
A
D
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C
D
A
E
C
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D
A
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D
E
B
B
C
E
B
B
D
D
C
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50.
B
E
E
B
D
E
A
E
A
E