Question 1

Calculate E$\omicron$ for the following cell.
Zn(s)|Zn2+(aq)MCl-(aq)|AgCl(s)|Ag(s)

Accepted Answer

A)  +0.54 V 
B)  +1.20 V 
C)  1.20 V 
D)  +0.98 V 
E)  0.54 V 
A)  +0.54 V 
B)  +1.20 V 
C)  1.20 V 
D)  +0.98 V 
E)  0.54 V

Question 2

For the reduction of Cu2+ by Zn,
$\Delta$Go = -212 kJ/mol and Eo = +1.10 V.If the coefficients in the chemical equation for this reaction are multiplied by 2,$\Delta$Go = -424 kJ/mol.This means Eo = +2.20 V.

Accepted Answer

A) True 
 B)False

Question 3

At the stoichiometric point in the titration of 0.260 M CH3NH2(aq) with 0.260 M HCl(aq),

Accepted Answer

A)  the pH is less than 7. 
B)  [CH3NH3+] = 0.260 M. 
C)  the pH is 7.0. 
D)  [CH3NH2] = 0.130 M. 
E)  the pH is greater than 7. 
A)  the pH is less than 7. 
B)  [CH3NH3+] = 0.260 M. 
C)  the pH is 7.0. 
D)  [CH3NH2] = 0.130 M. 
E)  the pH is greater than 7.

Question 4

The standard potential of the cell
Ag(s)|AgCl(s)MCl-(aq|Cu2+(aq)|Cu(s)
Is +0.12 V at 25S1U1P1$\circ$S1S1P0C.If the standard potential of the Cu2+/Cu couple is +0.34 V,
Calculate the standard potential of the AgCl/Ag,Cl-couple.

Accepted Answer

A)  -0.12 V 
B)  -0.46 V 
C)  +0.46 V 
D)  0.22 V 
E)  +0.22 V 
A)  -0.12 V 
B)  -0.46 V 
C)  +0.46 V 
D)  0.22 V 
E)  +0.22 V

Question 5

In a solution labeled "0.0018 M barium hydroxide" what is the molarity of OH-?

Accepted Answer

A)  0.0018 M 
B)  0.00090 M 
C)  0.0036 M 
D)  0.0072 M 
E)  None of the above. 
A)  0.0018 M 
B)  0.00090 M 
C)  0.0036 M 
D)  0.0072 M 
E)  None of the above.

Question 6

In the titration of 0.300 M CH3NH2(aq)with 0.300 M HCl(aq),what is the formula of the major species and what is its concentration at the equivalence point?

Accepted Answer

CH₃NH₃⁺(aq);

Question 7

Write the charge balance equation for a dilute aqueous solution of KOH.

Accepted Answer

A)  [KOH]initial = [K+] 
B)  [OH-] = [H3O+] + [K+] 
C)  [H3O+] = [OH-] 
D)  [K+] = [OH-] + [H3O+] 
E)  [OH-] = [K+] 
A)  [KOH]initial = [K+] 
B)  [OH-] = [H3O+] + [K+] 
C)  [H3O+] = [OH-] 
D)  [K+] = [OH-] + [H3O+] 
E)  [OH-] = [K+]

Question 8

The equation that represents Ka2 for phosphoric acid is

Accepted Answer

A)  HPO42-(aq) + H2O(l) ? PO43-(aq) + H3O+(aq) 
B)  H2PO4-(aq) + H2O(l) ? HPO42-(aq) + H3O+(aq). 
C)  H3PO4(aq) + 2H2O(l) ? HPO42-(aq) + 2H3O+(aq). 
D)  HPO42-(aq) + H2O(l) ? H2PO4-(aq) + OH-(aq). 
E)  H3PO4(aq) + H2O(l) ? H2PO4-(aq) + H3O+(aq). 
A)  HPO42-(aq) + H2O(l) ? PO43-(aq) + H3O+(aq) 
B)  H2PO4-(aq) + H2O(l) ? HPO42-(aq) + H3O+(aq). 
C)  H3PO4(aq) + 2H2O(l) ? HPO42-(aq) + 2H3O+(aq). 
D)  HPO42-(aq) + H2O(l) ? H2PO4-(aq) + OH-(aq). 
E)  H3PO4(aq) + H2O(l) ? H2PO4-(aq) + H3O+(aq).

Question 9

The Ksp for mercury(I) iodide is 1.2 *10-28.What is the solubility of mercury(I) Iodide?

Accepted Answer

A)  3.9 *10 -10 
B)  1.1 *10-14 
C)  5.2 *10-8 
D)  3.1 *10-10 
A)  3.9 *10 -10 
B)  1.1 *10-14 
C)  5.2 *10-8 
D)  3.1 *10-10

Question 10

Galvanized iron is protected from corrosion because zinc reduces any Fe2+ formed.

Accepted Answer

A) True 
 B)False

Question 11

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

Accepted Answer

A)  3.2 * 10-2 M 
B)  0.54 M 
C)  3.5 * 10-4 M 
D)  2.8 * 10-11 M 
E)  2.6 *10-5 M 
A)  3.2 * 10-2 M 
B)  0.54 M 
C)  3.5 * 10-4 M 
D)  2.8 * 10-11 M 
E)  2.6 *10-5 M

Question 12

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer HA(aq)/NaA(aq).The Ka of HA is 4.1 * 10-5.

Accepted Answer

4.1 * 10<s

Question 13

Bond polarity tends to dominate the trend of acid strengths for binary acids of elements of the same period.

Accepted Answer

A) True 
 B)False

Question 14

How many moles of O2(g) are produced by electrolysis of Na2SO4(aq)
If 0.120 A is passed through the solution for 65.0 min?

Accepted Answer

A)  0.001 21 mol 
B)  0.000 080 8 mol 
C)  0.002 42 mol 
D)  0.004 85 mol 
E)  0.000 020 2 mol 
A)  0.001 21 mol 
B)  0.000 080 8 mol 
C)  0.002 42 mol 
D)  0.004 85 mol 
E)  0.000 020 2 mol

Question 15

What is the pH at the stoichiometric point for the titration of 0.100 M CH3COOH(aq) with 0.100 M KOH(aq)? The value of Ka for acetic acid is 1.8 * 10-5.

Accepted Answer

A)  5.28 
B)  8.72 
C)  7.00 
D)  9.26 
E)  8.89 
A)  5.28 
B)  8.72 
C)  7.00 
D)  9.26 
E)  8.89

Question 16

Use the following diagram of a cell to answer questions 59-64:  
-In the cell shown above,A is a standard Ag+/Ag electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is +0.80 V,which electrode is negative?

Accepted Answer

Question 17

The amino acid alanine,HOOC-CH(CH3)NH3+,Has Ka1 = 4.5 * 10-3 and Ka2 = 1.4 * 10-10.Calculate$\alpha$(-OOC-CH(CH3)NH3+)At pH 10.

Accepted Answer

A)  0.42 
B)  0.29 
C)  1.0 
D)  0 
E)  0.58 
A)  0.42 
B)  0.29 
C)  1.0 
D)  0 
E)  0.58

Question 18

At the stoichiometric point in the titration of 0.130 M HCOOH(aq) with 0.130 M KOH(aq),

Accepted Answer

A)  the pH is 7.0. 
B)  [HCOOH] = 0.0650 M. 
C)  [HCO2-] = 0.130 M. 
D)  the pH is greater than 7. 
E)  the pH is less than 7. 
A)  the pH is 7.0. 
B)  [HCOOH] = 0.0650 M. 
C)  [HCO2-] = 0.130 M. 
D)  the pH is greater than 7. 
E)  the pH is less than 7.

Question 19

The following 0.1 M aqueous solutions are arranged in order of increasing pH, with the highest pH on the far right. $$\begin{array} { | l | l | l | l | l | } 
\hline \mathrm { HNO } _ { 3 } & \mathrm { C } _ { 5 } \mathrm { H } _ { 5 } \mathrm { NHCl } & \mathrm { HClO } & & \mathrm { NaClO } \
\hline
\end{array}$$
Which one of the following 0.10 M aqueous solutions should be placed in the empty box?

Accepted Answer

A)  NH4Cl 
B)  NaCN 
C)  Al2(SO4)3  
D)  CH3NH2  
E)  CH3COOH 
A)  NH4Cl 
B)  NaCN 
C)  Al2(SO4)3  
D)  CH3NH2  
E)  CH3COOH

Question 20

If the standard potential for Ti3+(aq)/Ti2+(aq) is -0.37 V and the standard potential for Ti2+(aq)/Ti(s)Is -1.63 V,Calculate the standard potential for
Ti3+(aq)+ 3e- $\rightarrow$ Ti(s).

Accepted Answer

A)  -1.19 V 
B)  -0.40 V 
C)  -2.00 V 
D)  -1.26 V 
E)  -1.21 V 
A)  -1.19 V 
B)  -0.40 V 
C)  -2.00 V 
D)  -1.26 V 
E)  -1.21 V

Calculate E^$\omicron$ for the following cell. Zn(s)|Zn²⁺(aq)MCl^-(aq)|AgCl(s)|Ag(s)

For the reduction of Cu²⁺ by Zn, $\Delta$ G^o = -212 kJ/mol and E^o = +1.10 V.If the coefficients in the chemical equation for this reaction are multiplied by 2, $\Delta$ G^o = -424 kJ/mol.This means E^o = +2.20 V.

At the stoichiometric point in the titration of 0.260 M CH₃NH₂(aq) with 0.260 M HCl(aq),

The standard potential of the cell Ag(s)|AgCl(s)MCl^-(aq|Cu²⁺(aq)|Cu(s) Is +0.12 V at 25^$\circ$C.If the standard potential of the Cu²⁺/Cu couple is +0.34 V, Calculate the standard potential of the AgCl/Ag,Cl^-couple.

In a solution labeled "0.0018 M barium hydroxide" what is the molarity of OH^-?

In the titration of 0.300 M CH₃NH₂(aq)with 0.300 M HCl(aq),what is the formula of the major species and what is its concentration at the equivalence point?

Write the charge balance equation for a dilute aqueous solution of KOH.

The equation that represents K_a2 for phosphoric acid is

The K_spfor mercury(I) iodide is 1.2 *10^{^-28}.What is the solubility of mercury(I) Iodide?

Galvanized iron is protected from corrosion because zinc reduces any Fe²⁺ formed.

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

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer HA(aq)/NaA(aq).The K_a of HA is 4.1 * 10^-⁵.

Bond polarity tends to dominate the trend of acid strengths for binary acids of elements of the same period.

How many moles of O₂(g) are produced by electrolysis of Na₂SO₄(aq) If 0.120 A is passed through the solution for 65.0 min?

What is the pH at the stoichiometric point for the titration of 0.100 M CH₃COOH(aq) with 0.100 M KOH(aq)? The value of K_a for acetic acid is 1.8 * 10^-⁵.

Use the following diagram of a cell to answer questions 59-64: -In the cell shown above,A is a standard Ag⁺/Ag electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is +0.80 V,which electrode is negative?

The amino acid alanine,HOOC-CH(CH₃)NH₃⁺,Has K_a1 = 4.5 * 10^-³ and K_a2 = 1.4 * 10^-¹⁰.Calculate $\alpha$ (^-OOC-CH(CH₃)NH₃⁺)At pH 10.

At the stoichiometric point in the titration of 0.130 M HCOOH(aq) with 0.130 M KOH(aq),

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?

If the standard potential for Ti³⁺(aq)/Ti²⁺(aq) is -0.37 V and the standard potential for Ti²⁺(aq)/Ti(s)Is -1.63 V,Calculate the standard potential for Ti³⁺(aq)+ 3e^- $\rightarrow$ Ti(s).

Atoms

Molecules

States of Matter

Thermodynamics

Equilibrium

Kinetics

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

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Exam 6: Reactions

Calculate E ο\omicronο for the following cell. Zn(s)|Zn2+(aq)MCl-(aq)|AgCl(s)|Ag(s)

For the reduction of Cu2+ by Zn, Δ\DeltaΔ Go = -212 kJ/mol and Eo = +1.10 V.If the coefficients in the chemical equation for this reaction are multiplied by 2, Δ\DeltaΔ Go = -424 kJ/mol.This means Eo = +2.20 V.

At the stoichiometric point in the titration of 0.260 M CH3NH2(aq) with 0.260 M HCl(aq),

The standard potential of the cell Ag(s)|AgCl(s)MCl-(aq|Cu2+(aq)|Cu(s) Is +0.12 V at 25 ∘\circ∘ C.If the standard potential of the Cu2+/Cu couple is +0.34 V, Calculate the standard potential of the AgCl/Ag,Cl-couple.

In a solution labeled "0.0018 M barium hydroxide" what is the molarity of OH-?

In the titration of 0.300 M CH3NH2(aq)with 0.300 M HCl(aq),what is the formula of the major species and what is its concentration at the equivalence point?

Write the charge balance equation for a dilute aqueous solution of KOH.

The equation that represents Ka2 for phosphoric acid is

The Ksp for mercury(I) iodide is 1.2 *10-28.What is the solubility of mercury(I) Iodide?

Galvanized iron is protected from corrosion because zinc reduces any Fe2+ formed.

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

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer HA(aq)/NaA(aq).The Ka of HA is 4.1 * 10-5.

Bond polarity tends to dominate the trend of acid strengths for binary acids of elements of the same period.

How many moles of O2(g) are produced by electrolysis of Na2SO4(aq) If 0.120 A is passed through the solution for 65.0 min?

What is the pH at the stoichiometric point for the titration of 0.100 M CH3COOH(aq) with 0.100 M KOH(aq)? The value of Ka for acetic acid is 1.8 * 10-5.

Use the following diagram of a cell to answer questions 59-64: -In the cell shown above,A is a standard Ag+/Ag electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is +0.80 V,which electrode is negative?

The amino acid alanine,HOOC-CH(CH3)NH3+,Has Ka1 = 4.5 * 10-3 and Ka2 = 1.4 * 10-10.Calculate α\alphaα (-OOC-CH(CH3)NH3+)At pH 10.

At the stoichiometric point in the titration of 0.130 M HCOOH(aq) with 0.130 M KOH(aq),

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?

If the standard potential for Ti3+(aq)/Ti2+(aq) is -0.37 V and the standard potential for Ti2+(aq)/Ti(s)Is -1.63 V,Calculate the standard potential for Ti3+(aq)+ 3e- →\rightarrow→ Ti(s).

Atoms

Molecules

States of Matter

Thermodynamics

Equilibrium

Kinetics

The Main-Group Elements

The D-Block Elements

Nuclear Chemistry

Organic Chemistry

Filters

Calculate E^$\omicron$ for the following cell. Zn(s)|Zn²⁺(aq)MCl^-(aq)|AgCl(s)|Ag(s)

For the reduction of Cu²⁺ by Zn, $\Delta$ G^o = -212 kJ/mol and E^o = +1.10 V.If the coefficients in the chemical equation for this reaction are multiplied by 2, $\Delta$ G^o = -424 kJ/mol.This means E^o = +2.20 V.

At the stoichiometric point in the titration of 0.260 M CH₃NH₂(aq) with 0.260 M HCl(aq),

The standard potential of the cell Ag(s)|AgCl(s)MCl^-(aq|Cu²⁺(aq)|Cu(s) Is +0.12 V at 25^$\circ$C.If the standard potential of the Cu²⁺/Cu couple is +0.34 V, Calculate the standard potential of the AgCl/Ag,Cl^-couple.

In a solution labeled "0.0018 M barium hydroxide" what is the molarity of OH^-?

In the titration of 0.300 M CH₃NH₂(aq)with 0.300 M HCl(aq),what is the formula of the major species and what is its concentration at the equivalence point?

The equation that represents K_a2 for phosphoric acid is

The K_spfor mercury(I) iodide is 1.2 *10^{^-28}.What is the solubility of mercury(I) Iodide?

Galvanized iron is protected from corrosion because zinc reduces any Fe²⁺ formed.

Calculate the equilibrium constant for the reaction that occurs when sodium hydroxide is added to the buffer HA(aq)/NaA(aq).The K_a of HA is 4.1 * 10^-⁵.

How many moles of O₂(g) are produced by electrolysis of Na₂SO₄(aq) If 0.120 A is passed through the solution for 65.0 min?

What is the pH at the stoichiometric point for the titration of 0.100 M CH₃COOH(aq) with 0.100 M KOH(aq)? The value of K_a for acetic acid is 1.8 * 10^-⁵.

Use the following diagram of a cell to answer questions 59-64: -In the cell shown above,A is a standard Ag⁺/Ag electrode connected to a standard hydrogen electrode (SHE).If the voltmeter reading is +0.80 V,which electrode is negative?

The amino acid alanine,HOOC-CH(CH₃)NH₃⁺,Has K_a1 = 4.5 * 10^-³ and K_a2 = 1.4 * 10^-¹⁰.Calculate $\alpha$ (^-OOC-CH(CH₃)NH₃⁺)At pH 10.

If the standard potential for Ti³⁺(aq)/Ti²⁺(aq) is -0.37 V and the standard potential for Ti²⁺(aq)/Ti(s)Is -1.63 V,Calculate the standard potential for Ti³⁺(aq)+ 3e^- $\rightarrow$ Ti(s).