Question 1

Of the following, which does not have an amphoteric oxide?

Accepted Answer

A)  BeO 
B)  PbO 
C)  SnO 
D)  Al2O3 
E)  MgO 
A)  BeO 
B)  PbO 
C)  SnO 
D)  Al2O3 
E)  MgO

Question 2

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 ~ 7?

Accepted Answer

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

Question 3

The pH of 0.30 M CH3NH2(aq)is 12.0.Therefore,the pH of a solution that is 0.30 M CH3NH2(aq)and 0.10 M CH3NH3Cl(aq)is greater than 12.0.

Accepted Answer

A) True 
 B)False

Question 4

Given: PH3(g) $\rightarrow$P4(s),Basic solution.
How many electrons appear in the balanced half-reaction?

Accepted Answer

A)  12 
B)  9 
C)  6 
D)  8 
E)  3 
A)  12 
B)  9 
C)  6 
D)  8 
E)  3

Question 5

The conjugate base of OH- is

Accepted Answer

A)  H+. 
B)  OH-. 
C)  O2-. 
D)  H3O+. 
E)  H2O. 
A)  H+. 
B)  OH-. 
C)  O2-. 
D)  H3O+. 
E)  H2O.

Question 6

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.

Question 7

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 8

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

Accepted Answer

A)  6.9 
B)  9 
C)  13 
D)  7.2 
E)  7.0 
A)  6.9 
B)  9 
C)  13 
D)  7.2 
E)  7.0

Question 9

The equation that represents Ka2 for sulfurous acid is

Accepted Answer

A)  HSO3-(aq) + H2O(l) ? H2SO3(aq) + OH-(aq). 
B)  HSO3-(aq) + H2O(l) ? SO32-(aq) + H3O+(aq). 
C)  H2SO3(aq) + 2H2O(l) ? SO32-(aq) + 2H3O+(aq). 
D)  SO32-(aq) + H2O(l) ? HSO3-(aq) + OH-(aq). 
E)  H2SO3(aq) + H2O(l) ? HSO3-(aq) + H3O+(aq). 
A)  HSO3-(aq) + H2O(l) ? H2SO3(aq) + OH-(aq). 
B)  HSO3-(aq) + H2O(l) ? SO32-(aq) + H3O+(aq). 
C)  H2SO3(aq) + 2H2O(l) ? SO32-(aq) + 2H3O+(aq). 
D)  SO32-(aq) + H2O(l) ? HSO3-(aq) + OH-(aq). 
E)  H2SO3(aq) + H2O(l) ? HSO3-(aq) + H3O+(aq).

Question 10

A buffer solution contains 0.0200 M acetic acid and 0.0200 M sodium acetate.What is the pH after 2.0 mmol of HCl is added to 1.00 L of this buffer? pKa = 4.75 for acetic acid.

Accepted Answer

A)  4.70 
B)  4.84 
C)  4.75 
D)  4.80 
E)  4.66 
A)  4.70 
B)  4.84 
C)  4.75 
D)  4.80 
E)  4.66

Question 11

The solubility of silver chloride is greater in 0.01 M NH3(aq) because of formation of the coordination complex Ag(NH3)2+(aq).

Accepted Answer

A) True 
 B)False

Question 12

The products of the electrolysis of CuSO4(aq) are

Accepted Answer

A)  H2(g) and H2SO3(aq). 
B)  H2SO3(aq) and O2(g). 
C)  Cu(s) and H2SO3(aq). 
D)  Cu(s) and O2(g). 
E)  H2(g) and O2(g). 
A)  H2(g) and H2SO3(aq). 
B)  H2SO3(aq) and O2(g). 
C)  Cu(s) and H2SO3(aq). 
D)  Cu(s) and O2(g). 
E)  H2(g) and O2(g).

Question 13

What current is required to produce 91.6 g of chromium meta from chromium(VI)oxide in 12.4 hours?

Accepted Answer

The answer of What current is required to produce 91.6...

Question 14

When sodium nitrite is added to HNO2(aq),

Accepted Answer

A)  the equilibrium concentration of HCOOH(aq) decreases. 
B)  the pH of the solution increases. 
C)  the Ka increases. 
D)  the pH of the solution does not change. 
E)  the pH of the solution decreases. 
A)  the equilibrium concentration of HCOOH(aq) decreases. 
B)  the pH of the solution increases. 
C)  the Ka increases. 
D)  the pH of the solution does not change. 
E)  the pH of the solution decreases.

Question 15

How many electrons appear in the balanced half reaction: NO3-(aq) $\rarr$ NO(g),
In acidic solution?

Accepted Answer

A)  2 
B)  3 
C)  4 
D)  6 
E)  8 
A)  2 
B)  3 
C)  4 
D)  6 
E)  8

Question 16

Write the charge balance equation for a solution that is 0.0010 M phenol(aq) .
Let phenol be represented by HA(aq).

Accepted Answer

A)  [H3O+] = [OH-] 
B)  Kw = [H3O+][OH-] 
C)  [H3O+] = [OH-] + [A-] 
D)  Ka = Kw/Kb  
E)  0.0010 = [HA] + [A-] 
A)  [H3O+] = [OH-] 
B)  Kw = [H3O+][OH-] 
C)  [H3O+] = [OH-] + [A-] 
D)  Ka = Kw/Kb  
E)  0.0010 = [HA] + [A-]

Question 17

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 equilibrium constant for the cell reaction.

Accepted Answer

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

Question 18

Consider the reaction:
2Ag+(aq)+ Cu(s)$\rightarrow$Cu2+(aq)+ 2Ag(s)If the standard potentials of Ag+ and Cu2+ are +0.80 V and +0.34 V,Respectively,Calculate the value of E$\omicron$ for the given reaction.

Accepted Answer

A)  +1.48 V 
B)  -1.26 V 
C)  -0.46 V 
D)  +1.26 V 
E)  +0.46 V 
A)  +1.48 V 
B)  -1.26 V 
C)  -0.46 V 
D)  +1.26 V 
E)  +0.46 V

Question 19

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer B(aq)/BHCl(aq).The Kb of B is 1.5 * 10-5.

Accepted Answer

6.7 * 10<s

Question 20

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

Of the following, which does not have an amphoteric oxide?

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 ~ 7?

The pH of 0.30 M CH₃NH₂(aq)is 12.0.Therefore,the pH of a solution that is 0.30 M CH₃NH₂(aq)and 0.10 M CH₃NH₃Cl(aq)is greater than 12.0.

Given: PH₃(g) $\rightarrow$ P₄(s),Basic solution. How many electrons appear in the balanced half-reaction?

The conjugate base of OH^- is

All of the following 0.1 M aqueous solutions are acidic except

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

Estimate the pH of 10^-⁷ M KOH(aq).

The equation that represents K_a2 for sulfurous acid is

A buffer solution contains 0.0200 M acetic acid and 0.0200 M sodium acetate.What is the pH after 2.0 mmol of HCl is added to 1.00 L of this buffer? pK_a = 4.75 for acetic acid.

The solubility of silver chloride is greater in 0.01 M NH₃(aq) because of formation of the coordination complex Ag(NH₃)₂⁺(aq).

The products of the electrolysis of CuSO₄(aq) are

What current is required to produce 91.6 g of chromium meta from chromium(VI)oxide in 12.4 hours?

When sodium nitrite is added to HNO₂(aq),

How many electrons appear in the balanced half reaction: NO₃^-(aq) $\rarr$ NO(g), In acidic solution?

Write the charge balance equation for a solution that is 0.0010 M phenol(aq) . Let phenol be represented by HA(aq).

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 equilibrium constant for the cell reaction.

Consider the reaction: 2Ag⁺(aq)+ Cu(s) $\rightarrow$ Cu²⁺(aq)+ 2Ag(s)If the standard potentials of Ag⁺ and Cu²⁺ are +0.80 V and +0.34 V,Respectively,Calculate the value of E^$\omicron$for the given reaction.

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer B(aq)/BHCl(aq).The K_b of B is 1.5 * 10^-⁵.

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?

Atoms

Molecules

States of Matter

Thermodynamics

Equilibrium

Kinetics

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

Organic Chemistry

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Exam 6: Reactions

Of the following, which does not have an amphoteric oxide?

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 ~ 7?

The pH of 0.30 M CH3NH2(aq)is 12.0.Therefore,the pH of a solution that is 0.30 M CH3NH2(aq)and 0.10 M CH3NH3Cl(aq)is greater than 12.0.

Given: PH3(g) →\rightarrow→ P4(s),Basic solution. How many electrons appear in the balanced half-reaction?

The conjugate base of OH- is

All of the following 0.1 M aqueous solutions are acidic except

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

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

The equation that represents Ka2 for sulfurous acid is

A buffer solution contains 0.0200 M acetic acid and 0.0200 M sodium acetate.What is the pH after 2.0 mmol of HCl is added to 1.00 L of this buffer? pKa = 4.75 for acetic acid.

The solubility of silver chloride is greater in 0.01 M NH3(aq) because of formation of the coordination complex Ag(NH3)2+(aq).

The products of the electrolysis of CuSO4(aq) are

What current is required to produce 91.6 g of chromium meta from chromium(VI)oxide in 12.4 hours?

When sodium nitrite is added to HNO2(aq),

How many electrons appear in the balanced half reaction: NO3-(aq) →\rarr→ NO(g), In acidic solution?

Write the charge balance equation for a solution that is 0.0010 M phenol(aq) . Let phenol be represented by HA(aq).

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 equilibrium constant for the cell reaction.

Consider the reaction: 2Ag+(aq)+ Cu(s) →\rightarrow→ Cu2+(aq)+ 2Ag(s)If the standard potentials of Ag+ and Cu2+ are +0.80 V and +0.34 V,Respectively,Calculate the value of E ο\omicronο for the given reaction.

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer B(aq)/BHCl(aq).The Kb of B is 1.5 * 10-5.

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?

Atoms

Molecules

States of Matter

Thermodynamics

Equilibrium

Kinetics

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

Organic Chemistry

Filters

The pH of 0.30 M CH₃NH₂(aq)is 12.0.Therefore,the pH of a solution that is 0.30 M CH₃NH₂(aq)and 0.10 M CH₃NH₃Cl(aq)is greater than 12.0.

Given: PH₃(g) $\rightarrow$ P₄(s),Basic solution. How many electrons appear in the balanced half-reaction?

The conjugate base of OH^- is

Estimate the pH of 10^-⁷ M KOH(aq).

The equation that represents K_a2 for sulfurous acid is

A buffer solution contains 0.0200 M acetic acid and 0.0200 M sodium acetate.What is the pH after 2.0 mmol of HCl is added to 1.00 L of this buffer? pK_a = 4.75 for acetic acid.

The solubility of silver chloride is greater in 0.01 M NH₃(aq) because of formation of the coordination complex Ag(NH₃)₂⁺(aq).

The products of the electrolysis of CuSO₄(aq) are

When sodium nitrite is added to HNO₂(aq),

How many electrons appear in the balanced half reaction: NO₃^-(aq) $\rarr$ NO(g), In acidic solution?

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 equilibrium constant for the cell reaction.

Consider the reaction: 2Ag⁺(aq)+ Cu(s) $\rightarrow$ Cu²⁺(aq)+ 2Ag(s)If the standard potentials of Ag⁺ and Cu²⁺ are +0.80 V and +0.34 V,Respectively,Calculate the value of E^$\omicron$for the given reaction.

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer B(aq)/BHCl(aq).The K_b of B is 1.5 * 10^-⁵.

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?