Question 1

Consider the following cell:
Ag(s)|Ag+(aq,0.100 M)mAg+(aq,0.100 M)|Ag(s)
What is the voltage of this cell?

Accepted Answer

A)  0 
B)  +0.0592 V 
C)  +0.0296 V 
D)  +0.80 V 
A)  0 
B)  +0.0592 V 
C)  +0.0296 V 
D)  +0.80 V A

Question 2

If $\alpha$(HSO3-) = 0.45 at pH 7.0,What are $\alpha$(H2SO3)And $\alpha$(SO32-)At this pH? For H2SO3,PKa1 and pKa2 are 1.81 and 6.91,Respectively.

Accepted Answer

A)  $\alpha$(H2SO3) = 0.225 and $\alpha$(SO32-) = 0.55 
B)  $\alpha$(H2SO3) = 0.55 and $\alpha$(SO32-) ~ 0 
C)  $\alpha$(H2SO3) ~ 0 and $\alpha$(SO32-) = 0.225 
D)  $\alpha$(H2SO3) ~ 0 and $\alpha$(SO32-) = 0.55 
E)  $\alpha$(H2SO3) = 0.45 and $\alpha$(SO32-) = 0.55 
A)  $\alpha$(H2SO3) = 0.225 and $\alpha$(SO32-) = 0.55 
B)  $\alpha$(H2SO3) = 0.55 and $\alpha$(SO32-) ~ 0 
C)  $\alpha$(H2SO3) ~ 0 and $\alpha$(SO32-) = 0.225 
D)  $\alpha$(H2SO3) ~ 0 and $\alpha$(SO32-) = 0.55 
E)  $\alpha$(H2SO3) = 0.45 and $\alpha$(SO32-) = 0.55 D

Question 3

What is the pH of an aqueous solution that is 0.10 M HCOOH (Ka =1.8 * 10-4) and 0.10 M NaHCO2?

Accepted Answer

A)  10.26 
B)  3.74 
C)  5.74 
D)  2.38 
E)  5.62 
A)  10.26 
B)  3.74 
C)  5.74 
D)  2.38 
E)  5.62 B

Question 4

A flask of 0.25 M HBrO(aq) has what pH? (pKa = 8.69)

Accepted Answer

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

Question 5

Estimate the pH of 10-7 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 6

The pH of 0.80 M benzenesulfonic acid is 0.51 .What is the percentage ionization of benzenesulfonic acid?

Accepted Answer

A)  25% 
B)  39% 
C)  51% 
D)  5.0% 
E)  64% 
A)  25% 
B)  39% 
C)  51% 
D)  5.0% 
E)  64%

Question 7

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

Question 8

The conjugate acid of HPO42- is

Accepted Answer

A)  HPO42-. 
B)  PO43-. 
C)  H2PO4-. 
D)  H3O+. 
E)  H3PO4. 
A)  HPO42-. 
B)  PO43-. 
C)  H2PO4-. 
D)  H3O+. 
E)  H3PO4.

Question 9

Which species will oxidize Cr2+ but not Mn2+?

Accepted Answer

A)  Pb4+  
B)  O3 in acidic medium 
C)  Zn2+  
D)  Fe2+  
E)  V3+  
A)  Pb4+  
B)  O3 in acidic medium 
C)  Zn2+  
D)  Fe2+  
E)  V3+

Question 10

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 11

True or false: the pH of 0.10 M and 0.40 M NaHCO3(aq) solutions is 8.31 for both?

Accepted Answer

A) True 
 B)False

Question 12

What is the pH at the half-stoichiometric point for the titration of 0.22 M HNO2(aq) with 0.10 M KOH(aq)? For HNO2,Ka = 4.3 * 10-4.

Accepted Answer

A)  2.31 
B)  7.00 
C)  2.01 
D)  3.37 
E)  2.16 
A)  2.31 
B)  7.00 
C)  2.01 
D)  3.37 
E)  2.16

Question 13

Use the following diagram of a cell to answer questions 59-64:  
-Using the cell shown above, A is a standard Ag+/Ag electrode connected to a standard hydrogen electrode (SHE).When the voltmeter reading is -0.80 V,
Which half-reaction occurs in the left-hand cell compartment?

Accepted Answer

A)  Ag(s) $\rightarrow$Ag+(aq) + e-  
B)  Ag+(aq) + e- $\rightarrow$ Ag(s) 
A)  Ag(s) $\rightarrow$Ag+(aq) + e-  
B)  Ag+(aq) + e- $\rightarrow$ Ag(s)

Question 14

A buffer contains equal concentrations of NH3(aq) and NH4Cl(aq).What is the pH of the buffer? (Kb (NH3)= 1.8 * 10-5)

Accepted Answer

A)  9.26 
B)  4.74 
C)  7.00 
D)  13.00 
A)  9.26 
B)  4.74 
C)  7.00 
D)  13.00

Question 15

What is the value of E for the following reaction?
2H+(aq,1.00 M)+ 2e- $\rightarrow$ H2(g,1.00 atm)

Accepted Answer

The answer of What is the value of E for...

Question 16

What is the main factor that determines the pH of any buffer?

Accepted Answer

The pK_a of

Question 17

Which of the following 0.10 M aqueous solutions has the lowest pH?

Accepted Answer

A)  B(OH)3  
B)  HIO 
C)  C2H5NH3Cl 
D)  C6H5OH 
A)  B(OH)3  
B)  HIO 
C)  C2H5NH3Cl 
D)  C6H5OH

Question 18

The titration curve for the titration of 0.100 M Na2CO3(aq) with 0.100 M HClO4(aq)
Is:  
The main species in the solution after the addition of 35 mL of HClO4 are

Accepted Answer

A)  HCO3-, H2CO3, Na+, and ClO4-. 
B)  H2CO3, Na+, and ClO4-. 
C)  CO32-, HCO3, Na+, and ClO4-. 
D)  CO32-, Na+, and ClO4-. 
E)  HCO3-, Na+, and ClO4-. 
A)  HCO3-, H2CO3, Na+, and ClO4-. 
B)  H2CO3, Na+, and ClO4-. 
C)  CO32-, HCO3, Na+, and ClO4-. 
D)  CO32-, Na+, and ClO4-. 
E)  HCO3-, Na+, and ClO4-.

Question 19

If $\alpha$(HSO3-) = 0.83 at pH 2.5,What are $\alpha$(H2SO3)And $\alpha$(SO32-)
At this pH? For H2SO3,PKa1 and pKa2 are 1.81 and 6.91,Respectively.

Accepted Answer

A)  $\alpha$H2SO3) ~ 0 and $\alpha$(SO32-) = 0.17 
B)  $\alpha$(H2SO3) = 0.415 and $\alpha$(SO32-) ~ 0 
C)  $\alpha$(H2SO3) = 0.0.085 and $\alpha$(SO32-) = 0.085 
D)  $\alpha$(H2SO3) = 0.17 and $\alpha$(SO32-) ~ 0 
E)  $\alpha$(H2SO3) = 0.17 and $\alpha$(SO32-) ~ 1 
A)  $\alpha$H2SO3) ~ 0 and $\alpha$(SO32-) = 0.17 
B)  $\alpha$(H2SO3) = 0.415 and $\alpha$(SO32-) ~ 0 
C)  $\alpha$(H2SO3) = 0.0.085 and $\alpha$(SO32-) = 0.085 
D)  $\alpha$(H2SO3) = 0.17 and $\alpha$(SO32-) ~ 0 
E)  $\alpha$(H2SO3) = 0.17 and $\alpha$(SO32-) ~ 1

Question 20

For the cell diagram
Cd(s)|CdSO4(aq)|Hg2SO4|Hg(l)
What reaction occurs at the cathode?

Accepted Answer

A)  CdSO4(s) + 2e-$\rarr$ 2Cd(s) + SO42-(aq) 
B)  2Hg(l) + SO42-(aq) $\rarr$ Hg2SO4(s) + 2e- 
C)  2Cd(s) + SO42-(aq) $
\rarr$ CdSO4(s) + 2e- 
D)  Hg2SO4(s) + 2e- $\rarr$ 2Hg(l) + SO42-(aq) 
E)  None of the above. 
A)  CdSO4(s) + 2e-$\rarr$ 2Cd(s) + SO42-(aq) 
B)  2Hg(l) + SO42-(aq) $\rarr$ Hg2SO4(s) + 2e- 
C)  2Cd(s) + SO42-(aq) $
\rarr$ CdSO4(s) + 2e- 
D)  Hg2SO4(s) + 2e- $\rarr$ 2Hg(l) + SO42-(aq) 
E)  None of the above.

Consider the following cell: Ag(s)|Ag⁺(aq,0.100 M)mAg⁺(aq,0.100 M)|Ag(s) What is the voltage of this cell?

If $\alpha$ (HSO₃^-) = 0.45 at pH 7.0,What are $\alpha$ (H₂SO₃)And $\alpha$ (SO₃²^-)At this pH? For H₂SO₃,PK_a1 and pK_a2 are 1.81 and 6.91,Respectively.

What is the pH of an aqueous solution that is 0.10 M HCOOH (K_a =1.8 * 10^-⁴) and 0.10 M NaHCO₂?

A flask of 0.25 M HBrO(aq) has what pH? (pK_a = 8.69)

Estimate the pH of 10^-⁷ M HClO₄(aq).

The pH of 0.80 M benzenesulfonic acid is 0.51 .What is the percentage ionization of benzenesulfonic acid?

Which of the following is the strongest acid?

The conjugate acid of HPO₄²^- is

Which species will oxidize Cr²⁺ but not Mn²⁺?

Which of the following is the weakest acid?

True or false: the pH of 0.10 M and 0.40 M NaHCO₃(aq) solutions is 8.31 for both?

What is the pH at the half-stoichiometric point for the titration of 0.22 M HNO₂(aq) with 0.10 M KOH(aq)? For HNO₂,K_a = 4.3 * 10^-⁴.

Use the following diagram of a cell to answer questions 59-64: -Using the cell shown above, A is a standard Ag⁺/Ag electrode connected to a standard hydrogen electrode (SHE).When the voltmeter reading is -0.80 V, Which half-reaction occurs in the left-hand cell compartment?

A buffer contains equal concentrations of NH₃(aq) and NH₄Cl(aq).What is the pH of the buffer? (K_b (NH₃)= 1.8 * 10^-⁵)

What is the value of E for the following reaction? 2H⁺(aq,1.00 M)+ 2e^- $\rightarrow$ H₂(g,1.00 atm)

What is the main factor that determines the pH of any buffer?

Which of the following 0.10 M aqueous solutions has the lowest pH?

The titration curve for the titration of 0.100 M Na₂CO₃(aq) with 0.100 M HClO₄(aq) Is: The main species in the solution after the addition of 35 mL of HClO₄ are

If $\alpha$ (HSO₃^-) = 0.83 at pH 2.5,What are $\alpha$ (H₂SO₃)And $\alpha$ (SO₃²^-) At this pH? For H₂SO₃,PK_a1 and pK_a2 are 1.81 and 6.91,Respectively.

For the cell diagram Cd(s)|CdSO₄(aq)|Hg₂SO₄|Hg(l) What reaction occurs at the cathode?

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Molecules

States of Matter

Thermodynamics

Equilibrium

Kinetics

The Main-Group Elements

The D-Block Elements

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Exam 6: Reactions

Consider the following cell: Ag(s)|Ag+(aq,0.100 M)mAg+(aq,0.100 M)|Ag(s) What is the voltage of this cell?

If α\alphaα (HSO3-) = 0.45 at pH 7.0,What are α\alphaα (H2SO3)And α\alphaα (SO32-)At this pH? For H2SO3,PKa1 and pKa2 are 1.81 and 6.91,Respectively.

What is the pH of an aqueous solution that is 0.10 M HCOOH (Ka =1.8 * 10-4) and 0.10 M NaHCO2?

A flask of 0.25 M HBrO(aq) has what pH? (pKa = 8.69)

Estimate the pH of 10-7 M HClO4(aq).

The pH of 0.80 M benzenesulfonic acid is 0.51 .What is the percentage ionization of benzenesulfonic acid?

Which of the following is the strongest acid?

The conjugate acid of HPO42- is

Which species will oxidize Cr2+ but not Mn2+?

Which of the following is the weakest acid?

True or false: the pH of 0.10 M and 0.40 M NaHCO3(aq) solutions is 8.31 for both?

What is the pH at the half-stoichiometric point for the titration of 0.22 M HNO2(aq) with 0.10 M KOH(aq)? For HNO2,Ka = 4.3 * 10-4.

Use the following diagram of a cell to answer questions 59-64: -Using the cell shown above, A is a standard Ag+/Ag electrode connected to a standard hydrogen electrode (SHE).When the voltmeter reading is -0.80 V, Which half-reaction occurs in the left-hand cell compartment?

A buffer contains equal concentrations of NH3(aq) and NH4Cl(aq).What is the pH of the buffer? (Kb (NH3)= 1.8 * 10-5)

What is the value of E for the following reaction? 2H+(aq,1.00 M)+ 2e- →\rightarrow→ H2(g,1.00 atm)

What is the main factor that determines the pH of any buffer?

Which of the following 0.10 M aqueous solutions has the lowest pH?

The titration curve for the titration of 0.100 M Na2CO3(aq) with 0.100 M HClO4(aq) Is: The main species in the solution after the addition of 35 mL of HClO4 are

If α\alphaα (HSO3-) = 0.83 at pH 2.5,What are α\alphaα (H2SO3)And α\alphaα (SO32-) At this pH? For H2SO3,PKa1 and pKa2 are 1.81 and 6.91,Respectively.

For the cell diagram Cd(s)|CdSO4(aq)|Hg2SO4|Hg(l) What reaction occurs at the cathode?

Atoms

Molecules

States of Matter

Thermodynamics

Equilibrium

Kinetics

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

Organic Chemistry

Filters

Consider the following cell: Ag(s)|Ag⁺(aq,0.100 M)mAg⁺(aq,0.100 M)|Ag(s) What is the voltage of this cell?

If $\alpha$ (HSO₃^-) = 0.45 at pH 7.0,What are $\alpha$ (H₂SO₃)And $\alpha$ (SO₃²^-)At this pH? For H₂SO₃,PK_a1 and pK_a2 are 1.81 and 6.91,Respectively.

What is the pH of an aqueous solution that is 0.10 M HCOOH (K_a =1.8 * 10^-⁴) and 0.10 M NaHCO₂?

A flask of 0.25 M HBrO(aq) has what pH? (pK_a = 8.69)

Estimate the pH of 10^-⁷ M HClO₄(aq).

The conjugate acid of HPO₄²^- is

Which species will oxidize Cr²⁺ but not Mn²⁺?

True or false: the pH of 0.10 M and 0.40 M NaHCO₃(aq) solutions is 8.31 for both?

What is the pH at the half-stoichiometric point for the titration of 0.22 M HNO₂(aq) with 0.10 M KOH(aq)? For HNO₂,K_a = 4.3 * 10^-⁴.

Use the following diagram of a cell to answer questions 59-64: -Using the cell shown above, A is a standard Ag⁺/Ag electrode connected to a standard hydrogen electrode (SHE).When the voltmeter reading is -0.80 V, Which half-reaction occurs in the left-hand cell compartment?

A buffer contains equal concentrations of NH₃(aq) and NH₄Cl(aq).What is the pH of the buffer? (K_b (NH₃)= 1.8 * 10^-⁵)

What is the value of E for the following reaction? 2H⁺(aq,1.00 M)+ 2e^- $\rightarrow$ H₂(g,1.00 atm)

The titration curve for the titration of 0.100 M Na₂CO₃(aq) with 0.100 M HClO₄(aq) Is: The main species in the solution after the addition of 35 mL of HClO₄ are

If $\alpha$ (HSO₃^-) = 0.83 at pH 2.5,What are $\alpha$ (H₂SO₃)And $\alpha$ (SO₃²^-) At this pH? For H₂SO₃,PK_a1 and pK_a2 are 1.81 and 6.91,Respectively.

For the cell diagram Cd(s)|CdSO₄(aq)|Hg₂SO₄|Hg(l) What reaction occurs at the cathode?