Question 1

Which of the following is the weakest acid?

Accepted Answer

A)  HCN (pKa = 9.31) 
B)  HIO3 (pKa = 0.77) 
C)  HF (pKa = 3.45) 
D)  CH3COOH (pKa = 4.75) 
E)  HNO2 (pKa = 3.37) 
A)  HCN (pKa = 9.31) 
B)  HIO3 (pKa = 0.77) 
C)  HF (pKa = 3.45) 
D)  CH3COOH (pKa = 4.75) 
E)  HNO2 (pKa = 3.37)

Question 2

Consider the titration of 15.0 mL of 0.200 M H3PO4(aq) with 0.200 M NaOH(aq).What is/are the major species in solution after the addition of 30.0 mL of base?

Accepted Answer

A)  OH-(aq) 
B)  H3PO4(aq) and H2PO4-(aq) 
C)  HPO42-(aq) 
D)  PO43-(aq) 
A)  OH-(aq) 
B)  H3PO4(aq) and H2PO4-(aq) 
C)  HPO42-(aq) 
D)  PO43-(aq)

Question 3

Of the following metals, which metal would be suitable to provide an iron bridge with cathodic protection from corrosion?

Accepted Answer

A)  Ni 
B)  Cu 
C)  Pb 
D)  Sn 
E)  None of the metals listed is suitable. 
A)  Ni 
B)  Cu 
C)  Pb 
D)  Sn 
E)  None of the metals listed is suitable.

Question 4

The standard voltage of the cell
Ag(s)|AgBr(s)|Br-(aq)M Ag+(aq)|Ag(s)
Is +0.73 V at 25$\omicron$C.Calculate the Ksp for AgBr.

Accepted Answer

A)  3.9 * 10-29  
B)  2.2 * 1012  
C)  2.0 * 10-15  
D)  5.1 * 1014  
E)  4.6 * 10-13  
A)  3.9 * 10-29  
B)  2.2 * 1012  
C)  2.0 * 10-15  
D)  5.1 * 1014  
E)  4.6 * 10-13

Question 5

Calculate E for the half-reaction below.
2H+(aq,1.00 * 10-5 M)+ 2e- $\rightarrow$ H2(g,1.00 atm)

Accepted Answer

A)  0 V 
B)  +0.592 V 
C)  -0.592 V 
D)  -0.296 V 
E)  +0.296 V 
A)  0 V 
B)  +0.592 V 
C)  -0.592 V 
D)  -0.296 V 
E)  +0.296 V

Question 6

The pH of 0.800 M aqueous benzenesulfonic acid is 0.51 .What is the value of Ka for benzenesulfonic acid?

Accepted Answer

A)  0.19 
B)  0.12 
C)  0.90 
D)  0.44 
E)  0.51 
A)  0.19 
B)  0.12 
C)  0.90 
D)  0.44 
E)  0.51

Question 7

Use the following to answer questions 55-58:  
-The galvanic cell shown above uses the half-cells Mg2+/Mg and Zn2+/Zn, and a salt bridge containing KCl(aq).The voltmeter gives a positive voltage reading.Identify A and write the half-reaction that occurs in that compartment.Does the size of the electrode A increase or decrease during operation of the cell? What is the voltmeter reading?

Accepted Answer

A IS Mg(S); Mg(S)@#LAT-DLM&Mg<

Question 8

What is the [H+] for a solution labeled "0.0500 M H2SO3(aq)" if pKa1 = 1.81, and pKa2 = 6.91?

Accepted Answer

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

Question 9

The following compounds are available as 0.10 M aqueous solutions. $$\begin{array} { | l | l | l | } 
\hline \text { A) pyridine } & \text { B) } \mathrm { LiClO } _ { 4 } & \text { C) } \mathrm { HClO } _ { 4 } \
\hline \text { D) } \mathrm { HClO } _ { 2 } & \text { E) } \mathrm { NaOH } & \text { F) phenol } \
\hline \text { G) triethylamine } & \text { H) } \mathrm { HClO } & \text { I) } \mathrm { NH } _ { 3 } \
\hline
\end{array}$$ 
Which two solutions could be used to prepare a buffer with a pH of ~ 9? More than one answer may be possible.

Accepted Answer

The answer of The following compounds are available as 0.10...

Question 10

Given: Zn(s) + OH-(aq)+ H2O(l)+ NO3-(aq$\rightarrow$Zn(OH)42-(aq)+ NH3(g)
If the coefficient of NO3- in the balanced equation is 1,How many electrons are transferred in the reaction?

Accepted Answer

A)  10 
B)  6 
C)  2 
D)  4 
E)  8 
A)  10 
B)  6 
C)  2 
D)  4 
E)  8

Question 11

The weak base, B,Has Kb = 3.1 × 10-4.The pH of a solution in which [B] = [BH+] is

Accepted Answer

A)  3.51 
B)  10.79 
C)  7.00 
D)  10.49 
E)  5.92 
A)  3.51 
B)  10.79 
C)  7.00 
D)  10.49 
E)  5.92

Question 12

The titration curve for the titration of 0.100 M H2SO3(aq) with 0.100 M KOH(aq) Is given below.  
The major species in solution after 75 mL of KOH(aq) Has been added are

Accepted Answer

A)  HSO3-(aq) and Na+(aq). 
B)  SO32-(aq), and Na+(aq). 
C)  SO32-(aq), OH-(aq), and Na+(aq). 
D)  H2SO3(aq), HSO3-, and Na+(aq). 
E)  HSO3-(aq), SO32-(aq), and Na+(aq). 
A)  HSO3-(aq) and Na+(aq). 
B)  SO32-(aq), and Na+(aq). 
C)  SO32-(aq), OH-(aq), and Na+(aq). 
D)  H2SO3(aq), HSO3-, and Na+(aq). 
E)  HSO3-(aq), SO32-(aq), and Na+(aq).

Question 13

Which of the following mixtures gives a buffer with a pH greater than 7.0? For HCNO, Ka = 2.2 * 10-4 and for NH3,Kb = 1.8 * 10-5.

Accepted Answer

A)  10 mL of 0.1 M NH3(aq) + 10 mL of 0.1 M HCl(aq) 
B)  10 mL of 0.1 M HCNO(aq) + 10 mL 0f 0.1 M NaOH(aq) 
C)  10 mL of 0.1 M HCNO(aq) + 5.0 mL of 0.1 M NaOH(aq) 
D)  10 mL of 0.1 M NH3(aq) + 10 ml of 0.1 M HCNO(aq) 
E)  10 mL of 0.1 M NH3(aq) + 5.0 mL of 0.1 M HCl(aq) 
A)  10 mL of 0.1 M NH3(aq) + 10 mL of 0.1 M HCl(aq) 
B)  10 mL of 0.1 M HCNO(aq) + 10 mL 0f 0.1 M NaOH(aq) 
C)  10 mL of 0.1 M HCNO(aq) + 5.0 mL of 0.1 M NaOH(aq) 
D)  10 mL of 0.1 M NH3(aq) + 10 ml of 0.1 M HCNO(aq) 
E)  10 mL of 0.1 M NH3(aq) + 5.0 mL of 0.1 M HCl(aq)

Question 14

In the determination of iron in vitamins, Fe2+ is titrated with permanganate, MnO4-,In acidic solution.The products of the reaction are Fe3+ and Mn2+.In the balanced equation,The number of electrons transferred is

Accepted Answer

A)  5 
B)  1 
C)  10 
D)  7 
A)  5 
B)  1 
C)  10 
D)  7

Question 15

Assuming no volume change on mixing,what mass of ammonium chloride should be added to 1.00 L of 0.250 M NH3(aq)to produce a buffer of pH 10.10? The molar mass of ammonium chloride is 53.49 g/mol.

Accepted Answer

Question 16

The pH of 0.010 M H3PO4(aq) is 2.24; estimate the concentration of PO43- in the solution.For H3PO4,The values of Ka1,Ka2,And Ka3 are 7.6 * 10-3,
6.2 * 10-8,And 2.1 * 10-13,Respectively.

Accepted Answer

A)  5.8 * 10-3 M 
B)  2.1 * 10-13 M 
C)  7.6 * 10-3 M 
D)  6.2 *10-8 M 
E)  2.3 * 10-18 M 
A)  5.8 * 10-3 M 
B)  2.1 * 10-13 M 
C)  7.6 * 10-3 M 
D)  6.2 *10-8 M 
E)  2.3 * 10-18 M

Question 17

What is the pH of an aqueous solution that is 0.018 M C6H5NH2 (Kb = 4.3 * 10-10) and 0.12 M C6H5NH3Cl?

Accepted Answer

A)  5.46 
B)  4.63 
C)  3.81 
D)  10.19 
E)  8.54 
A)  5.46 
B)  4.63 
C)  3.81 
D)  10.19 
E)  8.54

Question 18

Use the following:
Pb(s)|PbSO4(s)|SO42-(aq,0.60 M)M H+(aq,0.70 M)|H2(g,192.5 kPa)|Pt
In this cell,If E$\omicron$ is 0.36 V at 25$\omicron$C,What is the Nernst equation for the cell at this temperature?

Accepted Answer

A)  E = 0.36 - 0.012 85 ln[1.90/{(0.70)2(0.60)}] 
B)  E = 0.36 + 0.012 85 ln[1.90/{(0.70)2(0.60)}] 
C)  E = 0.36 + 0.012 85 ln[192.5/{(0.70)2(0.60)}] 
D)  E = 0.36 - 0.025 69 ln[192.5/{(0.70)2(0.60)}] 
E)  E = 0.36 - 0.012 85 ln[1.90/{(0.70)(0.60)}] 
A)  E = 0.36 - 0.012 85 ln[1.90/{(0.70)2(0.60)}] 
B)  E = 0.36 + 0.012 85 ln[1.90/{(0.70)2(0.60)}] 
C)  E = 0.36 + 0.012 85 ln[192.5/{(0.70)2(0.60)}] 
D)  E = 0.36 - 0.025 69 ln[192.5/{(0.70)2(0.60)}] 
E)  E = 0.36 - 0.012 85 ln[1.90/{(0.70)(0.60)}]

Question 19

What is the pH of 0.025 M (CH3)3N(aq) (Kb = 6.5 * 10-5)?

Accepted Answer

A)  11.91 
B)  12.40 
C)  11.11 
D)  8.29 
E)  9.81 
A)  11.91 
B)  12.40 
C)  11.11 
D)  8.29 
E)  9.81

Question 20

The fractional composition diagram for the amino acid alanine is shown below.   
What do the two points represent where alpha is 0.5?

Accepted Answer

The answer of The fractional composition diagram for the amino...

Which of the following is the weakest acid?

Consider the titration of 15.0 mL of 0.200 M H₃PO₄(aq) with 0.200 M NaOH(aq).What is/are the major species in solution after the addition of 30.0 mL of base?

Of the following metals, which metal would be suitable to provide an iron bridge with cathodic protection from corrosion?

The standard voltage of the cell Ag(s)|AgBr(s)|Br^-(aq)M Ag⁺(aq)|Ag(s) Is +0.73 V at 25^$\omicron$C.Calculate the K_sp for AgBr.

Calculate E for the half-reaction below. 2H⁺(aq,1.00 * 10^-⁵ M)+ 2e^- $\rightarrow$ H₂(g,1.00 atm)

The pH of 0.800 M aqueous benzenesulfonic acid is 0.51 .What is the value of K_a for benzenesulfonic acid?

What is the [H⁺] for a solution labeled "0.0500 M H₂SO₃(aq)" if pK_a1 = 1.81, and pK_a2 = 6.91?

The following compounds are available as 0.10 M aqueous solutions. A) pyridine B) C) D) E) F) phenol G) triethylamine H) I) Which two solutions could be used to prepare a buffer with a pH of ~ 9? More than one answer may be possible.

Given: Zn(s) + OH^-(aq)+ H₂O(l)+ NO₃^-(aq $\rightarrow$ Zn(OH)₄²^-(aq)+ NH₃(g) If the coefficient of NO₃^- in the balanced equation is 1,How many electrons are transferred in the reaction?

The weak base, B,Has K_b = 3.1 × 10^-⁴.The pH of a solution in which [B] = [BH⁺] is

The titration curve for the titration of 0.100 M H₂SO₃(aq) with 0.100 M KOH(aq) Is given below. The major species in solution after 75 mL of KOH(aq) Has been added are

Which of the following mixtures gives a buffer with a pH greater than 7.0? For HCNO, K_a = 2.2 * 10^-⁴ and for NH₃,K_b = 1.8 * 10^-⁵.

In the determination of iron in vitamins, Fe²⁺ is titrated with permanganate, MnO₄^-,In acidic solution.The products of the reaction are Fe³⁺ and Mn²⁺.In the balanced equation,The number of electrons transferred is

Assuming no volume change on mixing,what mass of ammonium chloride should be added to 1.00 L of 0.250 M NH₃(aq)to produce a buffer of pH 10.10? The molar mass of ammonium chloride is 53.49 g/mol.

The pH of 0.010 M H₃PO₄(aq) is 2.24; estimate the concentration of PO₄³^- in the solution.For H₃PO₄,The values of K_a1,K_a2,And K_a3 are 7.6 * 10^-³, 6.2 * 10^-⁸,And 2.1 * 10^-¹³,Respectively.

What is the pH of an aqueous solution that is 0.018 M C₆H₅NH₂ (K_b = 4.3 * 10^-¹⁰) and 0.12 M C₆H₅NH₃Cl?

Use the following: Pb(s)|PbSO₄(s)|SO₄2^-(aq,0.60 M)M H⁺(aq,0.70 M)|H₂(g,192.5 kPa)|Pt In this cell,If E^$\omicron$ is 0.36 V at 25^$\omicron$C,What is the Nernst equation for the cell at this temperature?

What is the pH of 0.025 M (CH₃)₃N(aq) (K_b = 6.5 * 10^-⁵)?

The fractional composition diagram for the amino acid alanine is shown below. $The fractional composition diagram for the amino acid alanine is shown below. What do the two points represent where alpha is 0.5?$ What do the two points represent where alpha is 0.5?

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Exam 6: Reactions

Which of the following is the weakest acid?

Consider the titration of 15.0 mL of 0.200 M H3PO4(aq) with 0.200 M NaOH(aq).What is/are the major species in solution after the addition of 30.0 mL of base?

Of the following metals, which metal would be suitable to provide an iron bridge with cathodic protection from corrosion?

The standard voltage of the cell Ag(s)|AgBr(s)|Br-(aq)M Ag+(aq)|Ag(s) Is +0.73 V at 25 ο\omicronο C.Calculate the Ksp for AgBr.

Calculate E for the half-reaction below. 2H+(aq,1.00 * 10-5 M)+ 2e- →\rightarrow→ H2(g,1.00 atm)

The pH of 0.800 M aqueous benzenesulfonic acid is 0.51 .What is the value of Ka for benzenesulfonic acid?

What is the [H+] for a solution labeled "0.0500 M H2SO3(aq)" if pKa1 = 1.81, and pKa2 = 6.91?

The following compounds are available as 0.10 M aqueous solutions. A) pyridine B) C) D) E) F) phenol G) triethylamine H) I) Which two solutions could be used to prepare a buffer with a pH of ~ 9? More than one answer may be possible.

Given: Zn(s) + OH-(aq)+ H2O(l)+ NO3-(aq →\rightarrow→ Zn(OH)42-(aq)+ NH3(g) If the coefficient of NO3- in the balanced equation is 1,How many electrons are transferred in the reaction?

The weak base, B,Has Kb = 3.1 × 10-4.The pH of a solution in which [B] = [BH+] is

The titration curve for the titration of 0.100 M H2SO3(aq) with 0.100 M KOH(aq) Is given below. The major species in solution after 75 mL of KOH(aq) Has been added are

Which of the following mixtures gives a buffer with a pH greater than 7.0? For HCNO, Ka = 2.2 * 10-4 and for NH3,Kb = 1.8 * 10-5.

In the determination of iron in vitamins, Fe2+ is titrated with permanganate, MnO4-,In acidic solution.The products of the reaction are Fe3+ and Mn2+.In the balanced equation,The number of electrons transferred is

Assuming no volume change on mixing,what mass of ammonium chloride should be added to 1.00 L of 0.250 M NH3(aq)to produce a buffer of pH 10.10? The molar mass of ammonium chloride is 53.49 g/mol.

The pH of 0.010 M H3PO4(aq) is 2.24; estimate the concentration of PO43- in the solution.For H3PO4,The values of Ka1,Ka2,And Ka3 are 7.6 * 10-3, 6.2 * 10-8,And 2.1 * 10-13,Respectively.

What is the pH of an aqueous solution that is 0.018 M C6H5NH2 (Kb = 4.3 * 10-10) and 0.12 M C6H5NH3Cl?

Use the following: Pb(s)|PbSO4(s)|SO42-(aq,0.60 M)M H+(aq,0.70 M)|H2(g,192.5 kPa)|Pt In this cell,If E ο\omicronο is 0.36 V at 25 ο\omicronο C,What is the Nernst equation for the cell at this temperature?

What is the pH of 0.025 M (CH3)3N(aq) (Kb = 6.5 * 10-5)?

The fractional composition diagram for the amino acid alanine is shown below. What do the two points represent where alpha is 0.5?

Atoms

Molecules

States of Matter

Thermodynamics

Equilibrium

Kinetics

The Main-Group Elements

The D-Block Elements

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Consider the titration of 15.0 mL of 0.200 M H₃PO₄(aq) with 0.200 M NaOH(aq).What is/are the major species in solution after the addition of 30.0 mL of base?

The standard voltage of the cell Ag(s)|AgBr(s)|Br^-(aq)M Ag⁺(aq)|Ag(s) Is +0.73 V at 25^$\omicron$C.Calculate the K_sp for AgBr.

Calculate E for the half-reaction below. 2H⁺(aq,1.00 * 10^-⁵ M)+ 2e^- $\rightarrow$ H₂(g,1.00 atm)

The pH of 0.800 M aqueous benzenesulfonic acid is 0.51 .What is the value of K_a for benzenesulfonic acid?

What is the [H⁺] for a solution labeled "0.0500 M H₂SO₃(aq)" if pK_a1 = 1.81, and pK_a2 = 6.91?

Given: Zn(s) + OH^-(aq)+ H₂O(l)+ NO₃^-(aq $\rightarrow$ Zn(OH)₄²^-(aq)+ NH₃(g) If the coefficient of NO₃^- in the balanced equation is 1,How many electrons are transferred in the reaction?

The weak base, B,Has K_b = 3.1 × 10^-⁴.The pH of a solution in which [B] = [BH⁺] is

The titration curve for the titration of 0.100 M H₂SO₃(aq) with 0.100 M KOH(aq) Is given below. The major species in solution after 75 mL of KOH(aq) Has been added are

Which of the following mixtures gives a buffer with a pH greater than 7.0? For HCNO, K_a = 2.2 * 10^-⁴ and for NH₃,K_b = 1.8 * 10^-⁵.

In the determination of iron in vitamins, Fe²⁺ is titrated with permanganate, MnO₄^-,In acidic solution.The products of the reaction are Fe³⁺ and Mn²⁺.In the balanced equation,The number of electrons transferred is

Assuming no volume change on mixing,what mass of ammonium chloride should be added to 1.00 L of 0.250 M NH₃(aq)to produce a buffer of pH 10.10? The molar mass of ammonium chloride is 53.49 g/mol.

The pH of 0.010 M H₃PO₄(aq) is 2.24; estimate the concentration of PO₄³^- in the solution.For H₃PO₄,The values of K_a1,K_a2,And K_a3 are 7.6 * 10^-³, 6.2 * 10^-⁸,And 2.1 * 10^-¹³,Respectively.

What is the pH of an aqueous solution that is 0.018 M C₆H₅NH₂ (K_b = 4.3 * 10^-¹⁰) and 0.12 M C₆H₅NH₃Cl?

Use the following: Pb(s)|PbSO₄(s)|SO₄2^-(aq,0.60 M)M H⁺(aq,0.70 M)|H₂(g,192.5 kPa)|Pt In this cell,If E^$\omicron$ is 0.36 V at 25^$\omicron$C,What is the Nernst equation for the cell at this temperature?

What is the pH of 0.025 M (CH₃)₃N(aq) (K_b = 6.5 * 10^-⁵)?

The fractional composition diagram for the amino acid alanine is shown below. $The fractional composition diagram for the amino acid alanine is shown below. What do the two points represent where alpha is 0.5?$ What do the two points represent where alpha is 0.5?