Question 1

Identify the pH of normal blood.

Accepted Answer

A)  6.9 
B)  7.1 
C)  7.4 
D)  7.6 
E)  7.9 
A)  6.9 
B)  7.1 
C)  7.4 
D)  7.6 
E)  7.9

Question 2

A 25.0 mL sample of 0.150 M nitrous acid is titrated with a 0.150 M NaOH solution.What is the pH at the equivalence point? The Ka of nitrous acid is 4.6 × 10-4.

Accepted Answer

A)  10.35 mL 
B)  10.65 mL 
C)  3.35 mL 
D)  7.00 mL 
E)  8.11 mL 
A)  10.35 mL 
B)  10.65 mL 
C)  3.35 mL 
D)  7.00 mL 
E)  8.11 mL

Question 3

Determine the molar solubility of BaF2 in pure water.Ksp for BaF2 = 2.45 × 10-5.

Accepted Answer

A)  1.83 × 10-2 M 
B)  1.23 × 10-5 M 
C)  2.90 × 10-2 M 
D)  4.95 × 10-3 M 
E)  6.13 × 10-6 M 
A)  1.83 × 10-2 M 
B)  1.23 × 10-5 M 
C)  2.90 × 10-2 M 
D)  4.95 × 10-3 M 
E)  6.13 × 10-6 M

Question 4

Give the name of the compound that is in antifreeze and is toxic to pets.

Accepted Answer

The answer of Give the name of the compound that...

Question 5

Define buffer capacity.

Accepted Answer

A)  Buffer capacity is the amount of acid or base that can be added to a buffer without destroying its effectiveness. 
B)  Buffer capacity is the amount of acid that can be added until all of the base is used up. 
C)  Buffer capacity is the amount of base that can be added until all of the acid is used up. 
D)  Buffer capacity is the amount of acid that can be added until all of the acid is used up. 
E)  Buffer capacity is the amount of base that can be added until all of the base is used up. 
A)  Buffer capacity is the amount of acid or base that can be added to a buffer without destroying its effectiveness. 
B)  Buffer capacity is the amount of acid that can be added until all of the base is used up. 
C)  Buffer capacity is the amount of base that can be added until all of the acid is used up. 
D)  Buffer capacity is the amount of acid that can be added until all of the acid is used up. 
E)  Buffer capacity is the amount of base that can be added until all of the base is used up.

Question 6

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 66.67 mL of LiOH (this is the equivalence point).

Accepted Answer

A)  0.97 
B)  13.03 
C)  2.76 
D)  11.24 
E)  7.00 
A)  0.97 
B)  13.03 
C)  2.76 
D)  11.24 
E)  7.00

Question 7

The molar solubility of CaF2 is 2.15 × 10-4 M in pure water.Calculate the Ksp for CaF2.

Accepted Answer

A)  1.63 × 10-12 
B)  8.05 × 10-9 
C)  3.97 × 10-11 
D)  4.47 × 10-12 
E)  5.31 × 10-10 
A)  1.63 × 10-12 
B)  8.05 × 10-9 
C)  3.97 × 10-11 
D)  4.47 × 10-12 
E)  5.31 × 10-10

Question 8

A solution contains 0.036 M Cu2+ and 0.044 M Fe2+.A solution containing sulfide ions is added to selectively precipitate one of the metal ions from solution.At what concentration of sulfide ion will a precipitate begin to form? What is the identity of the precipitate?
Ksp(CuS)= 1.3 × 10-36,Ksp(FeS)= 6.3 × 10-18.

Accepted Answer

A)  1.4 × 10-16 M, FeS 
B)  3.6 × 10-35 M, CuS 
C)  3.6 × 10-35 M, FeS 
D)  1.4 × 10-16 M, CuS 
E)  No precipitate will form at any concentration of sulfide ion. 
A)  1.4 × 10-16 M, FeS 
B)  3.6 × 10-35 M, CuS 
C)  3.6 × 10-35 M, FeS 
D)  1.4 × 10-16 M, CuS 
E)  No precipitate will form at any concentration of sulfide ion.

Question 9

Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 M HC7H5O2 with 100.0 mL of 0.30 M NaC7H5O2.The Ka for HC7H5O2 is 6.5 × 10-5.

Accepted Answer

A)  4.19 
B)  9.69 
C)  4.49 
D)  4.31 
E)  10.51 
A)  4.19 
B)  9.69 
C)  4.49 
D)  4.31 
E)  10.51

Question 10

Calculate the pH of a buffer that is 1.58 M HClO and 0.099 M NaClO.The Ka for HClO is 2.9 × 10-8.

Accepted Answer

A)  7.54 
B)  6.87 
C)  7.74 
D)  6.16 
E)  6.33 
A)  7.54 
B)  6.87 
C)  7.74 
D)  6.16 
E)  6.33

Question 11

You wish to prepare an HC2H3O2 buffer with a pH of 4.14.If the pKa of is 4.74,what ratio of C2H3O2⁻/HC2H3O2 must you use?

Accepted Answer

A)  0.10 
B)  0.60 
C)  0.25 
D)  3.98 
E)  4.0 
A)  0.10 
B)  0.60 
C)  0.25 
D)  3.98 
E)  4.0

Question 12

Calculate the percent ionization of nitrous acid in a solution that is 0.205 M in nitrous acid   and 0.295 M in potassium nitrite (   ).The acid dissociation constant of nitrous acid is

Accepted Answer

A)  59.0 
B)  0.151 
C)  17.1 
D)  2.72 ×   
E)  3.508 
A)  59.0 
B)  0.151 
C)  17.1 
D)  2.72 ×   
E)  3.508

Question 13

In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25°C?

Accepted Answer

A)  0.1 M HBr 
B)  0.1 M NaBr 
C)  0.1 M CaBr2 
D)  0.1 M K NO3 
A)  0.1 M HBr 
B)  0.1 M NaBr 
C)  0.1 M CaBr2 
D)  0.1 M K NO3

Question 14

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 3.5 × 10-4 M in calcium ion and 2.33 × 10-4 M in oxalate ion.What will happen once these solutions are mixed? Ksp (CaC2O4)= 2.3 × 10-9.

Accepted Answer

A)  Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds. 
B)  Nothing will happen Ksp > Q for all possible precipitants. 
C)  A precipitate will form as calcium oxalate is not soluble to any extent. 
D)  A precipitate will form since Q > Ksp for calcium oxalate. 
E)  There is not enough information to determine. 
A)  Nothing will happen since both calcium chloride and lithium oxalate are soluble compounds. 
B)  Nothing will happen Ksp > Q for all possible precipitants. 
C)  A precipitate will form as calcium oxalate is not soluble to any extent. 
D)  A precipitate will form since Q > Ksp for calcium oxalate. 
E)  There is not enough information to determine.

Question 15

Calculate the Ksp for zinc hydroxide if the solubility of Zn (OH)2 in pure water is 2.1 × 10-4 g/L.

Accepted Answer

A)  9.9 × 10-18 
B)  3.8 × 10-17 
C)  1.5 × 10-3 
D)  2.9 × 10-3 
A)  9.9 × 10-18 
B)  3.8 × 10-17 
C)  1.5 × 10-3 
D)  2.9 × 10-3

Question 16

Which one of the following statements is TRUE?

Accepted Answer

A)  A buffer is an aqueous solution composed of two strong bases. 
B)  A buffer can absorb an unlimited amount of base. 
C)  A buffer resists pH change by neutralizing added acids and bases. 
D)  A buffer does not change pH when strong base is added. 
E)  All of the above are true. 
A)  A buffer is an aqueous solution composed of two strong bases. 
B)  A buffer can absorb an unlimited amount of base. 
C)  A buffer resists pH change by neutralizing added acids and bases. 
D)  A buffer does not change pH when strong base is added. 
E)  All of the above are true.

Question 17

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 200.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

Accepted Answer

A)  6.44 
B)  1.48 
C)  2.00 
D)  12.52 
E)  12.00 
A)  6.44 
B)  1.48 
C)  2.00 
D)  12.52 
E)  12.00

Question 18

0.10 M potassium chromate is slowly added to a solution containing 0.10 M AgNO3 and 0.10 M Ba(NO3)2.What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and 1.2 × 10-10,respectively.

Accepted Answer

A)  6.5 × 10-5 M 
B)  1.3 × 10-4 M 
C)  3.2 × 10-4 M 
D)  3.0 × 10-2 M 
A)  6.5 × 10-5 M 
B)  1.3 × 10-4 M 
C)  3.2 × 10-4 M 
D)  3.0 × 10-2 M

Question 19

Give the expression for the solubility product constant for PbCl2.

Accepted Answer

A)    
B)    
C)  [Pb2+][Cl⁻]2 
D)    
E)  [Pb2+]2[ Cl⁻] 
A)    
B)    
C)  [Pb2+][Cl⁻]2 
D)    
E)  [Pb2+]2[ Cl⁻]

Question 20

What is the pH of a buffer solution that is 0.255 M in hypochlorous acid (HClO)and 0.333 M in sodium hypochlorite? The Ka of hypochlorous acid is 3.8 × 10-8.

Accepted Answer

A)  13.88 
B)  6.46 
C)  8.49 
D)  7.30 
E)  7.54 
A)  13.88 
B)  6.46 
C)  8.49 
D)  7.30 
E)  7.54

Exam 18: Aqueous Ionic Equilibrium

Identify the pH of normal blood.

A 25.0 mL sample of 0.150 M nitrous acid is titrated with a 0.150 M NaOH solution.What is the pH at the equivalence point? The Ka of nitrous acid is 4.6 × 10-4.

Determine the molar solubility of BaF2 in pure water.Ksp for BaF2 = 2.45 × 10-5.

Give the name of the compound that is in antifreeze and is toxic to pets.

Define buffer capacity.

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 66.67 mL of LiOH (this is the equivalence point).

The molar solubility of CaF2 is 2.15 × 10-4 M in pure water.Calculate the Ksp for CaF2.

Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 M HC7H5O2 with 100.0 mL of 0.30 M NaC7H5O2.The Ka for HC7H5O2 is 6.5 × 10-5.

Calculate the pH of a buffer that is 1.58 M HClO and 0.099 M NaClO.The Ka for HClO is 2.9 × 10-8.

You wish to prepare an HC2H3O2 buffer with a pH of 4.14.If the pKa of is 4.74,what ratio of C2H3O2⁻/HC2H3O2 must you use?

Calculate the percent ionization of nitrous acid in a solution that is 0.205 M in nitrous acid and 0.295 M in potassium nitrite ( ).The acid dissociation constant of nitrous acid is

In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25°C?

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is 3.5 × 10-4 M in calcium ion and 2.33 × 10-4 M in oxalate ion.What will happen once these solutions are mixed? Ksp (CaC2O4)= 2.3 × 10-9.

Calculate the Ksp for zinc hydroxide if the solubility of Zn (OH)2 in pure water is 2.1 × 10-4 g/L.

Which one of the following statements is TRUE?

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 200.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

0.10 M potassium chromate is slowly added to a solution containing 0.10 M AgNO3 and 0.10 M Ba(NO3)2.What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and 1.2 × 10-10,respectively.

Give the expression for the solubility product constant for PbCl2.

What is the pH of a buffer solution that is 0.255 M in hypochlorous acid (HClO)and 0.333 M in sodium hypochlorite? The Ka of hypochlorous acid is 3.8 × 10-8.

Essentials: Units, Measurements, and Problem Solving

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The Quantum Mechanical Model of the Atom

Periodic Properties of the Elements

Molecules and Compounds

Chemical Bonding I

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Chemical Reactions and Chemical Quantities

Introduction to Solutions and Aqueous Reactions

Thermochemistry

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Liquids, Solids, and Intermolecular Forces

Crystalline Solids and Modern Materials

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Chemical Kinetics

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Free Energy and Thermodynamics

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A 25.0 mL sample of 0.150 M nitrous acid is titrated with a 0.150 M NaOH solution.What is the pH at the equivalence point? The K_a of nitrous acid is 4.6 × 10^-4.

Determine the molar solubility of BaF₂in pure water.K_sp for BaF₂ = 2.45 × 10^-5.

A 100.0 mL sample of 0.18 M HClO₄ is titrated with 0.27 M LiOH.Determine the pH of the solution after the addition of 66.67 mL of LiOH (this is the equivalence point).

The molar solubility of CaF₂ is 2.15 × 10^-4 M in pure water.Calculate the K_sp for CaF₂.

Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 M HC₇H₅O₂ with 100.0 mL of 0.30 M NaC₇H₅O₂.The K_a for HC₇H₅O₂ is 6.5 × 10^-5.

Calculate the pH of a buffer that is 1.58 M HClO and 0.099 M NaClO.The K_a for HClO is 2.9 × 10^-8.

You wish to prepare an HC₂H₃O₂ buffer with a pH of 4.14.If the pK_a of is 4.74,what ratio of C₂H₃O₂⁻/HC₂H₃O₂ must you use?

In which of the following solutions would solid PbBr₂ be expected to be the least soluble at 25°C?

A solution containing CaCl₂ is mixed with a solution of Li₂C₂O₄ to form a solution that is 3.5 × 10^-4 M in calcium ion and 2.33 × 10^-4M in oxalate ion.What will happen once these solutions are mixed? K_sp (CaC₂O₄)= 2.3 × 10^-9.

Calculate the K_sp for zinc hydroxide if the solubility of Zn(OH)₂ in pure water is 2.1 × 10^-4g/L.

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 200.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

0.10 M potassium chromate is slowly added to a solution containing 0.10 M AgNO₃ and 0.10 M Ba(NO₃)₂.What is the Ag⁺ concentration when BaCrO₄ just starts to precipitate? The K_sp for Ag₂CrO₄ and BaCrO₄ are 1.1 × 10^-12 and 1.2 × 10^-10,respectively.

Give the expression for the solubility product constant for PbCl₂.

What is the pH of a buffer solution that is 0.255 M in hypochlorous acid (HClO)and 0.333 M in sodium hypochlorite? The K_a of hypochlorous acid is 3.8 × 10^-8.