Question 1

In a solution that is labeled "0.10 M H3PO4(aq)," [H3O+] = 0.024 M.Match the species below with their concentrations.

Accepted Answer

[H₃PO₄] = 8.0 * 10

Question 2

In the following reaction
SO2(g)+ H2O(l)$\rightarrow$ H2SO3(aq),
identify the Lewis acid and base.

Accepted Answer

Lewis acid,SO<sub>2<

Question 3

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?

Accepted Answer

A) CuSO4  
B) NaNO2  
C) CH3NH2  
D) NaHCO3  
E) Na2HPO4  
A) CuSO4  
B) NaNO2  
C) CH3NH2  
D) NaHCO3  
E) Na2HPO4

Question 4

The pH of 0.10 M solution and 0.35 M solution of NaHCO3(aq)must differ for each solution.

Accepted Answer

A) True 
 B)False

Question 5

What is the molarity of OH- in a 0.0018 M calcium hydroxide solution?

Accepted Answer

A) 0.0009 M 
B) 0.0036 M 
C) 0.0018 M 
D) 0.0072 M 
E) None of the above. 
A) 0.0009 M 
B) 0.0036 M 
C) 0.0018 M 
D) 0.0072 M 
E) None of the above.

Question 6

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 7

Of the following,which is not a Lewis acid?

Accepted Answer

A) H3O+ 
B) SO3 
C) NO2- 
D) BF3  
E) None of the above. 
A) H3O+ 
B) SO3 
C) NO2- 
D) BF3  
E) None of the above.

Question 8

Calculate the equilibrium constant for the reaction S2-(aq)+ H2O(l)↔ HS-(aq)+ OH-(aq),
Given Ka1 = 1.3 * 10-7 and Ka2 = 7.1 * 10-15 for H2S.

Accepted Answer

A) 1.3 * 10-7  
B) 9.2 * 10-22  
C) 7.7 * 10-8  
D) 7.1 * 10-15  
E) 1.4 
A) 1.3 * 10-7  
B) 9.2 * 10-22  
C) 7.7 * 10-8  
D) 7.1 * 10-15  
E) 1.4

Question 9

In a solution labeled "0.10 M HNO3," which of the following is correct?

Accepted Answer

A) [HNO3] = 0.10 M 
B) [H3O+] = 0.10 M,[NO3-] = 0.10 M 
C) [H3O+] = 0.090 M,[NO3-] = 0.010 M 
D) [HNO3] = 0.050 M,[H3O+] = 0.050 M,[NO3-] = 0.050 M 
E) [H3O+] = 0.10 M,[OH-] = 1.0 * 10-7 M 
A) [HNO3] = 0.10 M 
B) [H3O+] = 0.10 M,[NO3-] = 0.10 M 
C) [H3O+] = 0.090 M,[NO3-] = 0.010 M 
D) [HNO3] = 0.050 M,[H3O+] = 0.050 M,[NO3-] = 0.050 M 
E) [H3O+] = 0.10 M,[OH-] = 1.0 * 10-7 M

Question 10

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 11

The pH of 0.010 M H3PO4(aq)is 2.24.Estimate the concentration of HPO42- 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) 7.6 * 10-3 M 
C) 0.010 M 
D) 6.2 * 10-8 M 
E) 2.1 *10-13 M 
A) 5.8 * 10-3 M 
B) 7.6 * 10-3 M 
C) 0.010 M 
D) 6.2 * 10-8 M 
E) 2.1 *10-13 M

Question 12

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 13

The pH of 0.10 M pyridine(aq)is 9.13.What is the value of Kb for pyridine?

Accepted Answer

A) 2.7 * 10-4  
B) 7.4 * 10-10  
C) 2.7 * 10-5  
D) 1.8 * 10-10  
E) 1.8 * 10-9  
A) 2.7 * 10-4  
B) 7.4 * 10-10  
C) 2.7 * 10-5  
D) 1.8 * 10-10  
E) 1.8 * 10-9

Question 14

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

In a solution that is labeled "0.10 M H₃PO₄(aq)," [H₃O⁺] = 0.024 M.Match the species below with their concentrations.

In the following reaction SO₂(g)+ H₂O(l) $\rightarrow$ H₂SO₃(aq), identify the Lewis acid and base.

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 pH of 0.10 M solution and 0.35 M solution of NaHCO₃(aq)must differ for each solution.

What is the molarity of OH^- in a 0.0018 M calcium hydroxide solution?

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

Of the following,which is not a Lewis acid?

Calculate the equilibrium constant for the reaction S^2-(aq)+ H₂O(l)↔ HS^-(aq)+ OH^-(aq), Given K_a1 = 1.3 * 10^-7 and K_a2 = 7.1 * 10^-15 for H₂S.

In a solution labeled "0.10 M HNO₃," which of the following is correct?

Estimate the pH of 10^-7 M HClO₄(aq).

The pH of 0.010 M H₃PO₄(aq)is 2.24.Estimate the concentration of HPO₄²^- 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.

Which of the following is the weakest acid?

The pH of 0.10 M pyridine(aq)is 9.13.What is the value of K_bfor pyridine?

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.

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Physical Equilibria

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Exam 12: Acids and Bases

In a solution that is labeled "0.10 M H3PO4(aq)," [H3O+] = 0.024 M.Match the species below with their concentrations.

In the following reaction SO2(g)+ H2O(l) →\rightarrow→ H2SO3(aq), identify the Lewis acid and base.

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 pH of 0.10 M solution and 0.35 M solution of NaHCO3(aq)must differ for each solution.

What is the molarity of OH- in a 0.0018 M calcium hydroxide solution?

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

Of the following,which is not a Lewis acid?

Calculate the equilibrium constant for the reaction S2-(aq)+ H2O(l)↔ HS-(aq)+ OH-(aq), Given Ka1 = 1.3 * 10-7 and Ka2 = 7.1 * 10-15 for H2S.

In a solution labeled "0.10 M HNO3," which of the following is correct?

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

The pH of 0.010 M H3PO4(aq)is 2.24.Estimate the concentration of HPO42- 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.

Which of the following is the weakest acid?

The pH of 0.10 M pyridine(aq)is 9.13.What is the value of Kb for pyridine?

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.

The Quantum World

Quantum Mechanics in Action: Atoms

Chemical Bonds

Molecular Shape and Structure

The Properties of Gases

Liquids and Solids

Inorganic Materials

Thermodynamics: The First Law

Thermodynamics: The Second and Third Laws

Physical Equilibria

Chemical Equilibria

Aqueous Equilibria

Electrochemistry

Chemical Kinetics

The Elements: the Main Group Elements

The Elements: The D Block

Nuclear Chemistry

Organic Chemistry I

Organic Chemistry II

Filters

In a solution that is labeled "0.10 M H₃PO₄(aq)," [H₃O⁺] = 0.024 M.Match the species below with their concentrations.

In the following reaction SO₂(g)+ H₂O(l) $\rightarrow$ H₂SO₃(aq), identify the Lewis acid and base.

The pH of 0.10 M solution and 0.35 M solution of NaHCO₃(aq)must differ for each solution.

What is the molarity of OH^- in a 0.0018 M calcium hydroxide solution?

Calculate the equilibrium constant for the reaction S^2-(aq)+ H₂O(l)↔ HS^-(aq)+ OH^-(aq), Given K_a1 = 1.3 * 10^-7 and K_a2 = 7.1 * 10^-15 for H₂S.

In a solution labeled "0.10 M HNO₃," which of the following is correct?

Estimate the pH of 10^-7 M HClO₄(aq).

The pH of 0.010 M H₃PO₄(aq)is 2.24.Estimate the concentration of HPO₄²^- 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.

The pH of 0.10 M pyridine(aq)is 9.13.What is the value of K_bfor pyridine?

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.