Question 1

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH3COOH(aq) with 0.036 M NaOH(aq)? For acetic acid, Ka = 1.8 *10-5.

Accepted Answer

A)  0.018 M 
B)  0.0090 M 
C)  0.024 M 
D)  0.012 M 
E)  0.036 M 
A)  0.018 M 
B)  0.0090 M 
C)  0.024 M 
D)  0.012 M 
E)  0.036 M

Question 2

What potential does a cell have that uses bromine to oxidize hydrogen to H+ under standard conditions at 298 K?

Accepted Answer

A)  Negative 
B)  0 
C)  Positive 
D)  Negative at elevated pressure 
E)  None of the above 
A)  Negative 
B)  0 
C)  Positive 
D)  Negative at elevated pressure 
E)  None of the above

Question 3

When silver ions form a coordination complex with the thiosulfate ion,the latter acts as a Lewis acid.

Accepted Answer

A) True 
 B)False

Question 4

Consider the titration of 50.0 mL of 0.0200 M C6H5COOH(aq), with 0.100 M NaOH(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of base? Do not consider spectator ions.

Accepted Answer

C<sub>6</sub>H<sub>5

Question 5

What do the six strong acids have in common in all reactions?

Accepted Answer

A)  Each can fully dissociate one or two protons, depending on the reaction. 
B)  They each produce a reaction solution possessing a pH less than 7. 
C)  They each dissociate 100% in solution. 
D)  Nothing, other than being strong, they do not all dissociate the same in all reactions. 
A)  Each can fully dissociate one or two protons, depending on the reaction. 
B)  They each produce a reaction solution possessing a pH less than 7. 
C)  They each dissociate 100% in solution. 
D)  Nothing, other than being strong, they do not all dissociate the same in all reactions.

Question 6

Of the following, which is not a Lewis acid?

Accepted Answer

A)  H3O+ 
B)  SO3 
C)  NO2- 
D)  BF3  
E)  None of the above. 
A)  H3O+ 
B)  SO3 
C)  NO2- 
D)  BF3  
E)  None of the above.

Question 7

The equilibrium constant for the reaction
2Hg(l)+ 2Cl-(aq)+ Ni2+(aq)$\rightarrow$ Ni(s)+ Hg2Cl2(s)
Is 5.6 * 10-20 at 25$\omicron$C.Calculate the value of E$\omicron$ for a cell utilizing this reaction.

Accepted Answer

A)  +0.57 V 
B)  -0.25 V 
C)  +1.14 V 
D)  -1.14 V 
E) -0.57 V 
A)  +0.57 V 
B)  -0.25 V 
C)  +1.14 V 
D)  -1.14 V 
E) -0.57 V

Question 8

Consider the following reaction:
2Cu+(aq)$\rightarrow$ Cu(s)+ Cu2+(aq)If the standard potentials of Cu2+ and Cu+ are +0.34 and +0.52 V,Respectively,Calculate the value of E$\omicron$ for the given reaction.

Accepted Answer

A)  +0.86 V 
B)  +0.70 V 
C)  +0.18 V 
D)  -0.18 V 
E)  -0.70 V 
A)  +0.86 V 
B)  +0.70 V 
C)  +0.18 V 
D)  -0.18 V 
E)  -0.70 V

Question 9

For HF, pKa = 3.45.What is the pH of an aqueous buffer solution that is 0.100 M HF(aq)And 0.300 M KF(aq)?

Accepted Answer

A)  10.07 
B)  2.97 
C)  3.45 
D)  3.93 
E)  11.03 
A)  10.07 
B)  2.97 
C)  3.45 
D)  3.93 
E)  11.03

Question 10

Which of the following acids has the highest pKa?

Accepted Answer

A)  HClO 
B)  HClO3  
C)  HClO4 
D)  HBrO 
E)  HIO 
A)  HClO 
B)  HClO3  
C)  HClO4 
D)  HBrO 
E)  HIO

Question 11

Calculate the hydrogen ion concentration for an aqueous solution that has a pH of 3.45.

Accepted Answer

A)  0.54 M 
B)  3.5 * 10-4 M 
C)  2.8 * 10F-11  
D)  3.2 * 10-2 M 
E)  1.22 M 
A)  0.54 M 
B)  3.5 * 10-4 M 
C)  2.8 * 10F-11  
D)  3.2 * 10-2 M 
E)  1.22 M

Question 12

When a lead-acid battery discharges,sulfuric acid is produced.

Accepted Answer

A) True 
 B)False

Question 13

What is the equilibrium constant for the titration reaction involving HClO4(aq) and Ba(OH)2(aq)?

Accepted Answer

A)  1.0 * 1014 
B)  2.0 * 1014 
C)  1.0 * 107 
D)  1.0 * 10-14 
A)  1.0 * 1014 
B)  2.0 * 1014 
C)  1.0 * 107 
D)  1.0 * 10-14

Question 14

The pH of 0.50 M HNO2(aq) is 1.8.Therefore,the pH of a solution that is 0.50 M HNO2(aq)and 0.10 M KNO2(aq)is greater than 1.8.

Accepted Answer

A) True 
 B)False

Question 15

All of the following are strong bases in water except

Accepted Answer

A)  NaHCO3 
B)  CaO 
C)  Na2O 
D)  Na2SO4 
A)  NaHCO3 
B)  CaO 
C)  Na2O 
D)  Na2SO4

Question 16

Which of the following metals would be suitable to provide cathodic protection from corrosion for an iron bridge?

Accepted Answer

A)  Cu 
B)  Ni 
C)  Zn 
D)  Sn 
E)  Pb 
A)  Cu 
B)  Ni 
C)  Zn 
D)  Sn 
E)  Pb

Question 17

The standard potential of the cell
Pb(s)|PbSO4(s)|SO42-(aq)M Pb2+(aq)|Pb(s)Is +0.23 V at 25$\omicron$C.Calculate the equilibrium constant for the reaction of 1 M Pb2+(aq)With 1M SO42-(aq).

Accepted Answer

A)  3.7 * 1016  
B)  8.0 * 1017  
C)  6.0 * 107  
D)  1.7 * 10-8  
E)  7.7 * 103  
A)  3.7 * 1016  
B)  8.0 * 1017  
C)  6.0 * 107  
D)  1.7 * 10-8  
E)  7.7 * 103

Question 18

What is the pH of an aqueous solution that is 1.0 M HClO (Ka = 3.0 * 10-8) and 0.75 M NaClO?

Accepted Answer

A)  7.64 
B)  7.40 
C)  6.36 
D)  7.52 
E)  6.60 
A)  7.64 
B)  7.40 
C)  6.36 
D)  7.52 
E)  6.60

Question 19

If the pKa1 = 1.81, and pKa2 = 6.91 for a 0.05 M solution of H2SeO3, What is its [H+]?

Accepted Answer

A)  0.015 M 
B)  0.021 M 
C)  0.025 M 
D)  0.029 M 
E)  0.050 M 
A)  0.015 M 
B)  0.021 M 
C)  0.025 M 
D)  0.029 M 
E)  0.050 M

Question 20

All of the following are Lewis bases except

Accepted Answer

A)  OH- 
B)  H2O 
C)  SO3 
D)  Br- 
A)  OH- 
B)  H2O 
C)  SO3 
D)  Br-

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH₃COOH(aq) with 0.036 M NaOH(aq)? For acetic acid, K_a = 1.8 *10^-⁵.

What potential does a cell have that uses bromine to oxidize hydrogen to H⁺ under standard conditions at 298 K?

When silver ions form a coordination complex with the thiosulfate ion,the latter acts as a Lewis acid.

Consider the titration of 50.0 mL of 0.0200 M C₆H₅COOH(aq), with 0.100 M NaOH(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of base? Do not consider spectator ions.

What do the six strong acids have in common in all reactions?

Of the following, which is not a Lewis acid?

The equilibrium constant for the reaction 2Hg(l)+ 2Cl^-(aq)+ Ni²⁺(aq) $\rightarrow$ Ni(s)+ Hg₂Cl₂(s) Is 5.6 * 10^-²⁰ at 25^$\omicron$C.Calculate the value of E^$\omicron$for a cell utilizing this reaction.

Consider the following reaction: 2Cu⁺(aq) $\rightarrow$ Cu(s)+ Cu²⁺(aq)If the standard potentials of Cu²⁺ and Cu⁺ are +0.34 and +0.52 V,Respectively,Calculate the value of E^$\omicron$for the given reaction.

For HF, pK_a = 3.45.What is the pH of an aqueous buffer solution that is 0.100 M HF(aq)And 0.300 M KF(aq)?

Which of the following acids has the highest pK_a?

Calculate the hydrogen ion concentration for an aqueous solution that has a pH of 3.45.

When a lead-acid battery discharges,sulfuric acid is produced.

What is the equilibrium constant for the titration reaction involving HClO₄(aq) and Ba(OH)₂(aq)?

The pH of 0.50 M HNO₂(aq) is 1.8.Therefore,the pH of a solution that is 0.50 M HNO₂(aq)and 0.10 M KNO₂(aq)is greater than 1.8.

All of the following are strong bases in water except

Which of the following metals would be suitable to provide cathodic protection from corrosion for an iron bridge?

The standard potential of the cell Pb(s)|PbSO₄(s)|SO₄²^-(aq)M Pb²⁺(aq)|Pb(s)Is +0.23 V at 25^$\omicron$C.Calculate the equilibrium constant for the reaction of 1 M Pb²⁺(aq)With 1M SO₄²^-(aq).

What is the pH of an aqueous solution that is 1.0 M HClO (K_a = 3.0 * 10^-⁸) and 0.75 M NaClO?

If the pK_a1 = 1.81, and pK_a2 = 6.91 for a 0.05 M solution of H₂SeO₃, What is its [H⁺]?

All of the following are Lewis bases except

Atoms

Molecules

States of Matter

Thermodynamics

Equilibrium

Kinetics

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

Organic Chemistry

Filters

Exam 6: Reactions

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH3COOH(aq) with 0.036 M NaOH(aq)? For acetic acid, Ka = 1.8 *10-5.

What potential does a cell have that uses bromine to oxidize hydrogen to H+ under standard conditions at 298 K?

When silver ions form a coordination complex with the thiosulfate ion,the latter acts as a Lewis acid.

Consider the titration of 50.0 mL of 0.0200 M C6H5COOH(aq), with 0.100 M NaOH(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of base? Do not consider spectator ions.

What do the six strong acids have in common in all reactions?

Of the following, which is not a Lewis acid?

The equilibrium constant for the reaction 2Hg(l)+ 2Cl-(aq)+ Ni2+(aq) →\rightarrow→ Ni(s)+ Hg2Cl2(s) Is 5.6 * 10-20 at 25 ο\omicronο C.Calculate the value of E ο\omicronο for a cell utilizing this reaction.

Consider the following reaction: 2Cu+(aq) →\rightarrow→ Cu(s)+ Cu2+(aq)If the standard potentials of Cu2+ and Cu+ are +0.34 and +0.52 V,Respectively,Calculate the value of E ο\omicronο for the given reaction.

For HF, pKa = 3.45.What is the pH of an aqueous buffer solution that is 0.100 M HF(aq)And 0.300 M KF(aq)?

Which of the following acids has the highest pKa?

Calculate the hydrogen ion concentration for an aqueous solution that has a pH of 3.45.

When a lead-acid battery discharges,sulfuric acid is produced.

What is the equilibrium constant for the titration reaction involving HClO4(aq) and Ba(OH)2(aq)?

The pH of 0.50 M HNO2(aq) is 1.8.Therefore,the pH of a solution that is 0.50 M HNO2(aq)and 0.10 M KNO2(aq)is greater than 1.8.

All of the following are strong bases in water except

Which of the following metals would be suitable to provide cathodic protection from corrosion for an iron bridge?

The standard potential of the cell Pb(s)|PbSO4(s)|SO42-(aq)M Pb2+(aq)|Pb(s)Is +0.23 V at 25 ο\omicronο C.Calculate the equilibrium constant for the reaction of 1 M Pb2+(aq)With 1M SO42-(aq).

What is the pH of an aqueous solution that is 1.0 M HClO (Ka = 3.0 * 10-8) and 0.75 M NaClO?

If the pKa1 = 1.81, and pKa2 = 6.91 for a 0.05 M solution of H2SeO3, What is its [H+]?

All of the following are Lewis bases except

Atoms

Molecules

States of Matter

Thermodynamics

Equilibrium

Kinetics

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

Organic Chemistry

Filters

What is the concentration of acetate ion at the stoichiometric point in the titration of 0.018 M CH₃COOH(aq) with 0.036 M NaOH(aq)? For acetic acid, K_a = 1.8 *10^-⁵.

What potential does a cell have that uses bromine to oxidize hydrogen to H⁺ under standard conditions at 298 K?

Consider the titration of 50.0 mL of 0.0200 M C₆H₅COOH(aq), with 0.100 M NaOH(aq).What is the formula of the main species in the solution after the addition of 10.0 mL of base? Do not consider spectator ions.

The equilibrium constant for the reaction 2Hg(l)+ 2Cl^-(aq)+ Ni²⁺(aq) $\rightarrow$ Ni(s)+ Hg₂Cl₂(s) Is 5.6 * 10^-²⁰ at 25^$\omicron$C.Calculate the value of E^$\omicron$for a cell utilizing this reaction.

Consider the following reaction: 2Cu⁺(aq) $\rightarrow$ Cu(s)+ Cu²⁺(aq)If the standard potentials of Cu²⁺ and Cu⁺ are +0.34 and +0.52 V,Respectively,Calculate the value of E^$\omicron$for the given reaction.

For HF, pK_a = 3.45.What is the pH of an aqueous buffer solution that is 0.100 M HF(aq)And 0.300 M KF(aq)?

Which of the following acids has the highest pK_a?

What is the equilibrium constant for the titration reaction involving HClO₄(aq) and Ba(OH)₂(aq)?

The pH of 0.50 M HNO₂(aq) is 1.8.Therefore,the pH of a solution that is 0.50 M HNO₂(aq)and 0.10 M KNO₂(aq)is greater than 1.8.

The standard potential of the cell Pb(s)|PbSO₄(s)|SO₄²^-(aq)M Pb²⁺(aq)|Pb(s)Is +0.23 V at 25^$\omicron$C.Calculate the equilibrium constant for the reaction of 1 M Pb²⁺(aq)With 1M SO₄²^-(aq).

What is the pH of an aqueous solution that is 1.0 M HClO (K_a = 3.0 * 10^-⁸) and 0.75 M NaClO?

If the pK_a1 = 1.81, and pK_a2 = 6.91 for a 0.05 M solution of H₂SeO₃, What is its [H⁺]?