Question 1

The solubility of La(IO3)3 in a 0.10 M KIO3 solution is 1.0 × 10-7 mol/L. Calculate Ksp for La(IO3)3.

Accepted Answer

A)  2.7 × 10-9 
B)  2.7 × 10-27 
C)  1.0 × 10-8 
D)  1.0 × 10-10 
E)  none of these 
A)  2.7 × 10-9 
B)  2.7 × 10-27 
C)  1.0 × 10-8 
D)  1.0 × 10-10 
E)  none of these

Question 2

The observed solubility of the salt MX in 4.0 M strong acid is 2.30 × 10-3 M. The Ka value for the acid HX is 1.00 × 10-9. Calculate the value of Ksp for the salt MX.

Accepted Answer

A)  1.3 × 103 
B)  1.3 × 10-15 
C)  5.3 × 10-6 
D)  1.3 × 10-6 
E)  5.3 × 10-15 
A)  1.3 × 103 
B)  1.3 × 10-15 
C)  5.3 × 10-6 
D)  1.3 × 10-6 
E)  5.3 × 10-15

Question 3

Which of the following is a major species present at point IV?

Accepted Answer

A)  As2- 
B)  H+ 
C)  H2As 
D)  HAs- 
E)  none of these 
A)  As2- 
B)  H+ 
C)  H2As 
D)  HAs- 
E)  none of these

Question 4

The concentration of Ag+ in a saturated solution of Ag2CrO4 is 1.6 × 10-4 M. Calculate Ksp for Ag2CrO4.

Accepted Answer

A)  2.6 × 10-8 
B)  5.1 × 10-8 
C)  1.6 × 10-11 
D)  4.1 × 10-12 
E)  2.0 × 10-12 
A)  2.6 × 10-8 
B)  5.1 × 10-8 
C)  1.6 × 10-11 
D)  4.1 × 10-12 
E)  2.0 × 10-12

Question 5

The Ksp for Mn(OH)2 is 2.0 × 10-13. At what pH will Mn(OH)2 begin to precipitate from a solution in which the initial concentration of Mn2+ is 0.10 M?

Accepted Answer

A)  5.85 
B)  8.15 
C)  6.47 
D)  13.3 
E)  7.03 
A)  5.85 
B)  8.15 
C)  6.47 
D)  13.3 
E)  7.03

Question 6

A 133.4-mL sample of a 0.21 M solution of H3PO4 is titrated with 0.14 M NaOH. What volume of base must be added to reach the third equivalence point?

Accepted Answer

A)  4.0 × 102 mL 
B)  2.0 × 102 mL 
C)  6.0 × 102 mL 
D)  2.7 × 102 mL 
E)  67 mL 
A)  4.0 × 102 mL 
B)  2.0 × 102 mL 
C)  6.0 × 102 mL 
D)  2.7 × 102 mL 
E)  67 mL

Question 7

Determine the pH of a solution prepared by mixing the following:
25)0 mL of 0.200 M HCl
75)0 mL of 0.100 M NaOH
50)0 mL of 0.200 M NaH2PO4
For H3PO4 Ka1 = 7.5 × 10-3, Ka2 = 6.2 × 10-8, and Ka3 = 4.8 × 10-13.

Accepted Answer

A)  6.73 
B)  5.18 
C)  1.65 
D)  4.32 
E)  4.25 
A)  6.73 
B)  5.18 
C)  1.65 
D)  4.32 
E)  4.25

Question 8

Which of the following compounds has the lowest solubility, in moles per liter, in water at 25°C?

Accepted Answer

A)  CdS Ksp = 1.0 × 10-28 
B)  CaSO4  Ksp = 6.1 × 10-5 
C)  Al(OH)3  Ksp = 2.0 × 10-32 
D)  Sn(OH)2  Ksp = 3.0 × 10-27 
E)  Ag3PO4  Ksp = 1.8 × 10-18 
A)  CdS Ksp = 1.0 × 10-28 
B)  CaSO4  Ksp = 6.1 × 10-5 
C)  Al(OH)3  Ksp = 2.0 × 10-32 
D)  Sn(OH)2  Ksp = 3.0 × 10-27 
E)  Ag3PO4  Ksp = 1.8 × 10-18

Question 9

2.42 × 10-3 g of BaSO4 can dissolve in 1.00 L of water. Calculate Ksp for this salt.

Accepted Answer

A)  1.08 × 10-10 
B)  2.42 × 10-3 
C)  5.86 × 10-6 
D)  1.05 × 10-5 
E)  none of these 
A)  1.08 × 10-10 
B)  2.42 × 10-3 
C)  5.86 × 10-6 
D)  1.05 × 10-5 
E)  none of these

Question 10

In the titration of a weak acid HA with 0.100 M NaOH, the stoichiometric point is known to occur at a pH value of approximately 10. Which of the following indicator acids would be best to use to mark the endpoint of this titration?

Accepted Answer

A)  indicator A, Ka = 10-14 
B)  indicator C, Ka = 10-8 
C)  indicator D, Ka = 10-6 
D)  indicator B, Ka = 10-11 
E)  none of these 
A)  indicator A, Ka = 10-14 
B)  indicator C, Ka = 10-8 
C)  indicator D, Ka = 10-6 
D)  indicator B, Ka = 10-11 
E)  none of these

Question 11

48.8 mL of a 1.42 M NaOH solution is titrated with a 1.86 M HCl solution. What is the final volume of the solution when the NaOH has been completely neutralized by the HCl? (Assume the volumes are additive.)

Accepted Answer

A)  37.3 mL 
B)  86.1 mL 
C)  63.9 mL 
D)  49.6 mL 
E)  113 mL 
A)  37.3 mL 
B)  86.1 mL 
C)  63.9 mL 
D)  49.6 mL 
E)  113 mL

Question 12

How many moles of HCl need to be added to 150.0 mL of 0.50 M NaZ to have a solution with a pH of 6.50? (Ka of HZ is 2.3 × 10-5.) Assume negligible volume of the HCl.

Accepted Answer

A)  6.8 × 10-3 mol 
B)  7.5 × 10-2 mol 
C)  1.0 × 10-3 mol 
D)  5.0 × 10-1 mol 
E)  none of these 
A)  6.8 × 10-3 mol 
B)  7.5 × 10-2 mol 
C)  1.0 × 10-3 mol 
D)  5.0 × 10-1 mol 
E)  none of these

Question 13

Which of the following compounds has the lowest solubility, in moles per liter, in water?

Accepted Answer

A)  MgC2O4  Ksp = 8.6 × 10-5 
B)  PbSO4 Ksp = 1.3 × 10-8 
C)  CdS Ksp = 1.0 × 10-28 
D)  Al(OH)3  Ksp = 2 × 10-32 
E)  Sn(OH)2  Ksp = 3 × 10-27 
A)  MgC2O4  Ksp = 8.6 × 10-5 
B)  PbSO4 Ksp = 1.3 × 10-8 
C)  CdS Ksp = 1.0 × 10-28 
D)  Al(OH)3  Ksp = 2 × 10-32 
E)  Sn(OH)2  Ksp = 3 × 10-27

Question 14

For 120.0 mL of a buffer that is 0.40M in HOCl and 0.42 M in NaOCl, what is the pH after 17.5 mL of 1.1 M NaOH is added? Ka for HOCl = 3.5 × 10-8. (Assume the volumes are additive.)

Accepted Answer

A)  7.12 
B)  7.48 
C)  7.43 
D)  7.07 
E)  7.84 
A)  7.12 
B)  7.48 
C)  7.43 
D)  7.07 
E)  7.84

Question 15

Which titration curve would result from the titration of phosphoric acid by a strong base?

Accepted Answer

A)    
B)    
C)    
D)    
E)  None of the above 
A)    
B)    
C)    
D)    
E)  None of the above

Question 16

The shift in equilibrium position of a chemical reaction that occurs because of the addition of an ion already involved in its equilibrium reaction is called the_____.​

Accepted Answer

A)  complex ion equilibria 
B)  common ion effect 
C)  specific ion effect 
D)  Averch-Johnson effect 
E)  ​Quasi-perfect equilibrium 
A)  complex ion equilibria 
B)  common ion effect 
C)  specific ion effect 
D)  Averch-Johnson effect 
E)  ​Quasi-perfect equilibrium

Question 17

For ammonia, Kb is 1.8 × 10-5 . To make a buffered solution with pH 10.0, the ratio of NH4Cl to NH3 must be

Accepted Answer

A)  1.8 : 1. 
B)  0.18 : 1. 
C)  1 : 1.8. 
D)  1 : 0.18. 
E)  none of these 
A)  1.8 : 1. 
B)  0.18 : 1. 
C)  1 : 1.8. 
D)  1 : 0.18. 
E)  none of these

Question 18

Buffers in the human body

Accepted Answer

A)  precipitate proteins so enzymes are inactive. 
B)  help to keep the body temperature constant. 
C)  help change the blood plasma pH when foods are eaten. 
D)  help to maintain a constant blood pH. 
E)  none of these 
A)  precipitate proteins so enzymes are inactive. 
B)  help to keep the body temperature constant. 
C)  help change the blood plasma pH when foods are eaten. 
D)  help to maintain a constant blood pH. 
E)  none of these

Question 19

Consider the titration of 200.0 mL of a 0.100 M solution of the weak acid H2A with 0.200 M NaOH. The first equivalence point is reached after 100.0 mL of 0.200 M NaOH has been added, and the pH is 6.27. The pH after 65.0 mL of 0.200 M NaOH has been added, the pH is 4.95.Calculate the pH of the original acid (no NaOH added).

Accepted Answer

A)  3.19 
B)  2.84 
C)  2.55 
D)  4.68 
E)  none of these 
A)  3.19 
B)  2.84 
C)  2.55 
D)  4.68 
E)  none of these

Question 20

Which of the following is the net ionic equation for the reaction that occurs during the titration of nitrous acid with potassium hydroxide?

Accepted Answer

A)  HNO2 + KOH → K+ + NO2- + H2O 
B)  H+ + OH- → H2O 
C)  HNO2 + OH- → NO2- + H2O 
D)  HNO2 + H2O → NO2- + H3O+ 
E)  HNO2 + K+ + OH- → KNO2 + H2O 
A)  HNO2 + KOH → K+ + NO2- + H2O 
B)  H+ + OH- → H2O 
C)  HNO2 + OH- → NO2- + H2O 
D)  HNO2 + H2O → NO2- + H3O+ 
E)  HNO2 + K+ + OH- → KNO2 + H2O

The solubility of La(IO₃)₃ in a 0.10 M KIO₃ solution is 1.0 × 10^-7 mol/L. Calculate K_sp for La(IO₃)₃.

The observed solubility of the salt MX in 4.0 M strong acid is 2.30 × 10^-3 M. The K_a value for the acid HX is 1.00 × 10^-9. Calculate the value of K_sp for the salt MX.

Which of the following is a major species present at point IV?

The concentration of Ag⁺ in a saturated solution of Ag₂CrO₄ is 1.6 × 10^-4 M. Calculate K_sp for Ag₂CrO₄.

The K_sp for Mn(OH)₂ is 2.0 × 10^-13. At what pH will Mn(OH)₂ begin to precipitate from a solution in which the initial concentration of Mn²⁺ is 0.10 M?

A 133.4-mL sample of a 0.21 M solution of H₃PO₄ is titrated with 0.14 M NaOH. What volume of base must be added to reach the third equivalence point?

Determine the pH of a solution prepared by mixing the following: 25)0 mL of 0.200 M HCl 75)0 mL of 0.100 M NaOH 50)0 mL of 0.200 M NaH₂PO₄For H₃PO₄ K_a1 = 7.5 × 10^-3, K_a2 = 6.2 × 10^-8, and K_a3 = 4.8 × 10^-13.

Which of the following compounds has the lowest solubility, in moles per liter, in water at 25°C?

2.42 × 10^-3 g of BaSO₄ can dissolve in 1.00 L of water. Calculate K_sp for this salt.

In the titration of a weak acid HA with 0.100 M NaOH, the stoichiometric point is known to occur at a pH value of approximately 10. Which of the following indicator acids would be best to use to mark the endpoint of this titration?

48.8 mL of a 1.42 M NaOH solution is titrated with a 1.86 M HCl solution. What is the final volume of the solution when the NaOH has been completely neutralized by the HCl? (Assume the volumes are additive.)

How many moles of HCl need to be added to 150.0 mL of 0.50 M NaZ to have a solution with a pH of 6.50? (K_a of HZ is 2.3 × 10^-5.) Assume negligible volume of the HCl.

Which of the following compounds has the lowest solubility, in moles per liter, in water?

For 120.0 mL of a buffer that is 0.40M in HOCl and 0.42 M in NaOCl, what is the pH after 17.5 mL of 1.1 M NaOH is added? K_a for HOCl = 3.5 × 10^-8. (Assume the volumes are additive.)

Which titration curve would result from the titration of phosphoric acid by a strong base?

The shift in equilibrium position of a chemical reaction that occurs because of the addition of an ion already involved in its equilibrium reaction is called the_____.

For ammonia, K_b is 1.8 × 10^-5 . To make a buffered solution with pH 10.0, the ratio of NH₄Cl to NH₃ must be

Buffers in the human body

Which of the following is the net ionic equation for the reaction that occurs during the titration of nitrous acid with potassium hydroxide?

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Exam 8: Applications of Aqueous Equilibria

The solubility of La(IO3)3 in a 0.10 M KIO3 solution is 1.0 × 10-7 mol/L. Calculate Ksp for La(IO3)3.

The observed solubility of the salt MX in 4.0 M strong acid is 2.30 × 10-3 M. The Ka value for the acid HX is 1.00 × 10-9. Calculate the value of Ksp for the salt MX.

Which of the following is a major species present at point IV?

The concentration of Ag+ in a saturated solution of Ag2CrO4 is 1.6 × 10-4 M. Calculate Ksp for Ag2CrO4.

The Ksp for Mn(OH)2 is 2.0 × 10-13. At what pH will Mn(OH)2 begin to precipitate from a solution in which the initial concentration of Mn2+ is 0.10 M?

A 133.4-mL sample of a 0.21 M solution of H3PO4 is titrated with 0.14 M NaOH. What volume of base must be added to reach the third equivalence point?

Determine the pH of a solution prepared by mixing the following: 25)0 mL of 0.200 M HCl 75)0 mL of 0.100 M NaOH 50)0 mL of 0.200 M NaH2PO4 For H3PO4 Ka1 = 7.5 × 10-3, Ka2 = 6.2 × 10-8, and Ka3 = 4.8 × 10-13.

Which of the following compounds has the lowest solubility, in moles per liter, in water at 25°C?

2.42 × 10-3 g of BaSO4 can dissolve in 1.00 L of water. Calculate Ksp for this salt.

In the titration of a weak acid HA with 0.100 M NaOH, the stoichiometric point is known to occur at a pH value of approximately 10. Which of the following indicator acids would be best to use to mark the endpoint of this titration?

48.8 mL of a 1.42 M NaOH solution is titrated with a 1.86 M HCl solution. What is the final volume of the solution when the NaOH has been completely neutralized by the HCl? (Assume the volumes are additive.)

How many moles of HCl need to be added to 150.0 mL of 0.50 M NaZ to have a solution with a pH of 6.50? (Ka of HZ is 2.3 × 10-5.) Assume negligible volume of the HCl.

Which of the following compounds has the lowest solubility, in moles per liter, in water?

For 120.0 mL of a buffer that is 0.40M in HOCl and 0.42 M in NaOCl, what is the pH after 17.5 mL of 1.1 M NaOH is added? Ka for HOCl = 3.5 × 10-8. (Assume the volumes are additive.)

Which titration curve would result from the titration of phosphoric acid by a strong base?

The shift in equilibrium position of a chemical reaction that occurs because of the addition of an ion already involved in its equilibrium reaction is called the_____.​

For ammonia, Kb is 1.8 × 10-5 . To make a buffered solution with pH 10.0, the ratio of NH4Cl to NH3 must be

Buffers in the human body

Which of the following is the net ionic equation for the reaction that occurs during the titration of nitrous acid with potassium hydroxide?

Atoms, Molecules, and Ions

Stoichiometry

Types of Chemical Reactions and Solution Stoichiometry

Gases

Chemical Equilibrium

Acids and Bases

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

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The Nucleus: a Chemists View

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The solubility of La(IO₃)₃ in a 0.10 M KIO₃ solution is 1.0 × 10^-7 mol/L. Calculate K_sp for La(IO₃)₃.

The observed solubility of the salt MX in 4.0 M strong acid is 2.30 × 10^-3 M. The K_a value for the acid HX is 1.00 × 10^-9. Calculate the value of K_sp for the salt MX.

The concentration of Ag⁺ in a saturated solution of Ag₂CrO₄ is 1.6 × 10^-4 M. Calculate K_sp for Ag₂CrO₄.

The K_sp for Mn(OH)₂ is 2.0 × 10^-13. At what pH will Mn(OH)₂ begin to precipitate from a solution in which the initial concentration of Mn²⁺ is 0.10 M?

A 133.4-mL sample of a 0.21 M solution of H₃PO₄ is titrated with 0.14 M NaOH. What volume of base must be added to reach the third equivalence point?

Determine the pH of a solution prepared by mixing the following: 25)0 mL of 0.200 M HCl 75)0 mL of 0.100 M NaOH 50)0 mL of 0.200 M NaH₂PO₄For H₃PO₄ K_a1 = 7.5 × 10^-3, K_a2 = 6.2 × 10^-8, and K_a3 = 4.8 × 10^-13.

2.42 × 10^-3 g of BaSO₄ can dissolve in 1.00 L of water. Calculate K_sp for this salt.

How many moles of HCl need to be added to 150.0 mL of 0.50 M NaZ to have a solution with a pH of 6.50? (K_a of HZ is 2.3 × 10^-5.) Assume negligible volume of the HCl.

For 120.0 mL of a buffer that is 0.40M in HOCl and 0.42 M in NaOCl, what is the pH after 17.5 mL of 1.1 M NaOH is added? K_a for HOCl = 3.5 × 10^-8. (Assume the volumes are additive.)

The shift in equilibrium position of a chemical reaction that occurs because of the addition of an ion already involved in its equilibrium reaction is called the_____.

For ammonia, K_b is 1.8 × 10^-5 . To make a buffered solution with pH 10.0, the ratio of NH₄Cl to NH₃ must be