Question 1

Which one of the following salts forms aqueous solutions with pH F1F1F1S1F1F1F10 7?

Accepted Answer

A) Na2S 
B) NaBr 
C) NaClO2 
D) NaNO2 
E) Na2CO3 
A) Na2S 
B) NaBr 
C) NaClO2 
D) NaNO2 
E) Na2CO3

Question 2

Define a conjugate acidF1F1F1S1F1F1F10base pair and provide an example.

Accepted Answer

A conjugate acidF1F1F1S1F1F1F

Question 3

What is the concentration of the acetate ion in a 1.00 M CH3COOH solution given that the Ka of CH3COOH is 1.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105?

Accepted Answer

4.20 F1F1F

Question 4

Magnesium sulfate can be obtained at a drugstore as Epsom salts. The monohydrate is found as the mineral kieserite (MgSO4 F1F1F1S1F1F1F10 H2O, 138 g/mol). What would be the pH of a 500 mL aqueous solution containing 1.62 g of dissolved kieserite? The   value for sulfuric acid is 1.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F102.

Accepted Answer

A) 7.00 
B) 6.85 
C) 7.15 
D) 3.55 
E) 12.22 
A) 7.00 
B) 6.85 
C) 7.15 
D) 3.55 
E) 12.22

Question 5

Write the reaction and equilibrium constant that describes the autoionization of water.

Accepted Answer

The answer of Write the reaction and equilibrium constant that...

Question 6

Ammonia (NH3) acts as a weak base in aqueous solution. What is the acid that reacts with this base when ammonia is dissolved in water?

Accepted Answer

A) None, there are no acids in pure water. 
B) H2O 
C) NH4F1F1F1S1F1F1F10 
D) trick question, because no acids are present, ammonia cannot act as a base 
E) oxygen that always is dissolved in water 
A) None, there are no acids in pure water. 
B) H2O 
C) NH4F1F1F1S1F1F1F10 
D) trick question, because no acids are present, ammonia cannot act as a base 
E) oxygen that always is dissolved in water

Question 7

Sometimes liquid ammonia, NH3, is used as a solvent rather than water. Which expression defines the ammonia autoionization counterpart of Kw?

Accepted Answer

A) [H3OF1F1F1S1F1F1F10][OHF1F1F1S1F1F1F10] 
B) [NH3][NH4F1F1F1S1F1F1F10] 
C) [NH2F1F1F1S1F1F1F10][NH4F1F1F1S1F1F1F10] 
D) [H3OF1F1F1S1F1F1F10][NH2F1F1F1S1F1F1F10] 
E) [NH4F1F1F1S1F1F1F10][OHF1F1F1S1F1F1F10] 
A) [H3OF1F1F1S1F1F1F10][OHF1F1F1S1F1F1F10] 
B) [NH3][NH4F1F1F1S1F1F1F10] 
C) [NH2F1F1F1S1F1F1F10][NH4F1F1F1S1F1F1F10] 
D) [H3OF1F1F1S1F1F1F10][NH2F1F1F1S1F1F1F10] 
E) [NH4F1F1F1S1F1F1F10][OHF1F1F1S1F1F1F10]

Question 8

Three acids found in foods are lactic acid (in milk products), oxalic acid (in rhubarb), and malic acid (in apples). The pKa values are LA F1F1F1S1F1F1F10 3.88, OA F1F1F1S1F1F1F10 1.23, and MA F1F1F1S1F1F1F10 3.40. Which list has these acids in order of decreasing acid strength?

Accepted Answer

A) LA F1F1F1S1F1F1F10 OA F1F1F1S1F1F1F10 MA 
B) LA F1F1F1S1F1F1F10 MA F1F1F1S1F1F1F10 OA 
C) OA F1F1F1S1F1F1F10 MA F1F1F1S1F1F1F10 LA 
D) OA F1F1F1S1F1F1F10 LA F1F1F1S1F1F1F10 MA 
E) MA F1F1F1S1F1F1F10 LA F1F1F1S1F1F1F10 OA 
A) LA F1F1F1S1F1F1F10 OA F1F1F1S1F1F1F10 MA 
B) LA F1F1F1S1F1F1F10 MA F1F1F1S1F1F1F10 OA 
C) OA F1F1F1S1F1F1F10 MA F1F1F1S1F1F1F10 LA 
D) OA F1F1F1S1F1F1F10 LA F1F1F1S1F1F1F10 MA 
E) MA F1F1F1S1F1F1F10 LA F1F1F1S1F1F1F10 OA

Question 9

Which one of the following is not a conjugate acid-base pair?

Accepted Answer

A) NH3 and NH4F1F1F1S1F1F1F10 
B) H3OF1F1F1S1F1F1F10 and OHF1F1F1S1F1F1F10 
C) H2PO4F1F1F1S1F1F1F10 and HPO42F1F1F1S1F1F1F10 
D) HSF1F1F1S1F1F1F10 and H2S 
E) NH3 and NH2F1F1F1S1F1F1F10 
A) NH3 and NH4F1F1F1S1F1F1F10 
B) H3OF1F1F1S1F1F1F10 and OHF1F1F1S1F1F1F10 
C) H2PO4F1F1F1S1F1F1F10 and HPO42F1F1F1S1F1F1F10 
D) HSF1F1F1S1F1F1F10 and H2S 
E) NH3 and NH2F1F1F1S1F1F1F10

Question 10

Lactic acid is a major component of Ringer's solution, which is used as an intravenous fluid to maintain fluid balance in trauma patients. The pH of a 0.100 M lactic acid solution is around 2.44. Based on this information, determine the value of the acid ionization constant, Ka, for lactic acid.

Accepted Answer

1.4 F1F1F1

Question 11

Phosphoric acid is a triprotic acid, ionizing in the following sequential steps: H3PO4 F1F1F1S1F1F1F10 H2O   H2PO4F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 H3OF1F1F1S1F1F1F10   H2PO4F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 H2O   HPO42F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 H3OF1F1F1S1F1F1F10   HPO42F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 H2O   PO43F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 H3OF1F1F1S1F1F1F10   What is the Kb expression for the base, sodium phosphate?

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 12

Boric acid frequently is used as an eyewash to treat eye infections. The pH of a 0.050 M solution of boric acid is 5.28. What is the value of the boric acid ionization constant, Ka?

Accepted Answer

A) 5.25 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 
B) 5.51 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1010 
C) 5.43 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 
D) 5.79 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
E) 5.33 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1012 
A) 5.25 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 
B) 5.51 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1010 
C) 5.43 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 
D) 5.79 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
E) 5.33 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1012

Question 13

In the following reaction in aqueous solution, the acid reactant is ________ and its conjugate base product is ________. CH3COOH F1F1F1S1F1F1F10 NH3   CH3COOF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 NH4F1F1F1S1F1F1F10

Accepted Answer

A) CH3COOH; CH3COOF1F1F1S1F1F1F10 
B) CH3COOH; NH4F1F1F1S1F1F1F10 
C) NH3; CH3COOF1F1F1S1F1F1F10 
D) NH3; NH4F1F1F1S1F1F1F10 
E) CH3COOH; H3OF1F1F1S1F1F1F10 
A) CH3COOH; CH3COOF1F1F1S1F1F1F10 
B) CH3COOH; NH4F1F1F1S1F1F1F10 
C) NH3; CH3COOF1F1F1S1F1F1F10 
D) NH3; NH4F1F1F1S1F1F1F10 
E) CH3COOH; H3OF1F1F1S1F1F1F10

Question 14

Identify the weakest and strongest acids in the group below. The weakest acid is listed first in the responses. CH4, SiH4, SnH4

Accepted Answer

A) CH4 F1F1F1S1F1F1F10 SiH4 
B) CH4 F1F1F1S1F1F1F10 SnH4 
C) SiH4 F1F1F1S1F1F1F10 SnH4 
D) SiH4 F1F1F1S1F1F1F10 SnH4. 
E) SnH4 F1F1F1S1F1F1F10 CH4 
A) CH4 F1F1F1S1F1F1F10 SiH4 
B) CH4 F1F1F1S1F1F1F10 SnH4 
C) SiH4 F1F1F1S1F1F1F10 SnH4 
D) SiH4 F1F1F1S1F1F1F10 SnH4. 
E) SnH4 F1F1F1S1F1F1F10 CH4

Question 15

Which statement A-D is not correct? Pure water at 25F1F1F1S1F1F1F10C has ________

Accepted Answer

A) Kw F1F1F1S1F1F1F10 1.0 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1014. 
B) pOH F1F1F1S1F1F1F10 7. 
C) [H3OF1F1F1S1F1F1F10] F1F1F1S1F1F1F10 [OHF1F1F1S1F1F1F10]. 
D) pH F1F1F1S1F1F1F10 7. 
E) A-D are all correct. 
A) Kw F1F1F1S1F1F1F10 1.0 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1014. 
B) pOH F1F1F1S1F1F1F10 7. 
C) [H3OF1F1F1S1F1F1F10] F1F1F1S1F1F1F10 [OHF1F1F1S1F1F1F10]. 
D) pH F1F1F1S1F1F1F10 7. 
E) A-D are all correct.

Question 16

When [HF1F1F1S1F1F1F10] F1F1F1S1F1F1F10 4.0 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F109 M in water at 25F1F1F1S1F1F1F10C, then ________

Accepted Answer

A) pH F1F1F1S1F1F1F10 9.40. 
B) pH F1F1F1S1F1F1F10 7.00. 
C) pH F1F1F1S1F1F1F10 F1F1F1S1F1F1F108.40. 
D) pH F1F1F1S1F1F1F10 8.40. 
E) pH F1F1F1S1F1F1F10 F1F1F1S1F1F1F109.40. 
A) pH F1F1F1S1F1F1F10 9.40. 
B) pH F1F1F1S1F1F1F10 7.00. 
C) pH F1F1F1S1F1F1F10 F1F1F1S1F1F1F108.40. 
D) pH F1F1F1S1F1F1F10 8.40. 
E) pH F1F1F1S1F1F1F10 F1F1F1S1F1F1F109.40.

Question 17

Explain why some salts produce neutral solutions while others produce solutions that are acidic or basic, and give an example for each.

Accepted Answer

Acidic solutions are produced if the cat

Question 18

The degree of ionization ________

Accepted Answer

A) increases with increasing concentration of a weak acid. 
B) decreases with increasing concentration of a weak acid. 
C) does not change with changing concentration of a weak acid. 
D) is not related to the concentration of a weak acid. 
E) is independent of the composition of the weak acid. 
A) increases with increasing concentration of a weak acid. 
B) decreases with increasing concentration of a weak acid. 
C) does not change with changing concentration of a weak acid. 
D) is not related to the concentration of a weak acid. 
E) is independent of the composition of the weak acid.

Question 19

Three common weak bases are phosphate (P; PO43F1F1F1S1F1F1F10, pKb F1F1F1S1F1F1F10 1.3), carbonate (C; CO32F1F1F1S1F1F1F10, pKb F1F1F1S1F1F1F10 3.7), and acetate (A; CH3COOF1F1F1S1F1F1F10, pKb F1F1F1S1F1F1F10 9.3). Which response has these bases listed in order of increasing strength?

Accepted Answer

A) P F1F1F1S1F1F1F10 C F1F1F1S1F1F1F10 A 
B) C F1F1F1S1F1F1F10 P F1F1F1S1F1F1F10 A 
C) A F1F1F1S1F1F1F10 C F1F1F1S1F1F1F10 P 
D) C F1F1F1S1F1F1F10 A F1F1F1S1F1F1F10 P 
E) P F1F1F1S1F1F1F10 A F1F1F1S1F1F1F10 C 
A) P F1F1F1S1F1F1F10 C F1F1F1S1F1F1F10 A 
B) C F1F1F1S1F1F1F10 P F1F1F1S1F1F1F10 A 
C) A F1F1F1S1F1F1F10 C F1F1F1S1F1F1F10 P 
D) C F1F1F1S1F1F1F10 A F1F1F1S1F1F1F10 P 
E) P F1F1F1S1F1F1F10 A F1F1F1S1F1F1F10 C

Question 20

Which one A-D is not related to the water autoionization constant, Kw?

Accepted Answer

A) [H3OF1F1F1S1F1F1F10] [OHF1F1F1S1F1F1F10] 
B) 1.0 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1014 at 25F1F1F1S1F1F1F10C 
C) 2 H2O   H3OF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 OHF1F1F1S1F1F1F10 
D) pH F1F1F1S1F1F1F10 7 at 25F1F1F1S1F1F1F10C 
E) A-D are all related to Kw. 
A) [H3OF1F1F1S1F1F1F10] [OHF1F1F1S1F1F1F10] 
B) 1.0 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1014 at 25F1F1F1S1F1F1F10C 
C) 2 H2O   H3OF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 OHF1F1F1S1F1F1F10 
D) pH F1F1F1S1F1F1F10 7 at 25F1F1F1S1F1F1F10C 
E) A-D are all related to Kw.

Exam 15: Acidbase Equilibria: Proton Transfer in Biological Systems

Which one of the following salts forms aqueous solutions with pH  7?

Define a conjugate acidbase pair and provide an example.

What is the concentration of the acetate ion in a 1.00 M CH3COOH solution given that the Ka of CH3COOH is 1.8  105?

Magnesium sulfate can be obtained at a drugstore as Epsom salts. The monohydrate is found as the mineral kieserite (MgSO4  H2O, 138 g/mol). What would be the pH of a 500 mL aqueous solution containing 1.62 g of dissolved kieserite? The value for sulfuric acid is 1.2  102.

Write the reaction and equilibrium constant that describes the autoionization of water.

Ammonia (NH3) acts as a weak base in aqueous solution. What is the acid that reacts with this base when ammonia is dissolved in water?

Sometimes liquid ammonia, NH3, is used as a solvent rather than water. Which expression defines the ammonia autoionization counterpart of Kw?

Three acids found in foods are lactic acid (in milk products), oxalic acid (in rhubarb), and malic acid (in apples). The pKa values are LA  3.88, OA  1.23, and MA  3.40. Which list has these acids in order of decreasing acid strength?

Which one of the following is not a conjugate acid-base pair?

Lactic acid is a major component of Ringer's solution, which is used as an intravenous fluid to maintain fluid balance in trauma patients. The pH of a 0.100 M lactic acid solution is around 2.44. Based on this information, determine the value of the acid ionization constant, Ka, for lactic acid.

Phosphoric acid is a triprotic acid, ionizing in the following sequential steps: H3PO4  H2O H2PO4  H3O H2PO4  H2O HPO42  H3O HPO42  H2O PO43  H3O What is the Kb expression for the base, sodium phosphate?

Boric acid frequently is used as an eyewash to treat eye infections. The pH of a 0.050 M solution of boric acid is 5.28. What is the value of the boric acid ionization constant, Ka?

In the following reaction in aqueous solution, the acid reactant is ________ and its conjugate base product is ________. CH3COOH  NH3 CH3COO  NH4

Identify the weakest and strongest acids in the group below. The weakest acid is listed first in the responses. CH4, SiH4, SnH4

Which statement A-D is not correct? Pure water at 25C has ________

When [H]  4.0  109 M in water at 25C, then ________

Explain why some salts produce neutral solutions while others produce solutions that are acidic or basic, and give an example for each.

The degree of ionization ________

Three common weak bases are phosphate (P; PO43, pKb  1.3), carbonate (C; CO32, pKb  3.7), and acetate (A; CH3COO, pKb  9.3). Which response has these bases listed in order of increasing strength?

Which one A-D is not related to the water autoionization constant, Kw?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

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The Main Group Elements: Life and the Periodic Table

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What is the concentration of the acetate ion in a 1.00 M CH₃COOH solution given that the K_a of CH₃COOH is 1.8  10^⁵?

Magnesium sulfate can be obtained at a drugstore as Epsom salts. The monohydrate is found as the mineral kieserite (MgSO₄  H₂O, 138 g/mol). What would be the pH of a 500 mL aqueous solution containing 1.62 g of dissolved kieserite? The value for sulfuric acid is 1.2  10^².

Ammonia (NH₃) acts as a weak base in aqueous solution. What is the acid that reacts with this base when ammonia is dissolved in water?

Sometimes liquid ammonia, NH₃, is used as a solvent rather than water. Which expression defines the ammonia autoionization counterpart of K_w?

Three acids found in foods are lactic acid (in milk products), oxalic acid (in rhubarb), and malic acid (in apples). The pK_a values are LA  3.88, OA  1.23, and MA  3.40. Which list has these acids in order of decreasing acid strength?

Lactic acid is a major component of Ringer's solution, which is used as an intravenous fluid to maintain fluid balance in trauma patients. The pH of a 0.100 M lactic acid solution is around 2.44. Based on this information, determine the value of the acid ionization constant, K_a, for lactic acid.

Phosphoric acid is a triprotic acid, ionizing in the following sequential steps: H₃PO₄  H₂O H₂PO₄^  H₃O^ H₂PO₄^  H₂O HPO₄²^  H₃O^ HPO₄²^  H₂O PO₄³^  H₃O^ What is the K_b expression for the base, sodium phosphate?

Boric acid frequently is used as an eyewash to treat eye infections. The pH of a 0.050 M solution of boric acid is 5.28. What is the value of the boric acid ionization constant, K_a?

In the following reaction in aqueous solution, the acid reactant is and its conjugate base product is . CH₃COOH  NH₃ CH₃COO^  NH₄^

Identify the weakest and strongest acids in the group below. The weakest acid is listed first in the responses. CH₄, SiH₄, SnH₄

When [H^]  4.0  10^⁹ M in water at 25C, then ________

Three common weak bases are phosphate (P; PO₄³^, pK_b  1.3), carbonate (C; CO₃²^, pK_b  3.7), and acetate (A; CH₃COO^, pK_b  9.3). Which response has these bases listed in order of increasing strength?

Which one A-D is not related to the water autoionization constant, K_w?