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Worksheets

FINAL CHEMISTRY FOR OHARMACY

Total questions: 99

Worksheet time: 8hrs 15mins

Name
Class
Date
1.

Based on the (Hof data given, which compound is the most stable?

a)

N2O4(g), +9.7 kJ/mol

b)

H2S(g), -20.6 kJ/mol

c)

N2H4(g), +94.5 kJ/mol

d)

PH3(g), +5.4 kJ/mol

e)

NH3(g), -46.4 kJ/mol

2.

Which ionic solid is likely to have the largest exothermic lattice energy?

a)

KCl

b)

NaCl

c)

LiCl

d)

CsCl

e)

They all have the same value.

3.

Which of the following solids is likely to have the largest exothermic lattice energy?

a)

LiF

b)

NaCl

c)

AlCl3

d)

Al2O3

e)

CaCl2

4.

Sodium forms a monatomic ion which has the electronic configuration of a noble gas. What is the electron configuration of that noble gas?

a)

1s2

b)

1s2 2p6

c)

1s2 2s2 2p6

d)

1s2 2s2 2p6 3s2

e)

1s2 2s2 2p6 3s2 3p6

5.

Bromine tends to form a monatomic ion which has the electronic configuration of a noble gas. What is the electron configuration of that noble gas?

a)

1s2 2s2 2p6 3s2 3p6 3d10 4p6

b)

1s2 2s2 2p6 3s2 3p6 4p6 4d10

c)

1s2 2s2 2p6 3s2 3p6 4s2 4p6

d)

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6

e)

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10

6.

The octet rule is generally followed for cations of which elements?

a)

post transition metals and transition metals

b)

Group IA and Group IIA metals

c)

Group IVA elements

d)

lanthanide elements

e)

actinide elements

7.

Which ion of uranium has a noble gas configuration?

a)

U2+

b)

U3+

c)

U4+

d)

U6+

e)

U2

8.

Which atom has the same electron configuration as In3+?

a)

Te

b)

Pd

c)

Ir

d)

Zn

e)

Ga

9.

Give the ground state electron configuration and number of unpaired electrons for V3+.

a)

[Ar] 3d1; 2 unpaired electrons

b)

[Ar]; 1 unpaired electron

c)

[Ar] 3d2; 2 unpaired electrons

d)

[Ar] 3d3; 3 unpaired electrons

e)

[Ar] 3d4; 4 unpaired electrons

10.

Which metal ion is expected to have the electron configuration, [Kr]4d4?

a)

Mn2+

b)

Ru2+

c)

Zr2+

d)

Mo2+

e)

Sr2+

11.

Which element below has three valence electrons in its Lewis symbol?

a)

gallium

b)

fluorine

c)

iron

d)

nickel

e)

sulfur

12.

Which species below has eight valence electrons in its Lewis symbol?

a)

Ar+

b)

F+

c)

Mg+

d)

S 2-

e)

Si

13.

Which element below has six electrons surrounding its Lewis symbol?

a)

Cr

b)

Ni

c)

Ba

d)

Se

e)

As

14.

Which species has the most valence electrons in its Lewis symbol?

a)

Ar+

b)

Ga+

c)

Ba2+

d)

Br

e)

O 2-

15.

The atoms in the nitrogen molecule, N2, are held together by

a)

a single covalent bond

b)

a double covalent bond

c)

a triple covalent bond

d)

an ionic bond

e)

a magnetic dipole bond

16.

The atoms in the oxygen molecule, O2, are held together by

a)

a single covalent bond

b)

a double covalent bond

c)

a triple covalent bond

d)

an ionic bond

e)

a magnetic dipole bond

17.

A covalent bond is characterized by two properties. These are

a)

the energy of the bond and the location of the electron pair in the bond.

b)

the energy of the separated atoms and the energy of the new bond.

c)

the bond length and the polarity of the covalent bond.

d)

the bond length and the bond energy.

e)

the energy released when a bond forms, and the electronegativities of the two atoms.

18.

The Lewis symbol for the carbon atom has __ valence electrons. The number of covalent bonds which carbon usually forms in order to complete its valence shell and obey the octet rule is __.

a)

4, 1

b)

4, 2

c)

2, 4

d)

4, 3

e)

4, 4

19.

The Lewis symbol for the nitrogen atom has __ valence electrons. The number of covalent bonds which nitrogen usually forms in order to complete its valence shell and obey the octet rule is __.

a)

5, 1

b)

5, 2

c)

3, 4

d)

5, 3

e)

5, 4

20.

Alcohols belong to a class of organic compounds in which a hydrogen atom in a hydrocarbon is replaced by which of the following?

a)

Ar atom

b)

NO group

c)

OH group

d)

F atom

e)

A metal ion

21.

Ketones belong to a class of organic compounds in which a hydrogen atom in a hydrocarbon is replaced by which of the following?

a)

An argon atom

b)

A doubly bonded sulfur atom

c)

A doubly bonded carbon atom

d)

A triply bonded nitrogen atom

e)

A doubly bonded oxygen atom

22.

Organic acids are characterized by the presence of which particular group of atoms?

a)

Hydronium ion, H3O+

b)

An extra -CH2 group

c)

A doubly bonded carbon atom

d)

Carboxyl group, -CO2H

e)

A doubly bonded hydrogen atom

23.

How many lone pairs of electrons are on the group of atoms which characterize organic acids?

a)

6

b)

4

c)

3

d)

2

e)

1

24.

Amines are weak organic bases and can be considered derived from which compound?

a)

H2O

b)

SO2

c)

NH3

d)

CH3C1

e)

CO2

25.

Which bond is the most polar?

a)

H-C

b)

H-Cl

c)

H-P

d)

H-S

e)

H-Se

26.

Arrange the following in terms of increasing electronegativity values.

a)

P < Ga < Ge < As

b)

As < P < Ga < Ge

c)

Ga < Ge < As < P

d)

Ge < P < As < Ga

e)

Ga < P < As < Ge

27.

Based on electronegativity considerations, which species should be the strongest oxidizing agent?

a)

Ne

b)

Kr

c)

Br2

d)

Cl2

e)

S

28.

Based on the "best" Lewis structure after applying formal charge considerations, how many non-bonding valence electrons are around the nitrogen atom in the nitrate ion?

a)

0

b)

2

c)

4

d)

6

e)

8

29.

Draw a Lewis structure for CH2Cl2. Based on this Lewis structure, the calculated value for the formal charge on the carbon atom is

a)

0

b)

4+

c)

2+

d)

2

e)

4

30.

When the fluoride ion reacts with a BF3 molecule (a molecule in which there are no multiple bonds) an ion is formed in which the boron atom is the central atom. The bond between the boron triundefinedfluoride and the fluoride ion is

a)

an ionic bond.

b)

a regular covalent bond, where both species contribute 1 electron to the bond.

c)

a coordinate covalent bond.

d)

a resonance hybrid bond.

e)

a bond where two atoms share one electron instead of two.

31.

How many coordinate covalent bonds are formed in the reaction between H+ and NH3, and what is the formula of the only product?

a)

0, NH3

b)

1, NH4+

c)

2, NH4+

d)

3, N2H4+

e)

4, N2H5+

32.

Draw the Lewis structure for hydrogen peroxide, H2O2. Based on this structure, how many polar bonds and non-polar bonds are present?

a)

3 polar bonds and no non-polar bonds

b)

2 polar bonds and 1 non-polar bond

c)

1 polar bond and 2 non-polar bonds

d)

no polar bonds and 3 non-polar bonds

e)

2 polar bonds and 2 non-polar bonds

33.

The formal charge on the nitrogen atom in the nitrate ion is

a)

3-

b)

0

c)

1+

d)

3+

e)

5+

34.

Based on the 'best' Lewis structure after applying formal charge considerations, how many non-bonding valence electrons are around the carbon atom in the CO molecule?

a)

0

b)

2

c)

4

d)

6

e)

8

35.

Draw a Lewis structure for H3C-NH2. Based on this Lewis structure, the calculated value for the formal charge on the nitrogen atom is

a)

2

b)

3+

c)

3

d)

2+

e)

0

36.

Draw the Lewis structure for the H2CO molecule. Based on this structure, how many polar bonds and non-polar bonds are present?

a)

3 polar bonds and no non-polar bonds

b)

2 polar bonds and 1 non-polar bond

c)

1 polar bond and 2 non-polar bonds

d)

no polar bonds and 3 non-polar bonds

e)

2 polar bonds and 2 non-polar bonds

37.

Draw the 'best' Lewis structure for sulfur trioxide based on formal charge considerations. The number of resonance structures is

a)

1 (no resonance)

b)

2

c)

3

d)

4

e)

5

38.

How many resonance structures, if any, can be drawn for the nitrate ion?

a)

1 (no resonance)

b)

2

c)

3

d)

4

e)

5

39.

Which of the five basic geometries for molecules and ions has the largest bond angle?

a)

linear

b)

planar triangular

c)

tetrahedral

d)

square planar

e)

octahedral

40.

Which of the five basic geometries for molecules and ions has the smallest bond angle?

a)

linear

b)

planar triangular

c)

tetrahedral

d)

octahedral

e)

These all have the same bond angles.

41.

Which basic arrangement would best accommodate three electron domains in the valence shell of a covalently bonded atom?

a)

planar triangular

b)

octahedral

c)

tetrahedral

d)

linear

e)

trigonal bipyramidal

42.

Which basic arrangement would best accommodate five electron domains in the valence shell of a covalently bonded atom?

a)

planar triangular

b)

octahedral

c)

tetrahedral

d)

linear

e)

trigonal bipyramidal

43.

Based on the Lewis structure, the number of electron domains in the valence shell of the boron atom in the BF₃ molecule is

a)

1

b)

2

c)

3

d)

4

e)

5

44.

Based on the Lewis structure, the number of electron domains in the valence shell of the carbon atom in the CO₃²⁻ ion is

a)

1

b)

2

c)

3

d)

4

e)

5

45.

Based on the Lewis structure, the number of electron domains in the valence shell of the xenon atom in the XeF₂ molecule is

a)

1

b)

2

c)

3

d)

4

e)

5

46.

Application of the concepts of the VSEPR theory, suggests that the shape of the SO₃ molecule is

a)

trigonal pyramidal.

b)

square planar.

c)

regular tetrahedral.

d)

triangular planar.

e)

distorted tetrahedron.

47.

The geometry of the CS₂ molecule is best described as

a)

bent.

b)

linear.

c)

regular tetrahedral.

d)

triangular planar.

e)

trigonal pyramidal.

48.

Application of the VSEPR theory suggests that the geometric arrangement of the atoms in the carbonate ion, CO₃²⁻, is

a)

octahedral.

b)

square planar.

c)

regular tetrahedral.

d)

triangular planar.

e)

trigonal pyramidal.

49.

The bond angle in Cl₂O is expected to be approximately

a)

90 degrees.

b)

109.5 degrees.

c)

120 degrees.

d)

145 degrees.

e)

180 degrees.

50.

Application of the VSEPR model to the NCl₃ molecule leads to the prediction that

a)

the molecule should have trigonal pyramidal geometry.

b)

the molecule should have delocalized valence electrons.

c)

the molecule should be non-polar.

d)

the formal charge on the center atom is +3.

e)

the molecule should have a planar triangular geometry.

51.

Based on conclusions from application of the VSEPR theory, which one of the following is linear?

a)

IF₂⁻

b)

HCN

c)

H₂CO

d)

H₂S

e)

SO₂

52.

Based on observed periodic trends, arrange the following species, HBr, HCl, HF, HI, in order of increasing dipole moment.

a)

HF < HCl < HBr < HI

b)

HBr < HCl < HF < HI

c)

HI < HF < HCl < HBr

d)

HI < HBr < HCl < HF

e)

HCl < HBr < HI < HF

53.

Based on application of the VSEPR theory, which molecule should be nonpolar?

a)

CH₃Cl

b)

CSe₂

c)

H₂O

d)

NH₃

e)

OF₂

54.

Which molecule below is polar?

a)

CF₅

b)

BF₃

c)

C₂H₂

d)

CS₂

e)

IBr

55.

PR theory, which molecule should be nonpolar?

a)

CH₃Cl

b)

CSe₂ (*)

c)

H₂O

d)

NH₃

e)

OF₂

56.

Which molecule below is polar?

a)

CF₅

b)

BF₃

c)

C₂H₂

d)

CS₂

e)

IBr (*)

57.

Predict the molecular geometry and polarity of the SO₂ molecule by applying VSEPR theory.

a)

linear, nonpolar

b)

linear, polar

c)

bent, 109.5° bond angle, polar

d)

bent, 120° bond angle, polar (*)

e)

bent, 109.5° bond angle, nonpolar

58.

Bonding in the hydrogen chloride molecule can be explained by the valence bond theory in terms of an overlap between

a)

the 1s orbital of the hydrogen atom and the 1s orbital of the chlorine atom.

b)

the 1s orbital of the hydrogen atom and the 2s orbital of the chlorine atom.

c)

the 1s orbital of the hydrogen atom and the 2p orbital of the chlorine atom.

d)

the 1s orbital of the hydrogen atom and the 3p orbital of the chlorine atom. (*)

e)

the 1s orbital of the hydrogen atom and the 3p orbital of the chlorine atom.

59.

Draw a Lewis structure for the CH₄ molecule. What hybrid orbitals are used by the carbon atom for bonding?

a)

sp³d²

b)

sp

c)

sp³d

d)

sp³ (*)

e)

sp²

60.

Draw a Lewis structure for ethylene, C₂H₂. The hybridization on C is

a)

sp (*)

b)

sp²

c)

sp³

d)

sp³d

e)

sp³d²

61.

Draw a Lewis structure for the NH₃ molecule. What is the set of hybrid orbitals used by the nitrogen atom for bonding?

a)

sp³d²

b)

sp

c)

sp³d

d)

sp³ (*)

e)

sp²

62.

Draw a Lewis structure for the C₂H₄ molecule. What is the set of hybrid orbitals used by either of the carbon atoms for bonding?

a)

sp³d²

b)

sp

c)

sp³d

d)

sp³

e)

sp² (*)

63.

The central atom in SF₄ has σ-bonding pair(s) and lone pair(s) of electrons in the valence shell of the central atom.

a)

3, 2

b)

4, 0

c)

4, 1 (*)

d)

5, 0

e)

5, 1

64.

Draw a Lewis structure for H₃CNO₂. How many σ-bonds and π-bond(s) are in the molecule?

a)

7 σ-bonds and 0 π-bonds

b)

6 σ-bonds and 1 π-bond (*)

c)

1 σ-bond and 5 π-bonds

d)

5 σ-bonds and 2 π-bonds

e)

2 σ-bonds and 1 π-bond

65.

How many σ-bonds and π-bonds, respectively, are in a CO₂ molecule?

a)

1 σ-bond and 2 π-bonds

b)

2 σ-bonds and 0 π-bonds

c)

2 σ-bonds and 2 π-bonds (*)

d)

2 σ-bonds and 4 π-bonds

e)

4 σ-bonds and 0 π-bonds

66.

Which statement about the ammonia molecule is true?

a)

The N-H bonds are polar, but the molecule is non-polar.

b)

The molecule has both three σ- and one π-bond.

c)

The nitrogen atom can be said to utilize sp³ hybrid orbitals for σ-bonding. (*)

d)

The H-N-H bond angles are greater than 109.5 degrees.

e)

The molecular geometry is planar triangular.

67.

How many π-bonds are there in the CN⁻ ion?

a)

0

b)

1

c)

1.5

d)

2 (*)

e)

3

68.

Ozone (O₃) is an allotropic form of oxygen. Based on VSEPR and valence bond theory, which statement is true for this molecule?

a)

The molecule is linear, and has no lone pairs in the valence shell on the central atom.

b)

The molecule is linear, and has two π-bonds and one σ-bond.

c)

The molecule is T-shaped, and has two π-bonds and two σ-bonds.

d)

The molecule is bent, and has two lone pairs in the valence shell on the central atom.

e)

The molecule is bent, and has one π-bond and two σ-bonds. (*)

69.

What is the conjugate acid of HPO₄²⁻?

a)

H₂PO₄

b)

H₃PO₄

c)

PO₄³⁻

d)

PO₄²⁻

e)

H₂PO₄⁻ (Correct)

70.

What is the conjugate base of H₂AsO₄⁻?

a)

H₂AsO₄

b)

H₃AsO₄

c)

HAsO₄⁻

d)

HAsO₄²⁻ (Correct)

e)

AsO₄³⁻

71.

Which species is amphiprotic?

a)

PO₄³⁻(aq)

b)

HCl(g)

c)

HSO₄⁻(aq) (Correct)

d)

Cl⁻(aq)

e)

CO₃²⁻(aq)

72.

Which species does not have a conjugate base?

a)

H₂O

b)

H₃O⁺ (Correct)

c)

NH₂⁻

d)

OH⁻

e)

F⁻

73.

Which species has a conjugate base?

a)

Cl⁻

b)

SO₄²⁻

c)

CN⁻

d)

OH⁻

e)

CO₃²⁻ (Correct)

74.

In the reaction HClO₃ + N₂H₄ ⇌ ClO₃⁻ + N₂H₅⁺, which species are an acid-base conjugate pair?

a)

HClO₃, N₂H₄

b)

N₂H₄, ClO₃⁻

c)

HClO₃, N₂H₅⁺

d)

N₂H₄, N₂H₅⁺ (Correct)

e)

ClO₃⁻, N₂H₅⁺

75.

In the reaction HClO₃ + N₂H₄ ⇌ ClO₃⁻ + N₂H₅⁺, which two species are both acids?

a)

HClO₃, N₂H₄

b)

HClO₃, ClO₃⁻

c)

HClO₃, N₂H₅⁺ (Correct)

d)

N₂H₄, N₂H₅⁺

e)

ClO₃⁻, N₂H₅⁺

76.

In the reaction HClO₃ + N₂H₄ ⇌ ClO₃⁻ + N₂H₅⁺, which two species are both bases?

a)

HClO₃, N₂H₄

b)

HClO₃, ClO₃⁻

c)

HClO₃, N₂H₅⁺

d)

N₂H₄, N₂H₅⁺

e)

ClO₃⁻, N₂H₄ (Correct)

77.

Given the substances in order of increasing acid strength: HOCl(aq) < HC₂H₃O₂(aq) < HC₂O₄⁻(aq) < HOCN(aq) < HNO₂(aq) < HCl(aq), which species is the weakest base of that set?

a)

C₂H₃O₂⁻(aq)

b)

OCl⁻(aq)

c)

H₂C₂O₄(aq)

d)

Cl⁻(aq) (Correct)

e)

OCN⁻(aq)

78.

Which solution should be the most acidic?

a)

Al(NO₃)₃(aq) (Correct)

b)

Ca(NO₃)₂(aq)

c)

KNO₃(aq)

d)

Mg(NO₃)₂(aq)

e)

Zn(NO₃)₂(aq)

79.

Which species is the weakest acid?

a)

HBr

b)

HCl

c)

HF

d)

HI

e)

H₂Se

80.

Which species is the strongest acid?

a)

H₂O

b)

H₂S

c)

H₂Se

d)

H₂Te

e)

HCl

81.

NH₃ can react with BF₃, forming H₃N-BF₃. In this reaction,

a)

the NH₃ acts as a Brønsted acid, accepting a proton from the BF₃ molecule.

b)

the NH₃ acts as a Lewis base, donating a proton to the BF₃ molecule.

c)

the NH₃ acts as a Brønsted acid, donating a proton to the BF₃ molecule.

d)

the BF₃ molecule acts as a Lewis acid, accepting an electron pair from the NH₃ molecule to form a coordinate covalent bond.

e)

the BF₃ molecule acts as a Lewis base, donating an electron pair to the NH₃ molecule to form a coordinate covalent bond.

82.

Which solution would be the most basic?

a)

Al(NO₃)₃(aq)

b)

Ga(NO₃)₃(aq)

c)

AgNO₃(aq)

d)

Cu(NO₃)₂(aq)

e)

Zn(NO₃)₂(aq)

83.

Which solution would be the most acidic?

a)

Zn(NO₃)₂(aq)

b)

Cd(NO₃)₂(aq)

c)

Ga(NO₃)₃(aq)

d)

Hg(NO₃)₂(aq)

e)

Al(NO₃)₃(aq)

84.

If the OH- ion concentration in an aqueous solution at 25.0 °C is measured as 3.4 x 10-3 M, what is the pH?

a)

2.47

b)

7.22

c)

8.24

d)

11.53

e)

16.47

85.

The pH of a solution is measured to be 10.4. What are the values of [H3O+] and [OH-] for this solution?

a)

[H3O+] = 4.0 x 10-11, [OH-] = 4.0 x 10^3

b)

[H3O+] = 2.5 x 10-4, [OH-] = 4.0 x 10-11

c)

[H3O+] = 1.0 x 10-10, [OH-] = 3.6 x 10-4

d)

[H3O+] = 4.0 x 10-11, [OH-] = 2.5 x 10-4

e)

[H3O+] = 9.6 x 10-2, [OH-] = 2.8 x 10-1

86.

If the H+ ion concentration in an aqueous solution at 25.0 °C has a value of 0.100 M, what is the pOH of the solution?

a)

1.00

b)

7.00

c)

12.00

d)

13.00

e)

11.40

87.

Calculate the pH of a 0.020 M solution of Ca(OH)2 whose temperature is 25.0 °C.

a)

1.40

b)

0.040

c)

1.69

d)

12.60

e)

12.30

88.

Given 0.01 M solutions of each of the following bases, which solution would have the highest pH?

a)

Aniline (C6H5NH2), Kb = 3.9 x 10-10

b)

Dimethylamine ((CH3)2NH), Kb = 5.1 x 10-4

c)

Hydrazine (N2H4), Kb = 1.3 x 10-6

d)

Methylamine (CH3NH2), Kb = 4.4 x 10-4

e)

Pyridine (C5H5N), Kb = 1.7 x 10-9

89.

Given 0.01 M solutions of each of the following bases, which solution would have the highest pH?

a)

Aniline (C6H5NH2), pKb = 9.39

b)

Hydrazine (N2H4), pKb = 5.89

c)

Hydroxylamine (HONH2), pKb = 7.96

d)

Methylamine (CH3NH2), pKb = 3.36

e)

Butylamine (C4H9NH2), pKb = 3.23

90.

The ionization constant, Ka, for benzoic acid is 6.28 × 10-5. What is the pKa of this acid?

a)

1.592 × 104

b)

4.202

c)

4.452

d)

5.640

e)

9.800

91.

The ionization constant, Kb, for ammonia has a value of 1.76 × 10-5. What is the pKb of this base?

a)

+3.24

b)

-4.75

c)

+4.754

d)

-9.25

e)

+9.25

92.

Formic acid, HCO2H, has an ionization constant with the value: Ka = 1.76 × 10-4. Calculate the value of pKb for the conjugate base of formic acid.

a)

3.75

b)

5.35

c)

8.65

d)

10.25

e)

12.24

93.

What is the pH of a 1.00 molar solution of KCl?

a)

0.00

b)

6.90

c)

7.00

d)

7.10

e)

13.00

94.

What is the pH of a 1.00 molar solution of NH4Cl(aq)? The Kb for NH3 is 1.8 × 10-5.

a)

2.37

b)

4.63

c)

9.26

d)

9.37

e)

11.63

95.

Which one of the following salts will form a basic solution upon dissolving in water?

a)

NaCl

b)

NaNO2

c)

NH4NO3

d)

KBr

e)

AlCl3

96.

A mixture contains 0.060 moles of NaH2PO4 and 0.080 moles of K2HPO4. It is titrated with 0.500 molar NaOH(aq) to neutralize it completely. How many mL of the NaOH solution are required?

a)

280 mL

b)

313.3 mL

c)

372 mL

d)

400 mL

e)

440 mL

97.

Which is the most appropriate acid-base indicator to use in the titration of 0.100 molar acetic acid(aq) by 0.100 molar NaOH(aq)? This is the titration of a weak acid by a strong base.

a)

phenol red, for which pKIn = 7.3, also HInd is yellow and Ind is red

b)

bromothymol blue, for which pKIn = 6.8, also HInd is yellow and Ind is blue

c)

phenolphthalein, for which pKIn = 9.1, also HInd is colorless and Ind is pink

d)

cresol red, for which pKIn = 7.9, also HInd is yellow and Ind is red

e)

These indicators will all work equally well for the titration of a weak acid by a strong base.

98.

The pH at the equivalence point of the titration of perchloric acid solution by sodium hydroxide solution is

a)

< 2.00

b)

4.00 < pH < 7.00

c)

7.00

d)

7.00 < pH < 11.00

e)

> 11.0

99.

The pH at the equivalence point of the titration of ammonia solution by hydrochloric acid solution is

a)

< 2.00

b)

4.00 < pH < 7.00

c)

7.00

d)

7.00 < pH < 11.00

e)

> 11.0

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