A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 0.00 mL of KOH is ________ M.

A) 0.0181 B) 0.430 C) 0.723 D) 0.273 E) none of the above A) 0.0181 B) 0.430 C) 0.723 D) 0.273 E) none of the above

Calculate the pH of a solution that is 0.322 M in nitrous acid (HNO2)and 0.178 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is 4.50 × 10-4.

A) 3.093 B) 3.607 C) 14.26 D) 10.91 E) 4.589 A) 3.093 B) 3.607 C) 14.26 D) 10.91 E) 4.589

Determine the Ksp for magnesium hydroxide (Mg(OH)2)where the solubility of Mg(OH)2 is 1.4 × 10-4 M.

A) 2.7 × 10-12 B) 1.1 × 10-11 C) 2.0 × 10-8 D) 3.9 × 10-8 E) 1.4 × 10-4 A) 2.7 × 10-12 B) 1.1 × 10-11 C) 2.0 × 10-8 D) 3.9 × 10-8 E) 1.4 × 10-4

What is the molar solubility of calcium carbonate ( CaCO3 )in water? The solubility-product constant for CaCO3 is 4.5 × 10-9 at 25 °C.

A) 2.3 × 10-9 B) 9.0 × 10-9 C) 8.35 D) 9.5 × 10-5 E) 6.7 × 10-5 A) 2.3 × 10-9 B) 9.0 × 10-9 C) 8.35 D) 9.5 × 10-5 E) 6.7 × 10-5

Calculate the percent ionization of nitrous acid in a solution that is 0.241 M in nitrous acid (HNO2)and 0.195 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is 4.50 × 10-4.

A) 44.7 B) 0.229 C) 13.5 D) 2.11 × 10-3 E) 3.258 A) 44.7 B) 0.229 C) 13.5 D) 2.11 × 10-3 E) 3.258

The pH of a solution prepared by dissolving 0.350 mol of solid methylamine hydrochloride (CH3NH3Cl)in 1.00 L of 1.10 M methylamine (CH3NH2)is ________. The Kb for methylamine is 4.40 × 10-4. (Assume the final volume is 1.00 L.)

A) 1.66 B) 2.86 C) 10.28 D) 11.14 E) 10.61 A) 1.66 B) 2.86 C) 10.28 D) 11.14 E) 10.61

Exam 17: Additional Aspects of Aqueous Equilibria

A 25.0-mL sample of 0.150 M hydrocyanic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The K_a of hydrocyanic acid is 4.9 × 10^-10.

(Multiple Choice)

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Question 81

analysis determines only the presence or absence of a particular metal ion, whereas analysis determines how much of a given substance is present.

(Short Answer)

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Question 82

A buffer solution with a pH of 4.63 is prepared with 0.14 M formic acid and ________ M sodium formate. The K_a of formic acid is 1.8 × 10^-4.

(Multiple Choice)

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Question 83

A 25.0 mL sample of 0.723 M HClO₄ is titrated with a 0.273 M KOH solution. The H₃O⁺ concentration after the addition of 0.00 mL of KOH is ________ M.

(Multiple Choice)

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Question 84

Which of the following could be added to a solution of acetic acid to prepare a buffer?

(Multiple Choice)

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Question 85

In general, the solubility of a slightly soluble salt is ________ by the presence of a second solute that furnishes a common ion.

(Short Answer)

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Question 86

Calculate the pH of a solution that is 0.322 M in nitrous acid (HNO₂)and 0.178 M in potassium nitrite (KNO₂). The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

(Multiple Choice)

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Question 87

Metal oxides and hydroxides that are relatively insoluble in neutral water, but are soluble in both strongly acidic and strongly basic solutions are said to be ________.

(Short Answer)

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Question 88

Determine the K_sp for magnesium hydroxide (Mg(OH)₂)where the solubility of Mg(OH)₂ is 1.4 × 10^-4 M.

(Multiple Choice)

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Question 89

-A 25.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The unknown compound is ________.

(Multiple Choice)

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Question 90

A solution is prepared by dissolving 0.23 mol of benzoic acid and 0.27 mol of sodium benzoate in water sufficient to yield 1.00 L of solution.The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. The pH does not increase drastically because the NaOH reacts with the ________ present in the buffer solution. The K_a of benzoic acid is 6.3 × 10^-5.

(Multiple Choice)

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Question 91

What is the molar solubility of calcium carbonate ( CaCO₃ )in water? The solubility-product constant for CaCO₃ is 4.5 × 10^-9 at 25 °C.

(Multiple Choice)

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Question 92

Calculate the percent ionization of nitrous acid in a solution that is 0.241 M in nitrous acid (HNO₂)and 0.195 M in potassium nitrite (KNO₂). The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

(Multiple Choice)

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Question 93

Which one of the following will cause hemoglobin to release oxygen?

(Multiple Choice)

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Question 94

How many milliliters of 0.0839 M NaOH are required to titrate 25.0 mL of 0.0990 M HBr to the equivalence point?

(Multiple Choice)

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Question 95

Although CaCO₃ has a relatively small solubility product, it is quite soluble in the presence of ________.

(Short Answer)

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Question 96

The K_a of benzoic acid is 6.30 × 10^-5. The pH of a buffer prepared by combining 50.0 mL of 1.00 M potassium benzoate and 50.0 mL of 1.00 M benzoic acid is ________.

(Multiple Choice)

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Question 97

A buffer solution with a pH of 4.78 is prepared with ________ M formic acid and 0.90 M sodium formate. The K_a of formic acid is 1.8 × 10^-4.

(Multiple Choice)

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Question 98

Why does fluoride treatment render teeth more resistant to decay?

(Multiple Choice)

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Question 99

The pH of a solution prepared by dissolving 0.350 mol of solid methylamine hydrochloride (CH₃NH₃Cl)in 1.00 L of 1.10 M methylamine (CH₃NH₂)is ________. The K_b for methylamine is 4.40 × 10^-⁴. (Assume the final volume is 1.00 L.)

(Multiple Choice)

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Question 100

Showing 81 - 100 of 116

Exam 17: Additional Aspects of Aqueous Equilibria

A 25.0-mL sample of 0.150 M hydrocyanic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The Ka of hydrocyanic acid is 4.9 × 10-10.

________ analysis determines only the presence or absence of a particular metal ion, whereas ________ analysis determines how much of a given substance is present.

A buffer solution with a pH of 4.63 is prepared with 0.14 M formic acid and ________ M sodium formate. The Ka of formic acid is 1.8 × 10-4.

A 25.0 mL sample of 0.723 M HClO4 is titrated with a 0.273 M KOH solution. The H3O+ concentration after the addition of 0.00 mL of KOH is ________ M.

Which of the following could be added to a solution of acetic acid to prepare a buffer?

In general, the solubility of a slightly soluble salt is ________ by the presence of a second solute that furnishes a common ion.

Calculate the pH of a solution that is 0.322 M in nitrous acid (HNO2)and 0.178 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Metal oxides and hydroxides that are relatively insoluble in neutral water, but are soluble in both strongly acidic and strongly basic solutions are said to be ________.

Determine the Ksp for magnesium hydroxide (Mg(OH)2)where the solubility of Mg(OH)2 is 1.4 × 10-4 M.

-A 25.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The unknown compound is ________.

What is the molar solubility of calcium carbonate ( CaCO3 )in water? The solubility-product constant for CaCO3 is 4.5 × 10-9 at 25 °C.

Calculate the percent ionization of nitrous acid in a solution that is 0.241 M in nitrous acid (HNO2)and 0.195 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is 4.50 × 10-4.

Which one of the following will cause hemoglobin to release oxygen?

How many milliliters of 0.0839 M NaOH are required to titrate 25.0 mL of 0.0990 M HBr to the equivalence point?

Although CaCO3 has a relatively small solubility product, it is quite soluble in the presence of ________.

The Ka of benzoic acid is 6.30 × 10-5. The pH of a buffer prepared by combining 50.0 mL of 1.00 M potassium benzoate and 50.0 mL of 1.00 M benzoic acid is ________.

A buffer solution with a pH of 4.78 is prepared with ________ M formic acid and 0.90 M sodium formate. The Ka of formic acid is 1.8 × 10-4.

Why does fluoride treatment render teeth more resistant to decay?

The pH of a solution prepared by dissolving 0.350 mol of solid methylamine hydrochloride (CH3NH3Cl)in 1.00 L of 1.10 M methylamine (CH3NH2)is ________. The Kb for methylamine is 4.40 × 10-4. (Assume the final volume is 1.00 L.)

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A 25.0-mL sample of 0.150 M hydrocyanic acid is titrated with a 0.150 M NaOH solution. What is the pH before any base is added? The K_a of hydrocyanic acid is 4.9 × 10^-10.

analysis determines only the presence or absence of a particular metal ion, whereas analysis determines how much of a given substance is present.

A buffer solution with a pH of 4.63 is prepared with 0.14 M formic acid and ________ M sodium formate. The K_a of formic acid is 1.8 × 10^-4.

A 25.0 mL sample of 0.723 M HClO₄ is titrated with a 0.273 M KOH solution. The H₃O⁺ concentration after the addition of 0.00 mL of KOH is ________ M.

Calculate the pH of a solution that is 0.322 M in nitrous acid (HNO₂)and 0.178 M in potassium nitrite (KNO₂). The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

Determine the K_sp for magnesium hydroxide (Mg(OH)₂)where the solubility of Mg(OH)₂ is 1.4 × 10^-4 M.

What is the molar solubility of calcium carbonate ( CaCO₃ )in water? The solubility-product constant for CaCO₃ is 4.5 × 10^-9 at 25 °C.

Calculate the percent ionization of nitrous acid in a solution that is 0.241 M in nitrous acid (HNO₂)and 0.195 M in potassium nitrite (KNO₂). The acid dissociation constant of nitrous acid is 4.50 × 10^-4.

Although CaCO₃ has a relatively small solubility product, it is quite soluble in the presence of ________.

The K_a of benzoic acid is 6.30 × 10^-5. The pH of a buffer prepared by combining 50.0 mL of 1.00 M potassium benzoate and 50.0 mL of 1.00 M benzoic acid is ________.

A buffer solution with a pH of 4.78 is prepared with ________ M formic acid and 0.90 M sodium formate. The K_a of formic acid is 1.8 × 10^-4.

The pH of a solution prepared by dissolving 0.350 mol of solid methylamine hydrochloride (CH₃NH₃Cl)in 1.00 L of 1.10 M methylamine (CH₃NH₂)is ________. The K_b for methylamine is 4.40 × 10^-⁴. (Assume the final volume is 1.00 L.)