What is the pH of the buffer that results when 32 g sodium acetate (NaCH3CO2)is mixed with 500.0 mL of 1.0 M acetic acid (CH3CO2H)and diluted with water to 1.0 L? (Ka of CH3CO2H = 1.8 × 10-5)

A) 2.52 B) 4.23 C) 4.44 D) 4.64 E) 4.74 A) 2.52 B) 4.23 C) 4.44 D) 4.64 E) 4.74

Suppose 50.00 mL of 2.0 × 10-5 M Fe(NO3)3 is added to 50.00 mL of 2.0 ×10-4 M KIO3.Which of the following statements is true? For Fe(IO3)3,Ksp = 1.0 × 10-14.

A) A precipitate forms because Qc > Ksp. B) A precipitate forms because Qc sp. C) No precipitate forms because Qc sp. D) No precipitate forms because Qc = Ksp. E) No precipitate forms because Qc > Ksp. A) A precipitate forms because Qc > Ksp. B) A precipitate forms because Qc sp. C) No precipitate forms because Qc sp. D) No precipitate forms because Qc = Ksp. E) No precipitate forms because Qc > Ksp.

What is the pH at the equivalence point when a 25.0 mL sample of 0.200 M aqueous formic acid (HCO2H)is titrated with 0.100 M aqueous potassium hydroxide? (Ka of HCO2H = 1.8 × 10-4)

A) 5.71 B) 7.00 C) 8.28 D) 8.52 E) 10.26 A) 5.71 B) 7.00 C) 8.28 D) 8.52 E) 10.26

What is the maximum hydroxide-ion concentration that a 0.019 M MgCl2 solution could have without causing the precipitation of Mg(OH)2? For Mg(OH)2,Ksp = 1.8 × 10-11.

A) 4.2 × 10-6 B) 1.7 × 10-4 C) 1.2 × 10-8 D) 9.5 × 10-9 E) 3.1 × 10-5 A) 4.2 × 10-6 B) 1.7 × 10-4 C) 1.2 × 10-8 D) 9.5 × 10-9 E) 3.1 × 10-5

If 20 mL of 0.10 M NaOH is added to 40 mL of 0.20 M HC2H3O2,what is the pH of the resulting solution at 25°C? Ka for HC2H3O2 is 1.8 × 10-5 at 25°C.

A) 9.8 B) 4.1 C) 5.2 D) 2.7 E) 4.3 A) 9.8 B) 4.1 C) 5.2 D) 2.7 E) 4.3

What is the minimum mass of Na2CO3 (molar mass = 105.990 g/mol)that must be added to 43.4 mL of a 1.0 × 10-4 M AgNO3 solution in order for precipitation to occur? The Ksp of Ag2CO3 is 8.6 × 10-12.Assume no volume change occurs upon addition of Na2CO3.

A) 4.6 × 10-4 g B) 3.1 × 10-4 g C) 2.3 × 10-4 g D) 4.0 × 10-7 g E) 4.0 × 10-3 g A) 4.6 × 10-4 g B) 3.1 × 10-4 g C) 2.3 × 10-4 g D) 4.0 × 10-7 g E) 4.0 × 10-3 g

If 0.50 L of a buffer containing 1.0 mol H2PO4− and 1.0 mol HPO42− is diluted to a volume of 5.0 L,the pH

A) increases by 1. B) decreases by 1. C) increases by 10. D) decreases by 10. E) remains unchanged. A) increases by 1. B) decreases by 1. C) increases by 10. D) decreases by 10. E) remains unchanged.

If 500 mL of 1.4 × 10-6 M AgNO3 is mixed with 500 mL of 1.4 × 10-6 M NaBr,what will occur? For AgBr,Ksp = 5 × 10-13.

A) Silver(I)bromide will precipitate. B) The concentration of Ag+ will be 1.4 × 10-6 M. C) 7.0 × 10-7 mol of AgBr will form. D) No precipitation will occur. E) Sodium bromide will precipitate. A) Silver(I)bromide will precipitate. B) The concentration of Ag+ will be 1.4 × 10-6 M. C) 7.0 × 10-7 mol of AgBr will form. D) No precipitation will occur. E) Sodium bromide will precipitate.

Exam 17: Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

What is the pH of the buffer that results when 32 g sodium acetate (NaCH₃CO₂)is mixed with 500.0 mL of 1.0 M acetic acid (CH₃CO₂H)and diluted with water to 1.0 L? (K_a of CH₃CO₂H = 1.8 × 10^-5)

(Multiple Choice)

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Question 61

What molar ratio of acetic acid to sodium acetate is required to create a buffer solution having a pH of 4.88 at 25°C? K_a for HC₂H₃O₂ is 1.8 × 10^-5.

(Multiple Choice)

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Question 62

What mass of sodium hydroxide must be added to 65.0 mL of 0.926 M acetic acid in order to create a buffer with a pH of 4.83? K_a for acetic acid is 1.8 × 10^-5.

(Multiple Choice)

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Question 63

Suppose 50.00 mL of 2.0 × 10^-5 M Fe(NO₃)₃ is added to 50.00 mL of 2.0 ×10^-4 M KIO₃.Which of the following statements is true? For Fe(IO₃)₃,K_sp = 1.0 × 10^-14.

(Multiple Choice)

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Question 64

A 50.00-mL solution of 0.0426 M trimethylamine (K_b = 6.5 × 10^-5)is titrated with a 0.0257 M solution of hydrochloric acid as the titrant.What is the pH of the base solution after 22.31 mL of titrant have been added? (K_w = 1.00 × 10^-14)

(Multiple Choice)

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Question 65

What is the pH at the equivalence point when a 25.0 mL sample of 0.200 M aqueous formic acid (HCO₂H)is titrated with 0.100 M aqueous potassium hydroxide? (K_a of HCO₂H = 1.8 × 10^-4)

(Multiple Choice)

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Question 66

Two important biological buffer systems control pH in the range of 6.9 to 7.4.These buffer systems are H₂CO₃/HCO₃^- and _____.

(Short Answer)

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Question 67

What is the maximum hydroxide-ion concentration that a 0.019 M MgCl₂ solution could have without causing the precipitation of Mg(OH)₂? For Mg(OH)₂,K_sp = 1.8 × 10^-11.

(Multiple Choice)

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Question 68

What will be the pH of the solution when 0.10 mol of H⁺ ion is added to a 2.0 liter buffered solution composed of 0.45 M ammonia,NH3,and 0.26 M ammonium fluoride,NH₄F? (K_b for ammonia = 1.8 × 10^-5)

(Multiple Choice)

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Question 69

The hydroxide ion concentration of a saturated solution of Fe(OH)₂ is M.What is the solubility product constant for Fe(OH)₂?

(Multiple Choice)

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Question 70

What is the pH of a buffer that results when 0.50 mole of H₃PO₄ is mixed with 0.75 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are K_a1 = 7.5 × 10^-3,K_a2 = 6.2 × 10^-8,and K_a3 = 3.6 × 10^-13)

(Multiple Choice)

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Question 71

How many moles of solid NaF would have to be added to 1.0 L of 2.16 M HF solution to achieve a buffer of pH 3.35? Assume there is no volume change.(K_a for HF = 7.2 × 10^-4)

(Multiple Choice)

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Question 72

If 25 mL of 0.750 M HCl are added to 100.mL of 0.302 M NaOH,what is the final pH?

(Multiple Choice)

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Question 73

If 20 mL of 0.10 M NaOH is added to 40 mL of 0.20 M HC₂H₃O₂,what is the pH of the resulting solution at 25°C? K_a for HC₂H₃O₂ is 1.8 × 10^-5 at 25°C.

(Multiple Choice)

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Question 74

What is the minimum mass of Na₂CO₃ (molar mass = 105.990 g/mol)that must be added to 43.4 mL of a 1.0 × 10^-4 M AgNO₃ solution in order for precipitation to occur? The K_sp of Ag₂CO₃ is 8.6 × 10^-12.Assume no volume change occurs upon addition of Na₂CO₃.

(Multiple Choice)

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Question 75

When a weak base is titrated with a strong acid,the pH at the equivalence point is _____.

(Multiple Choice)

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Question 76

All of the following statements concerning acid-base buffers are true EXCEPT

(Multiple Choice)

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Question 77

If 0.50 L of a buffer containing 1.0 mol H₂PO₄− and 1.0 mol HPO₄²⁻ is diluted to a volume of 5.0 L,the pH

(Multiple Choice)

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Question 78

If 500 mL of 1.4 × 10^-6 M AgNO₃ is mixed with 500 mL of 1.4 × 10^-6 M NaBr,what will occur? For AgBr,K_sp = 5 × 10^-13.

(Multiple Choice)

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Question 79

Which of the following indicators is most suitable for the titration of a 25.00-mL sample of 0.140 M propionic acid,HC₃H₅O₂,with strong base?

(Multiple Choice)

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Question 80

Showing 61 - 80 of 86

Exam 17: Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

What is the pH of the buffer that results when 32 g sodium acetate (NaCH3CO2)is mixed with 500.0 mL of 1.0 M acetic acid (CH3CO2H)and diluted with water to 1.0 L? (Ka of CH3CO2H = 1.8 × 10-5)

What molar ratio of acetic acid to sodium acetate is required to create a buffer solution having a pH of 4.88 at 25°C? Ka for HC2H3O2 is 1.8 × 10-5.

What mass of sodium hydroxide must be added to 65.0 mL of 0.926 M acetic acid in order to create a buffer with a pH of 4.83? Ka for acetic acid is 1.8 × 10-5.

Suppose 50.00 mL of 2.0 × 10-5 M Fe(NO3)3 is added to 50.00 mL of 2.0 ×10-4 M KIO3.Which of the following statements is true? For Fe(IO3)3,Ksp = 1.0 × 10-14.

A 50.00-mL solution of 0.0426 M trimethylamine (Kb = 6.5 × 10-5)is titrated with a 0.0257 M solution of hydrochloric acid as the titrant.What is the pH of the base solution after 22.31 mL of titrant have been added? (Kw = 1.00 × 10-14)

What is the pH at the equivalence point when a 25.0 mL sample of 0.200 M aqueous formic acid (HCO2H)is titrated with 0.100 M aqueous potassium hydroxide? (Ka of HCO2H = 1.8 × 10-4)

Two important biological buffer systems control pH in the range of 6.9 to 7.4.These buffer systems are H2CO3/HCO3- and _____.

What is the maximum hydroxide-ion concentration that a 0.019 M MgCl2 solution could have without causing the precipitation of Mg(OH)2? For Mg(OH)2,Ksp = 1.8 × 10-11.

What will be the pH of the solution when 0.10 mol of H+ ion is added to a 2.0 liter buffered solution composed of 0.45 M ammonia,NH3,and 0.26 M ammonium fluoride,NH4F? (Kb for ammonia = 1.8 × 10-5)

The hydroxide ion concentration of a saturated solution of Fe(OH)2 is M.What is the solubility product constant for Fe(OH)2?

What is the pH of a buffer that results when 0.50 mole of H3PO4 is mixed with 0.75 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are Ka1 = 7.5 × 10-3,Ka2 = 6.2 × 10-8,and Ka3 = 3.6 × 10-13)

How many moles of solid NaF would have to be added to 1.0 L of 2.16 M HF solution to achieve a buffer of pH 3.35? Assume there is no volume change.(Ka for HF = 7.2 × 10-4)

If 25 mL of 0.750 M HCl are added to 100.mL of 0.302 M NaOH,what is the final pH?

If 20 mL of 0.10 M NaOH is added to 40 mL of 0.20 M HC2H3O2,what is the pH of the resulting solution at 25°C? Ka for HC2H3O2 is 1.8 × 10-5 at 25°C.

What is the minimum mass of Na2CO3 (molar mass = 105.990 g/mol)that must be added to 43.4 mL of a 1.0 × 10-4 M AgNO3 solution in order for precipitation to occur? The Ksp of Ag2CO3 is 8.6 × 10-12.Assume no volume change occurs upon addition of Na2CO3.

When a weak base is titrated with a strong acid,the pH at the equivalence point is _____.

All of the following statements concerning acid-base buffers are true EXCEPT

If 0.50 L of a buffer containing 1.0 mol H2PO4− and 1.0 mol HPO42− is diluted to a volume of 5.0 L,the pH

If 500 mL of 1.4 × 10-6 M AgNO3 is mixed with 500 mL of 1.4 × 10-6 M NaBr,what will occur? For AgBr,Ksp = 5 × 10-13.

Which of the following indicators is most suitable for the titration of a 25.00-mL sample of 0.140 M propionic acid,HC3H5O2,with strong base?

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What is the pH of the buffer that results when 32 g sodium acetate (NaCH₃CO₂)is mixed with 500.0 mL of 1.0 M acetic acid (CH₃CO₂H)and diluted with water to 1.0 L? (K_a of CH₃CO₂H = 1.8 × 10^-5)

What molar ratio of acetic acid to sodium acetate is required to create a buffer solution having a pH of 4.88 at 25°C? K_a for HC₂H₃O₂ is 1.8 × 10^-5.

What mass of sodium hydroxide must be added to 65.0 mL of 0.926 M acetic acid in order to create a buffer with a pH of 4.83? K_a for acetic acid is 1.8 × 10^-5.

Suppose 50.00 mL of 2.0 × 10^-5 M Fe(NO₃)₃ is added to 50.00 mL of 2.0 ×10^-4 M KIO₃.Which of the following statements is true? For Fe(IO₃)₃,K_sp = 1.0 × 10^-14.

A 50.00-mL solution of 0.0426 M trimethylamine (K_b = 6.5 × 10^-5)is titrated with a 0.0257 M solution of hydrochloric acid as the titrant.What is the pH of the base solution after 22.31 mL of titrant have been added? (K_w = 1.00 × 10^-14)

What is the pH at the equivalence point when a 25.0 mL sample of 0.200 M aqueous formic acid (HCO₂H)is titrated with 0.100 M aqueous potassium hydroxide? (K_a of HCO₂H = 1.8 × 10^-4)

Two important biological buffer systems control pH in the range of 6.9 to 7.4.These buffer systems are H₂CO₃/HCO₃^- and _____.

What is the maximum hydroxide-ion concentration that a 0.019 M MgCl₂ solution could have without causing the precipitation of Mg(OH)₂? For Mg(OH)₂,K_sp = 1.8 × 10^-11.

What will be the pH of the solution when 0.10 mol of H⁺ ion is added to a 2.0 liter buffered solution composed of 0.45 M ammonia,NH3,and 0.26 M ammonium fluoride,NH₄F? (K_b for ammonia = 1.8 × 10^-5)

The hydroxide ion concentration of a saturated solution of Fe(OH)₂ is M.What is the solubility product constant for Fe(OH)₂?

What is the pH of a buffer that results when 0.50 mole of H₃PO₄ is mixed with 0.75 mole of NaOH and diluted with water to 1.00 L? (The acid dissociation constants of phosphoric acid are K_a1 = 7.5 × 10^-3,K_a2 = 6.2 × 10^-8,and K_a3 = 3.6 × 10^-13)

How many moles of solid NaF would have to be added to 1.0 L of 2.16 M HF solution to achieve a buffer of pH 3.35? Assume there is no volume change.(K_a for HF = 7.2 × 10^-4)

If 20 mL of 0.10 M NaOH is added to 40 mL of 0.20 M HC₂H₃O₂,what is the pH of the resulting solution at 25°C? K_a for HC₂H₃O₂ is 1.8 × 10^-5 at 25°C.

What is the minimum mass of Na₂CO₃ (molar mass = 105.990 g/mol)that must be added to 43.4 mL of a 1.0 × 10^-4 M AgNO₃ solution in order for precipitation to occur? The K_sp of Ag₂CO₃ is 8.6 × 10^-12.Assume no volume change occurs upon addition of Na₂CO₃.

If 0.50 L of a buffer containing 1.0 mol H₂PO₄− and 1.0 mol HPO₄²⁻ is diluted to a volume of 5.0 L,the pH

If 500 mL of 1.4 × 10^-6 M AgNO₃ is mixed with 500 mL of 1.4 × 10^-6 M NaBr,what will occur? For AgBr,K_sp = 5 × 10^-13.

Which of the following indicators is most suitable for the titration of a 25.00-mL sample of 0.140 M propionic acid,HC₃H₅O₂,with strong base?