Question 1

Which of the following mixtures gives a buffer with a pH less than 7.0? For acetic acid, Ka = 1.8 * 10-5 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 aqueous acetic acid + 5.0 mL of 0.1 M NaOH(aq) 
C)  10 mL of 0.1 M aqueous acetic acid + 10 mL of 0.1 M NaOH(aq) 
D)  10 mL of 0.1 M aqueous acetic acid + 10 mL 0f 0.1 M NH3(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 aqueous acetic acid + 5.0 mL of 0.1 M NaOH(aq) 
C)  10 mL of 0.1 M aqueous acetic acid + 10 mL of 0.1 M NaOH(aq) 
D)  10 mL of 0.1 M aqueous acetic acid + 10 mL 0f 0.1 M NH3(aq) 
E)  10 mL of 0.1 M NH3(aq) + 5.0 mL of 0.1 M HCl(aq)

Question 2

The following 0.1 M aqueous solutions are arranged in order of increasing pH, with the highest pH on the far right. $$\begin{array} { | l | l | l | l | l | } 
\hline \mathrm { HClO } _ { 4 } & & \mathrm { KNO } _ { 3 } & \mathrm { KNO } _ { 2 } & \mathrm { RbOH } \
\hline
\end{array}$$
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

Question 3

The standard potential of the Cu2+/Cu electrode is +0.34 V and the standard potential of the cell
Pb(s)|Pb2+(aq)M Cu2+(aq)|Cu(s)
Is +0.47 V.What is the standard potential of the Pb2+/Pb electrode?

Accepted Answer

A)  -0.26 V 
B)  +0.81 V 
C)  -0.81V 
D) -0.13 V 
E)  +0.13 V 
A)  -0.26 V 
B)  +0.81 V 
C)  -0.81V 
D) -0.13 V 
E)  +0.13 V

Question 4

The pH of a 0.0050 M aqueous solution of calcium hydroxide is

Accepted Answer

A)  11.40 
B)  2.00 
C)  12.00 
D)  12.70 
E)  11.70 
A)  11.40 
B)  2.00 
C)  12.00 
D)  12.70 
E)  11.70

Question 5

Calculate the equilibrium constant for the reaction that occurs when nitric acid is added to the buffer HA(aq)/NaA(aq).The Ka of HA is 1.2 * 10 -5.

Accepted Answer

8.3 * 10<s

Question 6

Which species will reduce Br2 but not V3+?

Accepted Answer

A)  Ce 
B)  Zn 
C)  Cu 
D)  Cr2+  
E)  Al 
A)  Ce 
B)  Zn 
C)  Cu 
D)  Cr2+  
E)  Al

Question 7

When CaO(s) is dissolved in water,Which of the following is true?

Accepted Answer

A)  The solution contains O2-(aq), OH-(aq), and Ca2+(aq). 
B)  The solution contains CaO(aq). 
C)  CaO(s) does not dissolve in water. 
D)  The solution contains O2-(aq) and Ca2+(aq). 
E)  The solution contains OH-(aq) and Ca2+(aq). 
A)  The solution contains O2-(aq), OH-(aq), and Ca2+(aq). 
B)  The solution contains CaO(aq). 
C)  CaO(s) does not dissolve in water. 
D)  The solution contains O2-(aq) and Ca2+(aq). 
E)  The solution contains OH-(aq) and Ca2+(aq).

Question 8

The fractional composition diagram for the amino acid alanine is given below.  
 Write the structure of the dominant species at pH 1,6,and 12,respectively.

Accepted Answer

HOOC-CH(CH₃)NH

Question 9

The titration curve for the titration of 0.100 M Na2CO3(aq) with 0.100 M HClO4(aq)
Is:  
Estimate pKb2.

Accepted Answer

A)  7.6 
B)  10.3 
C)  6.4 
D)  8.5 
E)  3.7 
A)  7.6 
B)  10.3 
C)  6.4 
D)  8.5 
E)  3.7

Question 10

What is the pH at the stoichiometric point for the titration of 0.26 M CH3NH2(aq) with 0.26 M HClO4(aq)? For CH3NH2,Kb = 3.6 * 10-4.

Accepted Answer

A)  5.72 
B)  7.00 
C)  5.57 
D)  2.16 
E)  2.01 
A)  5.72 
B)  7.00 
C)  5.57 
D)  2.16 
E)  2.01

Question 11

The following compounds are available as 0.10 M aqueous solutions. $$\begin{array} { | l | l | l | } 
\hline \text { A) } \mathrm { HCl } & \text { B) aniline } & \text { C) } \mathrm { HCN } \
\hline \text { D) } \mathrm { KOH } & \text { E) methylamine } & \text { F) } \mathrm { HClO } \
\hline \text { G) } \mathrm { HClO } _ { 2 } & \text { H) } \mathrm { NaClO } _ { 2 } & \text { I) triethylamine } \
\hline
\end{array}$$ 
Pick two solutions that could be used to prepare a buffer with a pH of ~ 4.

Accepted Answer

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

Question 12

Given: S2O42-(aq) $\rightarrow$SO32-(aq),Basic solution. How many electrons appear in the balanced half-reaction?

Accepted Answer

A)  3 
B)  6 
C)  1 
D)  4 
E)  2 
A)  3 
B)  6 
C)  1 
D)  4 
E)  2

Question 13

Calculate the value of the equilibrium constant for the reaction.
AgCl(s)+ 2NH3(aq) 
$f$
Ag(NH3)2+(aq)+ Cl-(aq)
Given Ksp = 1.6 * 10-10 for silver chloride and Kf = 1.6 * 107 for the ammonia complex of Ag+ ions,
Ag(NH3)2+.

Accepted Answer

A)  1.0 * 10-17  
B)  6.3 * 109  
C)  6.3 * 10-8  
D)  1.0 * 1017  
E)  2.6 * 10-3  
A)  1.0 * 10-17  
B)  6.3 * 109  
C)  6.3 * 10-8  
D)  1.0 * 1017  
E)  2.6 * 10-3

Question 14

If 10.0 mmol of sodium hydroxide is added to 1.00 L of a buffer that is 0.200 M HClO(aq) and 0.155 M NaHClO(aq),The final concentrations of HClO(aq)
And ClO-(aq),Respectively,Are

Accepted Answer

A)  0.190 M and 0.155 M. 
B)  0.210 M and 0.155 M. 
C)  0.210 M and 0.165 M. 
D)  0.190 M and 0.165 M. 
E)  0.200 M and 0.155 M 
A)  0.190 M and 0.155 M. 
B)  0.210 M and 0.155 M. 
C)  0.210 M and 0.165 M. 
D)  0.190 M and 0.165 M. 
E)  0.200 M and 0.155 M

Question 15

What is the pKa of the conjugate acid of hydrazine,given that the pKb of hydrazine is 5.77? Write the formula of the conjugate acid of hydrazine.

Accepted Answer

Question 16

Write the proper cell diagram for the following reaction:
2AuCl(s)+ H2(g)$\rightarrow$2Au(s)+ 2H+(aq)+ 2Cl-(aq)

Accepted Answer

Question 17

A buffer contains equal concentrations of a weak acid, HA,And its conjugate base,A-.If the value of Ka for HA is 1.0 * 10-9,What is the pH of the buffer?

Accepted Answer

A)  13.0 
B)  5.0 
C)  7.0 
D)  1.0 
E)  9.0 
A)  13.0 
B)  5.0 
C)  7.0 
D)  1.0 
E)  9.0

Question 18

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

Accepted Answer

A)  CCl3COOH (pKa = 0.52) 
B)  Because all are acids, the pH is the same for all solutions. 
C)  HF (pKa = 3.45) 
D)  CH3COOH (pKa = 4.75) 
E)  H3PO4 (pKa1 = 2.12) 
A)  CCl3COOH (pKa = 0.52) 
B)  Because all are acids, the pH is the same for all solutions. 
C)  HF (pKa = 3.45) 
D)  CH3COOH (pKa = 4.75) 
E)  H3PO4 (pKa1 = 2.12)

Question 19

Calculate the equilibrium concentration of sulfurous acid in a solution labeled "0.100 M H2SO3(aq)" if pKa1 = 1.81, and pKa2 = 6.91.

Accepted Answer

A)  0.068 M 
B)  0.015 M 
C)  0.100 M 
D)  0.050 M 
E)  0.032 M 
A)  0.068 M 
B)  0.015 M 
C)  0.100 M 
D)  0.050 M 
E)  0.032 M

Question 20

Sodium is produced by electrolysis of molten sodium chloride .What are the products at the anode and cathode,Respectively?

Accepted Answer

A)  Na(l) and O2(g) 
B)  Cl-(aq) and Na2O(l) 
C)  Cl2(g) and Na2O(l) 
D)  O2(g) and Na(l) 
E)  Cl2(g) and Na(l) 
A)  Na(l) and O2(g) 
B)  Cl-(aq) and Na2O(l) 
C)  Cl2(g) and Na2O(l) 
D)  O2(g) and Na(l) 
E)  Cl2(g) and Na(l)

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

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?

The standard potential of the Cu²⁺/Cu electrode is +0.34 V and the standard potential of the cell Pb(s)|Pb²⁺(aq)M Cu²⁺(aq)|Cu(s) Is +0.47 V.What is the standard potential of the Pb²⁺/Pb electrode?

The pH of a 0.0050 M aqueous solution of calcium hydroxide is

Calculate the equilibrium constant for the reaction that occurs when nitric acid is added to the buffer HA(aq)/NaA(aq).The K_a of HA is 1.2 * 10 ^-⁵.

Which species will reduce Br₂ but not V³⁺?

When CaO(s) is dissolved in water,Which of the following is true?

The titration curve for the titration of 0.100 M Na₂CO₃(aq) with 0.100 M HClO₄(aq) Is: Estimate pK_b2.

What is the pH at the stoichiometric point for the titration of 0.26 M CH₃NH₂(aq) with 0.26 M HClO₄(aq)? For CH₃NH₂,K_b = 3.6 * 10^-⁴.

The following compounds are available as 0.10 M aqueous solutions. A) B) aniline C) D) E) methylamine F) G) H) I) triethylamine Pick two solutions that could be used to prepare a buffer with a pH of ~ 4.

Given: S₂O₄²^-(aq) $\rightarrow$ SO₃²^-(aq),Basic solution. How many electrons appear in the balanced half-reaction?

Calculate the value of the equilibrium constant for the reaction. AgCl(s)+ 2NH₃(aq) $f$ Ag(NH₃)₂+(aq)+ Cl^-(aq) Given K_sp = 1.6 * 10^-¹⁰ for silver chloride and K_f = 1.6 * 10⁷ for the ammonia complex of Ag⁺ ions, Ag(NH₃)²⁺.

If 10.0 mmol of sodium hydroxide is added to 1.00 L of a buffer that is 0.200 M HClO(aq) and 0.155 M NaHClO(aq),The final concentrations of HClO(aq) And ClO^-(aq),Respectively,Are

What is the pK_a of the conjugate acid of hydrazine,given that the pK_b of hydrazine is 5.77? Write the formula of the conjugate acid of hydrazine.

Write the proper cell diagram for the following reaction: 2AuCl(s)+ H₂(g) $\rightarrow$ 2Au(s)+ 2H⁺(aq)+ 2Cl^-(aq)

A buffer contains equal concentrations of a weak acid, HA,And its conjugate base,A^-.If the value of K_a for HA is 1.0 * 10^-⁹,What is the pH of the buffer?

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

Calculate the equilibrium concentration of sulfurous acid in a solution labeled "0.100 M H₂SO₃(aq)" if pK_a1 = 1.81, and pK_a2 = 6.91.

Sodium is produced by electrolysis of molten sodium chloride .What are the products at the anode and cathode,Respectively?

Atoms

Molecules

States of Matter

Thermodynamics

Equilibrium

Kinetics

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

Organic Chemistry

Filters

Exam 6: Reactions

Which of the following mixtures gives a buffer with a pH less than 7.0? For acetic acid, Ka = 1.8 * 10-5 and for NH3,Kb = 1.8 *10 -5.

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?

The standard potential of the Cu2+/Cu electrode is +0.34 V and the standard potential of the cell Pb(s)|Pb2+(aq)M Cu2+(aq)|Cu(s) Is +0.47 V.What is the standard potential of the Pb2+/Pb electrode?

The pH of a 0.0050 M aqueous solution of calcium hydroxide is

Calculate the equilibrium constant for the reaction that occurs when nitric acid is added to the buffer HA(aq)/NaA(aq).The Ka of HA is 1.2 * 10 -5.

Which species will reduce Br2 but not V3+?

When CaO(s) is dissolved in water,Which of the following is true?

The fractional composition diagram for the amino acid alanine is given below. Write the structure of the dominant species at pH 1,6,and 12,respectively.

The titration curve for the titration of 0.100 M Na2CO3(aq) with 0.100 M HClO4(aq) Is: Estimate pKb2.

What is the pH at the stoichiometric point for the titration of 0.26 M CH3NH2(aq) with 0.26 M HClO4(aq)? For CH3NH2,Kb = 3.6 * 10-4.

The following compounds are available as 0.10 M aqueous solutions. A) B) aniline C) D) E) methylamine F) G) H) I) triethylamine Pick two solutions that could be used to prepare a buffer with a pH of ~ 4.

Given: S2O42-(aq) →\rightarrow→ SO32-(aq),Basic solution. How many electrons appear in the balanced half-reaction?

Calculate the value of the equilibrium constant for the reaction. AgCl(s)+ 2NH3(aq) fff Ag(NH3)2+(aq)+ Cl-(aq) Given Ksp = 1.6 * 10-10 for silver chloride and Kf = 1.6 * 107 for the ammonia complex of Ag+ ions, Ag(NH3)2+.

If 10.0 mmol of sodium hydroxide is added to 1.00 L of a buffer that is 0.200 M HClO(aq) and 0.155 M NaHClO(aq),The final concentrations of HClO(aq) And ClO-(aq),Respectively,Are

What is the pKa of the conjugate acid of hydrazine,given that the pKb of hydrazine is 5.77? Write the formula of the conjugate acid of hydrazine.

Write the proper cell diagram for the following reaction: 2AuCl(s)+ H2(g) →\rightarrow→ 2Au(s)+ 2H+(aq)+ 2Cl-(aq)

A buffer contains equal concentrations of a weak acid, HA,And its conjugate base,A-.If the value of Ka for HA is 1.0 * 10-9,What is the pH of the buffer?

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

Calculate the equilibrium concentration of sulfurous acid in a solution labeled "0.100 M H2SO3(aq)" if pKa1 = 1.81, and pKa2 = 6.91.

Sodium is produced by electrolysis of molten sodium chloride .What are the products at the anode and cathode,Respectively?

Atoms

Molecules

States of Matter

Thermodynamics

Equilibrium

Kinetics

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

Organic Chemistry

Filters

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

The standard potential of the Cu²⁺/Cu electrode is +0.34 V and the standard potential of the cell Pb(s)|Pb²⁺(aq)M Cu²⁺(aq)|Cu(s) Is +0.47 V.What is the standard potential of the Pb²⁺/Pb electrode?

Calculate the equilibrium constant for the reaction that occurs when nitric acid is added to the buffer HA(aq)/NaA(aq).The K_a of HA is 1.2 * 10 ^-⁵.

Which species will reduce Br₂ but not V³⁺?

The titration curve for the titration of 0.100 M Na₂CO₃(aq) with 0.100 M HClO₄(aq) Is: Estimate pK_b2.

What is the pH at the stoichiometric point for the titration of 0.26 M CH₃NH₂(aq) with 0.26 M HClO₄(aq)? For CH₃NH₂,K_b = 3.6 * 10^-⁴.

Given: S₂O₄²^-(aq) $\rightarrow$ SO₃²^-(aq),Basic solution. How many electrons appear in the balanced half-reaction?

Calculate the value of the equilibrium constant for the reaction. AgCl(s)+ 2NH₃(aq) $f$ Ag(NH₃)₂+(aq)+ Cl^-(aq) Given K_sp = 1.6 * 10^-¹⁰ for silver chloride and K_f = 1.6 * 10⁷ for the ammonia complex of Ag⁺ ions, Ag(NH₃)²⁺.

If 10.0 mmol of sodium hydroxide is added to 1.00 L of a buffer that is 0.200 M HClO(aq) and 0.155 M NaHClO(aq),The final concentrations of HClO(aq) And ClO^-(aq),Respectively,Are

What is the pK_a of the conjugate acid of hydrazine,given that the pK_b of hydrazine is 5.77? Write the formula of the conjugate acid of hydrazine.

Write the proper cell diagram for the following reaction: 2AuCl(s)+ H₂(g) $\rightarrow$ 2Au(s)+ 2H⁺(aq)+ 2Cl^-(aq)

A buffer contains equal concentrations of a weak acid, HA,And its conjugate base,A^-.If the value of K_a for HA is 1.0 * 10^-⁹,What is the pH of the buffer?

Calculate the equilibrium concentration of sulfurous acid in a solution labeled "0.100 M H₂SO₃(aq)" if pK_a1 = 1.81, and pK_a2 = 6.91.