Question 1

All of the following 0.1 M aqueous solutions are acidic except

Accepted Answer

A) Na2SO4. 
B) Cr(ClO4)3. 
C) C6H5OH. 
D) C2H5NH3Cl. 
A) Na2SO4. 
B) Cr(ClO4)3. 
C) C6H5OH. 
D) C2H5NH3Cl. A

Question 2

The following 0.1 M aqueous solutions are arranged in order of increasing pH,with the highest pH on the far right.   Which one of the following 0.10 M aqueous solutions should be placed in the empty box?

Accepted Answer

A) CuSO4  
B) NaNO2  
C) CH3NH2  
D) NaHCO3  
E) Na2HPO4  
A) CuSO4  
B) NaNO2  
C) CH3NH2  
D) NaHCO3  
E) Na2HPO4  A

Question 3

Which of the following is the strongest acid?

Accepted Answer

A) CH3CH2OH 
B) CH3COOH 
C) CHCl2COOH 
D) CH2ClCOOH 
E) CCl3COOH 
A) CH3CH2OH 
B) CH3COOH 
C) CHCl2COOH 
D) CH2ClCOOH 
E) CCl3COOH E

Question 4

The boxes below contain a series of 0.1 M aqueous solutions of increasing pH where A is the solution of lowest pH and E is the solution of highest pH.   Match each box with the correct compound.
phenol,pKa = 9.89
cyanide ion,pKb = 4.69
pyridine,pKb = 8.75
hydrogen sulfate ion,pKa = 1.92
sodium nitrate

Accepted Answer

phenol,pK_a = 9.89 (B) cyanide i

Question 5

In liquid ammonia,the acid HB is a strong acid if it is a weaker proton donor than NH4+.True or false?

Accepted Answer

A) True 
 B)False

Question 6

The conjugate base of ammonia is

Accepted Answer

A) NH2OH. 
B) NH2F1F1F1S1F1F1F10. 
C) NH4+. 
D) NH3. 
E) OHF1F1F1S1F1F1F10. 
A) NH2OH. 
B) NH2F1F1F1S1F1F1F10. 
C) NH4+. 
D) NH3. 
E) OHF1F1F1S1F1F1F10.

Question 7

For a solution labeled "0.10 M H2SO4(aq),"

Accepted Answer

A) [HSO4F1F1F1S1F1F1F10] is greater than 0.10 M. 
B) the pH is less than 1.0. 
C) [SO42F1F1F1S1F1F1F10] = 0.10 M. 
D) the pH equals 1.0. 
E) the pH is greater than 1.0. 
A) [HSO4F1F1F1S1F1F1F10] is greater than 0.10 M. 
B) the pH is less than 1.0. 
C) [SO42F1F1F1S1F1F1F10] = 0.10 M. 
D) the pH equals 1.0. 
E) the pH is greater than 1.0.

Question 8

The following 0.1 M aqueous solutions are arranged in order of increasing pH,with the highest pH on the far right.   Which one of the following 0.10 M aqueous solutions should be placed in the empty box?

Accepted Answer

A) NaI 
B) HCOOH 
C) C6H5NH2  
D) CH3NH3Cl 
E) NaClO 
A) NaI 
B) HCOOH 
C) C6H5NH2  
D) CH3NH3Cl 
E) NaClO

Question 9

Estimate the pH of 10F1F1F1S1F1F1F107 M HClO4(aq).

Accepted Answer

A) 6.8 
B) 8.0 
C) 1.0 
D) 5.0 
E) 7.0 
A) 6.8 
B) 8.0 
C) 1.0 
D) 5.0 
E) 7.0

Question 10

Calculate the equilibrium constant for the reaction S2F1F1F1S1F1F1F10(aq)+ H2O(l)↔ HSF1F1F1S1F1F1F10(aq)+ OHF1F1F1S1F1F1F10(aq),
Given Ka1 = 1.3 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F107 and Ka2 = 7.1 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1015 for H2S.

Accepted Answer

A) 1.3 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F107  
B) 9.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1022  
C) 7.7 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108  
D) 7.1 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1015  
E) 1.4 
A) 1.3 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F107  
B) 9.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1022  
C) 7.7 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108  
D) 7.1 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1015  
E) 1.4

Question 11

All of the following acids have the same strength in water except

Accepted Answer

A) HNO3 
B) HClO3 
C) HBr 
D) HF 
A) HNO3 
B) HClO3 
C) HBr 
D) HF

Question 12

Which of the following is the weakest acid?

Accepted Answer

A) HNO3  
B) HBr 
C) HCl 
D) HF 
E) HI 
A) HNO3  
B) HBr 
C) HCl 
D) HF 
E) HI

Question 13

The equation that represents Ka2 for phosphoric acid is

Accepted Answer

A) HPO42F1F1F1S1F1F1F10(aq)+ H2O(l)↔ PO43F1F1F1S1F1F1F10(aq)+ H3O+(aq) 
B) H2PO4F1F1F1S1F1F1F10(aq)+ H2O(l)↔ HPO42F1F1F1S1F1F1F10(aq)+ H3O+(aq). 
C) H3PO4(aq)+ 2H2O(l)↔ HPO42F1F1F1S1F1F1F10(aq)+ 2H3O+(aq). 
D) HPO42F1F1F1S1F1F1F10(aq)+ H2O(l)↔ H2PO4F1F1F1S1F1F1F10(aq)+ OHF1F1F1S1F1F1F10(aq). 
E) H3PO4(aq)+ H2O(l)↔ H2PO4F1F1F1S1F1F1F10(aq)+ H3O+(aq). 
A) HPO42F1F1F1S1F1F1F10(aq)+ H2O(l)↔ PO43F1F1F1S1F1F1F10(aq)+ H3O+(aq) 
B) H2PO4F1F1F1S1F1F1F10(aq)+ H2O(l)↔ HPO42F1F1F1S1F1F1F10(aq)+ H3O+(aq). 
C) H3PO4(aq)+ 2H2O(l)↔ HPO42F1F1F1S1F1F1F10(aq)+ 2H3O+(aq). 
D) HPO42F1F1F1S1F1F1F10(aq)+ H2O(l)↔ H2PO4F1F1F1S1F1F1F10(aq)+ OHF1F1F1S1F1F1F10(aq). 
E) H3PO4(aq)+ H2O(l)↔ H2PO4F1F1F1S1F1F1F10(aq)+ H3O+(aq).

Question 14

The amino acid methionine,HOOC-CH(CH2CH2SCH3)NH3+,has pKa1 = 2.2 and pKa2 = 9.1.If this amino acid is represented by H2L+,the major species at pH 6 is

Accepted Answer

A) HL 
B) H2L+ 
C) LF1F1F1S1F1F1F10 
D) HL and LF1F1F1S1F1F1F10 
A) HL 
B) H2L+ 
C) LF1F1F1S1F1F1F10 
D) HL and LF1F1F1S1F1F1F10

Question 15

The following 0.1 M aqueous solutions are arranged in order of increasing pH,with the highest pH on the far right.   Which one of the following 0.10 M aqueous solutions should be placed in the empty box?

Accepted Answer

A) NH4Cl 
B) NaCN 
C) Al2(SO4)3  
D) CH3NH2  
E) CH3COOH 
A) NH4Cl 
B) NaCN 
C) Al2(SO4)3  
D) CH3NH2  
E) CH3COOH

Question 16

Which of the following aqueous solutions gives a pH greater than 7?

Accepted Answer

A) 10F1F1F1S1F1F1F108 M NH4Cl 
B) None of the solutions gives a pH greater than 7. 
C) 10F1F1F1S1F1F1F108 M CH3COOH 
D) 10F1F1F1S1F1F1F108 M HCl 
E) 10F1F1F1S1F1F1F108 M HCOOH 
A) 10F1F1F1S1F1F1F108 M NH4Cl 
B) None of the solutions gives a pH greater than 7. 
C) 10F1F1F1S1F1F1F108 M CH3COOH 
D) 10F1F1F1S1F1F1F108 M HCl 
E) 10F1F1F1S1F1F1F108 M HCOOH

Question 17

What is the molarity of OHF1F1F1S1F1F1F10 in a 0.0018 M calcium hydroxide solution?

Accepted Answer

A) 0.0009 M 
B) 0.0036 M 
C) 0.0018 M 
D) 0.0072 M 
E) None of the above. 
A) 0.0009 M 
B) 0.0036 M 
C) 0.0018 M 
D) 0.0072 M 
E) None of the above.

Question 18

If F1F1F1S1F1F1F10(HSO3F1F1F1S1F1F1F10)= 0.45 at pH 7.0,what are F1F1F1S1F1F1F10(H2SO3)and F1F1F1S1F1F1F10(SO32F1F1F1S1F1F1F10)at this pH? For H2SO3,pKa1 and pKa2 are 1.81 and 6.91,respectively.

Accepted Answer

A) (F1F1F1S1F1F1F10(H2SO3)= 0.225 and F1F1F1S1F1F1F10(SO32F1F1F1S1F1F1F10)= 0.55) 
B) (F1F1F1S1F1F1F10(H2SO3)= 0.55 and F1F1F1S1F1F1F10(SO32F1F1F1S1F1F1F10)~ 0) 
C) (F1F1F1S1F1F1F10(H2SO3)~ 0 and F1F1F1S1F1F1F10(SO32F1F1F1S1F1F1F10)= 0.225) 
D) (F1F1F1S1F1F1F10(H2SO3)~ 0 and F1F1F1S1F1F1F10(SO32F1F1F1S1F1F1F10)= 0.55) 
E) (F1F1F1S1F1F1F10(H2SO3)= 0.45 and F1F1F1S1F1F1F10(SO32F1F1F1S1F1F1F10)= 0.55) 
A) (F1F1F1S1F1F1F10(H2SO3)= 0.225 and F1F1F1S1F1F1F10(SO32F1F1F1S1F1F1F10)= 0.55) 
B) (F1F1F1S1F1F1F10(H2SO3)= 0.55 and F1F1F1S1F1F1F10(SO32F1F1F1S1F1F1F10)~ 0) 
C) (F1F1F1S1F1F1F10(H2SO3)~ 0 and F1F1F1S1F1F1F10(SO32F1F1F1S1F1F1F10)= 0.225) 
D) (F1F1F1S1F1F1F10(H2SO3)~ 0 and F1F1F1S1F1F1F10(SO32F1F1F1S1F1F1F10)= 0.55) 
E) (F1F1F1S1F1F1F10(H2SO3)= 0.45 and F1F1F1S1F1F1F10(SO32F1F1F1S1F1F1F10)= 0.55)

Question 19

For a 0.10 M solution of a weak acid,HA,with pKa = 10,which of the following is true?

Accepted Answer

A) [HA] F1F1F1S1F1F1F10 0 
B) [HA] = [AF1F1F1S1F1F1F10] 
C) [HA] = [H3O+] 
D) [HA] = Ka  
E) [HA] F1F1F1S1F1F1F10 [H3O+] 
A) [HA] F1F1F1S1F1F1F10 0 
B) [HA] = [AF1F1F1S1F1F1F10] 
C) [HA] = [H3O+] 
D) [HA] = Ka  
E) [HA] F1F1F1S1F1F1F10 [H3O+]

Question 20

HBrO(aq),in a 0.25 M solution,has a pKa = 8.69.What is its pH?

Accepted Answer

A) 0.60 
B) 4.65 
C) 5.90 
D) 8.10 
E) 9.30 
A) 0.60 
B) 4.65 
C) 5.90 
D) 8.10 
E) 9.30

All of the following 0.1 M aqueous solutions are acidic except

The following 0.1 M aqueous solutions are arranged in order of increasing pH,with the highest pH on the far right. Which one of the following 0.10 M aqueous solutions should be placed in the empty box?

Which of the following is the strongest acid?

In liquid ammonia,the acid HB is a strong acid if it is a weaker proton donor than NH₄⁺.True or false?

The conjugate base of ammonia is

For a solution labeled "0.10 M H₂SO₄(aq),"

The following 0.1 M aqueous solutions are arranged in order of increasing pH,with the highest pH on the far right. Which one of the following 0.10 M aqueous solutions should be placed in the empty box?

Estimate the pH of 10^⁷ M HClO₄(aq).

Calculate the equilibrium constant for the reaction S²^(aq)+ H₂O(l)↔ HS^(aq)+ OH^(aq), Given K_a1 = 1.3  10^⁷ and K_a2 = 7.1  10^¹⁵ for H₂S.

All of the following acids have the same strength in water except

Which of the following is the weakest acid?

The equation that represents K_a2 for phosphoric acid is

The amino acid methionine,HOOC-CH(CH₂CH₂SCH₃)NH₃⁺,has pK_a1 = 2.2 and pK_a2 = 9.1.If this amino acid is represented by H₂L⁺,the major species at pH 6 is

The following 0.1 M aqueous solutions are arranged in order of increasing pH,with the highest pH on the far right. Which one of the following 0.10 M aqueous solutions should be placed in the empty box?

Which of the following aqueous solutions gives a pH greater than 7?

What is the molarity of OH^ in a 0.0018 M calcium hydroxide solution?

If (HSO₃^)= 0.45 at pH 7.0,what are (H₂SO₃)and (SO₃²^)at this pH? For H₂SO₃,pK_a1 and pK_a2 are 1.81 and 6.91,respectively.

For a 0.10 M solution of a weak acid,HA,with pK_a = 10,which of the following is true?

HBrO(aq),in a 0.25 M solution,has a pK_a = 8.69.What is its pH?

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Exam 12: Acids and Bases

All of the following 0.1 M aqueous solutions are acidic except

The following 0.1 M aqueous solutions are arranged in order of increasing pH,with the highest pH on the far right. Which one of the following 0.10 M aqueous solutions should be placed in the empty box?

Which of the following is the strongest acid?

In liquid ammonia,the acid HB is a strong acid if it is a weaker proton donor than NH4+.True or false?

The conjugate base of ammonia is

For a solution labeled "0.10 M H2SO4(aq),"

The following 0.1 M aqueous solutions are arranged in order of increasing pH,with the highest pH on the far right. Which one of the following 0.10 M aqueous solutions should be placed in the empty box?

Estimate the pH of 107 M HClO4(aq).

Calculate the equilibrium constant for the reaction S2(aq)+ H2O(l)↔ HS(aq)+ OH(aq), Given Ka1 = 1.3  107 and Ka2 = 7.1  1015 for H2S.

All of the following acids have the same strength in water except

Which of the following is the weakest acid?

The equation that represents Ka2 for phosphoric acid is

The amino acid methionine,HOOC-CH(CH2CH2SCH3)NH3+,has pKa1 = 2.2 and pKa2 = 9.1.If this amino acid is represented by H2L+,the major species at pH 6 is

The following 0.1 M aqueous solutions are arranged in order of increasing pH,with the highest pH on the far right. Which one of the following 0.10 M aqueous solutions should be placed in the empty box?

Which of the following aqueous solutions gives a pH greater than 7?

What is the molarity of OH in a 0.0018 M calcium hydroxide solution?

If (HSO3)= 0.45 at pH 7.0,what are (H2SO3)and (SO32)at this pH? For H2SO3,pKa1 and pKa2 are 1.81 and 6.91,respectively.

For a 0.10 M solution of a weak acid,HA,with pKa = 10,which of the following is true?

HBrO(aq),in a 0.25 M solution,has a pKa = 8.69.What is its pH?

The Quantum World

Quantum Mechanics in Action: Atoms

Chemical Bonds

Molecular Shape and Structure

The Properties of Gases

Liquids and Solids

Inorganic Materials

Thermodynamics: the First Law

Thermodynamics: the Second and Third Laws

Physical Equilibria

Chemical Equilibria

Aqueous Equilibria

Electrochemistry

Chemical Kinetics

The Elements: the Main Group Elements

The Elements: the D Block

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Organic Chemistry II

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In liquid ammonia,the acid HB is a strong acid if it is a weaker proton donor than NH₄⁺.True or false?

For a solution labeled "0.10 M H₂SO₄(aq),"

Estimate the pH of 10^⁷ M HClO₄(aq).

Calculate the equilibrium constant for the reaction S²^(aq)+ H₂O(l)↔ HS^(aq)+ OH^(aq), Given K_a1 = 1.3  10^⁷ and K_a2 = 7.1  10^¹⁵ for H₂S.

The equation that represents K_a2 for phosphoric acid is

The amino acid methionine,HOOC-CH(CH₂CH₂SCH₃)NH₃⁺,has pK_a1 = 2.2 and pK_a2 = 9.1.If this amino acid is represented by H₂L⁺,the major species at pH 6 is

What is the molarity of OH^ in a 0.0018 M calcium hydroxide solution?

If (HSO₃^)= 0.45 at pH 7.0,what are (H₂SO₃)and (SO₃²^)at this pH? For H₂SO₃,pK_a1 and pK_a2 are 1.81 and 6.91,respectively.

For a 0.10 M solution of a weak acid,HA,with pK_a = 10,which of the following is true?

HBrO(aq),in a 0.25 M solution,has a pK_a = 8.69.What is its pH?