When NH4Cl is dissolved in water the following species will be present: NH4+, Cl - OH - , H3O+, and NH3. Which of the following represents the correct relationship between the species in solution?

A) [NH4+] [Cl - ] > [OH - ] > [NH3] > [H3O+] B) [NH4+] [Cl - ] > [NH3] [H3O+] > [OH - ] C) [NH4+] [Cl - ] > [NH3] [OH - ] > [H3O+] D) [NH3] [OH - ] [Cl - ] > [NH4+] [H3O+] E) [NH3] [H3O+] [Cl - ] > [NH4+] [OHF - ] A) [NH4+] [Cl - ] > [OH - ] > [NH3] > [H3O+] B) [NH4+] [Cl - ] > [NH3] [H3O+] > [OH - ] C) [NH4+] [Cl - ] > [NH3] [OH - ] > [H3O+] D) [NH3] [OH - ] [Cl - ] > [NH4+] [H3O+] E) [NH3] [H3O+] [Cl - ] > [NH4+] [OHF - ]

A solution is known to have a hydronium ion concentration of 1.0 x 10-6 M. What percentage of the total H3O+ ion concentration comes from the dissociation of water?

A) 1% B) 3% C) 5% D) 10% E) 100% A) 1% B) 3% C) 5% D) 10% E) 100%

Which of the following compounds aren't acids in water? (I) NH4Cl (II) HNO3 (III) NH3 (IV) HI (V) K2S

A) I and II B) II and III C) III and V D) I, II and IV E) all of the above are acids in water A) I and II B) II and III C) III and V D) I, II and IV E) all of the above are acids in water

Which of the following equations can be used to calculate Kb1 and Kb2 for Na2Gly from Ka1 and Ka2 for H2Gly?

A) Kb1 = Kw x Ka1 &emsp; and &emsp; Kb2 = Kw x Ka2 B) Kb1 = Kw/Ka1 &emsp; and &emsp; Kb2 = Kw/Ka2 C) Kb1 = Ka1/Kw &emsp; and &emsp; Kb2 = Ka1/Kw D) Kb1 = Kw x Ka2 &emsp; and &emsp; Kb2 = Kw x Ka1 E) Kb1 = Kw/Ka2 &emsp; and &emsp; Kb2 = Kw/Ka1 A) Kb1 = Kw x Ka1 &emsp; and &emsp; Kb2 = Kw x Ka2 B) Kb1 = Kw/Ka1 &emsp; and &emsp; Kb2 = Kw/Ka2 C) Kb1 = Ka1/Kw &emsp; and &emsp; Kb2 = Ka1/Kw D) Kb1 = Kw x Ka2 &emsp; and &emsp; Kb2 = Kw x Ka1 E) Kb1 = Kw/Ka2 &emsp; and &emsp; Kb2 = Kw/Ka1

What is the pH of a 0.0250 M HClO4 solution.

A) 2.50 B) -2.50 C) 1.60 D) 12.40 E) none of these A) 2.50 B) -2.50 C) 1.60 D) 12.40 E) none of these

Exam 11: Acids and Bases

The dissociation of water into H₃O⁺ and OH^- is an endothermic process. As the temperature of pure water is raised, the degree to which water dissociates and the pH .

(Multiple Choice)

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Question 41

Which of the following acid-base reactions should go more or less to completion?

(Multiple Choice)

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Question 42

Sulfurous acid (H₂SO₃) is an acid and the sulfite ion (SO₃^2-) is a base. Which equation correctly describes the relationship between the equilibrium constants for these compounds?

(Multiple Choice)

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Question 43

When NH₄Cl is dissolved in water the following species will be present: NH₄⁺, Cl ^- OH ^- , H₃O⁺, and NH₃. Which of the following represents the correct relationship between the species in solution?

(Multiple Choice)

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Question 44

A solution is known to have a hydronium ion concentration of 1.0 x 10^-6 M. What percentage of the total H₃O⁺ ion concentration comes from the dissociation of water?

(Multiple Choice)

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Question 45

Which of the following compounds is not an Arrhenius base?

(Multiple Choice)

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Question 46

Which of the following represents a conjugate acid/base pair?

(Multiple Choice)

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Question 47

NaHCO₃ can be used to neutralize strong bases, such as NaOH. What conclusion can be drawn from the fact that the following acid-base reaction proceeds to the right as written? HCO₃^-(aq) + OH^-(aq) CO₃^2-(aq) + H₂O(l)

(Multiple Choice)

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Question 48

Which equation best describes a 0.10 M solution of a strong acid such as hydroiodic acid (HI: K_a = 3 x 10⁹)?

(Multiple Choice)

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Question 49

Which of the following compounds aren't acids in water? (I) NH₄Cl (II) HNO₃ (III) NH₃ (IV) HI (V) K₂S

(Multiple Choice)

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Question 50

Use the relationship between K_a1 and K_a2 for H₂SO₃ and K_b1 and K_b2 for the SO₃^2- ion to predict whether a 0.10 M solution of the HSO₃^- (bisulfite) ion would be acidic, basic or neutral. (H₂SO₃: K_a1 = 1.7 x 10^-2, K_a2 = 6.4 x 10^-8)

(Multiple Choice)

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Question 51

For a particular weak acid, HA, in pure water, as the initial concentration of the weak acid increases, the acid-dissociation equilibrium constant of that acid should

(Multiple Choice)

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Question 52

Which of the following equations can be used to calculate K_b1 and K_b2 for Na₂Gly from K_a1 and K_a2 for H₂Gly?

(Multiple Choice)

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Question 53

When 1.0 x 10^-5 mole of HOCl (K_a = 3.5 x 10^-8) is dissolved in pure water and diluted to 1.00 L, which assumption can't be applied in the calculation of the pH of this solution?

(Multiple Choice)

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Question 54

Predict the products of the following acid-base reaction. NaOCH₃(aq) + NaHCO₃(aq)

(Essay)

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Question 55

Which of the following solutions has a pH greater than 7.0?

(Multiple Choice)

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Question 56

What is the pH of a 0.0250 M HClO₄ solution.

(Multiple Choice)

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Question 57

Which of the following solutions has the highest pH?

(Multiple Choice)

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Question 58

Which of the following compounds is not an Arrhenius acid?

(Multiple Choice)

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Question 59

What can we conclude from the fact that the following reaction proceeds as written? NaNH₂(s) + H₂O(l) NH₃(aq) + OH^-(aq)

(Multiple Choice)

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Question 60

Showing 41 - 60 of 125

The dissociation of water into H₃O⁺ and OH^- is an endothermic process. As the temperature of pure water is raised, the degree to which water dissociates and the pH .

Which of the following acid-base reactions should go more or less to completion?

Sulfurous acid (H₂SO₃) is an acid and the sulfite ion (SO₃^2-) is a base. Which equation correctly describes the relationship between the equilibrium constants for these compounds?

When NH₄Cl is dissolved in water the following species will be present: NH₄⁺, Cl ^- OH ^- , H₃O⁺, and NH₃. Which of the following represents the correct relationship between the species in solution?

A solution is known to have a hydronium ion concentration of 1.0 x 10^-6 M. What percentage of the total H₃O⁺ ion concentration comes from the dissociation of water?

Which of the following compounds is not an Arrhenius base?

Which of the following represents a conjugate acid/base pair?

NaHCO₃ can be used to neutralize strong bases, such as NaOH. What conclusion can be drawn from the fact that the following acid-base reaction proceeds to the right as written? HCO₃^-(aq) + OH^-(aq) CO₃^2-(aq) + H₂O(l)

Which equation best describes a 0.10 M solution of a strong acid such as hydroiodic acid (HI: K_a = 3 x 10⁹)?

Which of the following compounds aren't acids in water? (I) NH₄Cl (II) HNO₃ (III) NH₃ (IV) HI (V) K₂S

Use the relationship between K_a1 and K_a2 for H₂SO₃ and K_b1 and K_b2 for the SO₃^2- ion to predict whether a 0.10 M solution of the HSO₃^- (bisulfite) ion would be acidic, basic or neutral. (H₂SO₃: K_a1 = 1.7 x 10^-2, K_a2 = 6.4 x 10^-8)

For a particular weak acid, HA, in pure water, as the initial concentration of the weak acid increases, the acid-dissociation equilibrium constant of that acid should

Which of the following equations can be used to calculate K_b1 and K_b2 for Na₂Gly from K_a1 and K_a2 for H₂Gly?

When 1.0 x 10^-5 mole of HOCl (K_a = 3.5 x 10^-8) is dissolved in pure water and diluted to 1.00 L, which assumption can't be applied in the calculation of the pH of this solution?

Predict the products of the following acid-base reaction. NaOCH₃(aq) + NaHCO₃(aq)

Which of the following solutions has a pH greater than 7.0?

What is the pH of a 0.0250 M HClO₄ solution.

Which of the following solutions has the highest pH?

Which of the following compounds is not an Arrhenius acid?

What can we conclude from the fact that the following reaction proceeds as written? NaNH₂(s) + H₂O(l) NH₃(aq) + OH^-(aq)

Elements Compounds

The Mole

Structure of the Atom

The Covalent Bond

Ionic and Metallic Bonds

Gases

Making and Breaking of Bonds

Liquids and Solutions

Solids

An Introduction to Kinetics and Equilibrium

Oxidation-Reduction Reactions

Chemical Thermodynamics

Kinetics

Nuclear Chemistry

Organic Chemistry

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Exam 11: Acids and Bases

The dissociation of water into H3O+ and OH- is an endothermic process. As the temperature of pure water is raised, the degree to which water dissociates ________ and the pH ________.

Which of the following acid-base reactions should go more or less to completion?

Sulfurous acid (H2SO3) is an acid and the sulfite ion (SO32-) is a base. Which equation correctly describes the relationship between the equilibrium constants for these compounds?

When NH4Cl is dissolved in water the following species will be present: NH4+, Cl - OH - , H3O+, and NH3. Which of the following represents the correct relationship between the species in solution?

A solution is known to have a hydronium ion concentration of 1.0 x 10-6 M. What percentage of the total H3O+ ion concentration comes from the dissociation of water?

Which of the following compounds is not an Arrhenius base?

Which of the following represents a conjugate acid/base pair?

NaHCO3 can be used to neutralize strong bases, such as NaOH. What conclusion can be drawn from the fact that the following acid-base reaction proceeds to the right as written? HCO3-(aq) + OH-(aq) CO32-(aq) + H2O(l)

Which equation best describes a 0.10 M solution of a strong acid such as hydroiodic acid (HI: Ka = 3 x 109)?

Which of the following compounds aren't acids in water? (I) NH4Cl (II) HNO3 (III) NH3 (IV) HI (V) K2S

Use the relationship between Ka1 and Ka2 for H2SO3 and Kb1 and Kb2 for the SO32- ion to predict whether a 0.10 M solution of the HSO3- (bisulfite) ion would be acidic, basic or neutral. (H2SO3: Ka1 = 1.7 x 10-2, Ka2 = 6.4 x 10-8)

For a particular weak acid, HA, in pure water, as the initial concentration of the weak acid increases, the acid-dissociation equilibrium constant of that acid should

Which of the following equations can be used to calculate Kb1 and Kb2 for Na2Gly from Ka1 and Ka2 for H2Gly?

When 1.0 x 10-5 mole of HOCl (Ka = 3.5 x 10-8) is dissolved in pure water and diluted to 1.00 L, which assumption can't be applied in the calculation of the pH of this solution?

Predict the products of the following acid-base reaction. NaOCH3(aq) + NaHCO3(aq)

Which of the following solutions has a pH greater than 7.0?

What is the pH of a 0.0250 M HClO4 solution.

Which of the following solutions has the highest pH?

Which of the following compounds is not an Arrhenius acid?

What can we conclude from the fact that the following reaction proceeds as written? NaNH2(s) + H2O(l) NH3(aq) + OH-(aq)

Elements Compounds

The Mole

Structure of the Atom

The Covalent Bond

Ionic and Metallic Bonds

Gases

Making and Breaking of Bonds

Liquids and Solutions

Solids

An Introduction to Kinetics and Equilibrium

Oxidation-Reduction Reactions

Chemical Thermodynamics

Kinetics

Nuclear Chemistry

Organic Chemistry

Filters

The dissociation of water into H₃O⁺ and OH^- is an endothermic process. As the temperature of pure water is raised, the degree to which water dissociates and the pH .

Sulfurous acid (H₂SO₃) is an acid and the sulfite ion (SO₃^2-) is a base. Which equation correctly describes the relationship between the equilibrium constants for these compounds?

When NH₄Cl is dissolved in water the following species will be present: NH₄⁺, Cl ^- OH ^- , H₃O⁺, and NH₃. Which of the following represents the correct relationship between the species in solution?

A solution is known to have a hydronium ion concentration of 1.0 x 10^-6 M. What percentage of the total H₃O⁺ ion concentration comes from the dissociation of water?

NaHCO₃ can be used to neutralize strong bases, such as NaOH. What conclusion can be drawn from the fact that the following acid-base reaction proceeds to the right as written? HCO₃^-(aq) + OH^-(aq) CO₃^2-(aq) + H₂O(l)

Which equation best describes a 0.10 M solution of a strong acid such as hydroiodic acid (HI: K_a = 3 x 10⁹)?

Which of the following compounds aren't acids in water? (I) NH₄Cl (II) HNO₃ (III) NH₃ (IV) HI (V) K₂S

Use the relationship between K_a1 and K_a2 for H₂SO₃ and K_b1 and K_b2 for the SO₃^2- ion to predict whether a 0.10 M solution of the HSO₃^- (bisulfite) ion would be acidic, basic or neutral. (H₂SO₃: K_a1 = 1.7 x 10^-2, K_a2 = 6.4 x 10^-8)

Which of the following equations can be used to calculate K_b1 and K_b2 for Na₂Gly from K_a1 and K_a2 for H₂Gly?

When 1.0 x 10^-5 mole of HOCl (K_a = 3.5 x 10^-8) is dissolved in pure water and diluted to 1.00 L, which assumption can't be applied in the calculation of the pH of this solution?

Predict the products of the following acid-base reaction. NaOCH₃(aq) + NaHCO₃(aq)

What is the pH of a 0.0250 M HClO₄ solution.

What can we conclude from the fact that the following reaction proceeds as written? NaNH₂(s) + H₂O(l) NH₃(aq) + OH^-(aq)