What is the hydroxide-ion concentration in a 0.10 M solution of Na2CO3? For carbonic acid, Ka1 = 4.2 × 10-7 and Ka2 = 4.8 × 10-11. (Kw = 1.0 × 10-14)

A) 4.6 × 10-3 M B) 2.0 × 10-4 M C) 4.9 × 10-5 M D) 4.2 × 10-9 M E) 2.2 × 10-6 M A) 4.6 × 10-3 M B) 2.0 × 10-4 M C) 4.9 × 10-5 M D) 4.2 × 10-9 M E) 2.2 × 10-6 M

What is the conjugate base of [Fe(H2O)6]3+(aq)?

A) H3O+ B) [Fe(H2O)6]2+ C) [Fe(H2O)5H3O]4+ D) [Fe(H2O)5OH]2+ E) [Fe(H2O)5]3+ A) H3O+ B) [Fe(H2O)6]2+ C) [Fe(H2O)5H3O]4+ D) [Fe(H2O)5OH]2+ E) [Fe(H2O)5]3+

What volume of water must be added to 14.4 mL of a pH 2.0 solution of HNO3 in order to change the pH to 4.0?

A) 14.4 mL B) 143 mL C) 1.43 × 103 mL D) 36 mL E) 86 mL A) 14.4 mL B) 143 mL C) 1.43 × 103 mL D) 36 mL E) 86 mL

What is the pH of a 0.33 M solution of methylamine (CH3NH2, Kb = 4.4 × 10-4) at 25oC? (Kw = 1.01 × 10-14)

A) 5.56 B) 0.48 C) 12.07 D) 13.52 E) 1.93 A) 5.56 B) 0.48 C) 12.07 D) 13.52 E) 1.93

Calculate the pH of a 1.7 M solution of H2A (Ka1 = 1.0 × 10-6 and Ka2 is 1.0 × 10-10).

A) 10.00 B) 2.88 C) 11.12 D) 5.77 E) 7.00 A) 10.00 B) 2.88 C) 11.12 D) 5.77 E) 7.00

Exam 17: Principles of Chemical Reactivity: the Chemistry of Acids and Bases

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What is the hydroxide-ion concentration in a 0.10 M solution of Na₂CO₃? For carbonic acid, K_a1 = 4.2 × 10^-7 and K_a2 = 4.8 × 10^-11. (K_w = 1.0 × 10^-14)

(Multiple Choice)

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Question 61

Identify from the following list of molecules and ions which behave as Lewis acids: CO₂, NH₃, BCl₃, and Fe³⁺.

(Multiple Choice)

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Question 62

Given that K_a for the weak acid HA is 3.49 × 10^-8, calculate K for the reaction of HA with OH^-. HA(aq) + OH?(aq) D A?(aq) + H₂O( $\ell$ )

(Multiple Choice)

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Question 63

Which of the following substances is never a Brønsted-Lowry base in an aqueous solution?

(Multiple Choice)

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Question 64

What is the pH of the solution which results from mixing 50.0 mL of 0.30 M HF(aq) and 50.0 mL of 0.30 M NaOH(aq) at 25 °C? (K_a of HF = 7.2 × 10^-4)

(Multiple Choice)

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Question 65

What is the conjugate base of [Fe(H₂O)₆]³⁺(aq)?

(Multiple Choice)

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Question 66

What volume of water must be added to 14.4 mL of a pH 2.0 solution of HNO₃ in order to change the pH to 4.0?

(Multiple Choice)

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Question 67

What is the hydronium-ion concentration of a 0.25 M solution of HCN (K_a = 4.9 × 10^-10) at 25°C?

(Multiple Choice)

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Question 68

Arrange the following acids in order of decreasing acid strength in aqueous solution: HBr, HOCl, HOBr, and HOI.

(Multiple Choice)

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Question 69

Aqueous solutions of ammonia (NH₃) and hydrogen cyanide (HCN) react to produce ammonium cyanide, (NH₄CN) according to the following equilibrium reaction. NH3(aq) + HCN(aq) D NH₄⁺(aq) + CN?(aq) Given the following equilibrium constants, which statement best describes the reaction once equilibrium is established? (K_w = 1.01 × 10^-14) =5.6\times1 =4.0\times1

(Multiple Choice)

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Question 70

What is the pH of a solution prepared by dissolving 0.459 L of HCl(g), measured at STP, in enough water such that the total volume of the solution is 5.50 L? (R = 0.0821 L · atm/K·mol)

(Multiple Choice)

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Question 71

The autoionization of pure water, as represented by the equation below, is known to be endothermic (?_r? > 0). Which of the following correctly states what occurs as the temperature of pure water is raised? H₂O(l) + H₂O(l) $\rightleftharpoons$ H₃O⁺(aq) + OH^-(aq) ?_r? > 0

(Multiple Choice)

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Question 72

Which of the following ionic compounds does not produce a basic aqueous solution at 25 °C?

(Multiple Choice)

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Question 73

The concentration of H₃O⁺ in a solution is 5 × 10^-4 M at 25°C. What is its hydroxide-ion concentration? (K_w = 1.01 × 10^-14)

(Multiple Choice)

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Question 74

What is the pH of a 0.33 M solution of methylamine (CH₃NH₂, K_b = 4.4 × 10^-4) at 25^oC? (K_w = 1.01 × 10^-14)

(Multiple Choice)

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Question 75

What is the equilibrium hydronium ion concentration of an initially 4.5 M solution of hypoiodous acid, HOI, at 25°C (K_a = $2.3 \times 10 ^ { - 11 }$ )?

(Multiple Choice)

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Question 76

At 25 °C, all of the following ions produce an acidic solution, except ____.

(Multiple Choice)

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Question 77

Calculate the pH of a 1.7 M solution of H₂A (K_a1= 1.0 × 10^-6 and K_a2 is 1.0 × 10^-10).

(Multiple Choice)

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Question 78

The chemical equations below show the reaction of Al(OH)₃ as a Lewis acid and as a Lewis base, respectively. Al(OH)₃(s) + OH^-(aq) $\rightleftharpoons$ Al(OH)₄^-(aq) Al(OH)₃(s) + 3 H₃O⁺(aq) $\rightleftharpoons$ Al³⁺(aq) + 3 H₂O( $\ell$ ) Substances that can behave as either Lewis acids or bases are called ________ substances.

(Short Answer)

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Question 79

An aqueous solution with a pH of 10.60 is diluted from 1.0 L to 2.0 L. What is the pH of the diluted solution?

(Multiple Choice)

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Question 80

Showing 61 - 80 of 97

Exam 17: Principles of Chemical Reactivity: the Chemistry of Acids and Bases

What is the hydroxide-ion concentration in a 0.10 M solution of Na2CO3? For carbonic acid, Ka1 = 4.2 × 10-7 and Ka2 = 4.8 × 10-11. (Kw = 1.0 × 10-14)

Identify from the following list of molecules and ions which behave as Lewis acids: CO2, NH3, BCl3, and Fe3+.

Given that Ka for the weak acid HA is 3.49 × 10-8, calculate K for the reaction of HA with OH-. HA(aq) + OH?(aq) D A?(aq) + H2O( ℓ\ellℓ )

Which of the following substances is never a Brønsted-Lowry base in an aqueous solution?

What is the pH of the solution which results from mixing 50.0 mL of 0.30 M HF(aq) and 50.0 mL of 0.30 M NaOH(aq) at 25 °C? (Ka of HF = 7.2 × 10-4)

What is the conjugate base of [Fe(H2O)6]3+(aq)?

What volume of water must be added to 14.4 mL of a pH 2.0 solution of HNO3 in order to change the pH to 4.0?

What is the hydronium-ion concentration of a 0.25 M solution of HCN (Ka = 4.9 × 10-10) at 25°C?

Arrange the following acids in order of decreasing acid strength in aqueous solution: HBr, HOCl, HOBr, and HOI.

What is the pH of a solution prepared by dissolving 0.459 L of HCl(g), measured at STP, in enough water such that the total volume of the solution is 5.50 L? (R = 0.0821 L · atm/K·mol)

The autoionization of pure water, as represented by the equation below, is known to be endothermic (?r? > 0). Which of the following correctly states what occurs as the temperature of pure water is raised? H2O(l) + H2O(l) ⇌\rightleftharpoons⇌ H3O+(aq) + OH-(aq) ?r? > 0

Which of the following ionic compounds does not produce a basic aqueous solution at 25 °C?

The concentration of H3O+ in a solution is 5 × 10-4 M at 25°C. What is its hydroxide-ion concentration? (Kw = 1.01 × 10-14)

What is the pH of a 0.33 M solution of methylamine (CH3NH2, Kb = 4.4 × 10-4) at 25oC? (Kw = 1.01 × 10-14)

What is the equilibrium hydronium ion concentration of an initially 4.5 M solution of hypoiodous acid, HOI, at 25°C (Ka = 2.3×10−112.3 \times 10 ^ { - 11 }2.3×10−11 )?

At 25 °C, all of the following ions produce an acidic solution, except ____.

Calculate the pH of a 1.7 M solution of H2A (Ka1 = 1.0 × 10-6 and Ka2 is 1.0 × 10-10).

An aqueous solution with a pH of 10.60 is diluted from 1.0 L to 2.0 L. What is the pH of the diluted solution?

Basic Concepts of Chemistry

Lets Review: the Tools of Quantitative Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

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Carbon: Not Just Another Element

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What is the hydroxide-ion concentration in a 0.10 M solution of Na₂CO₃? For carbonic acid, K_a1 = 4.2 × 10^-7 and K_a2 = 4.8 × 10^-11. (K_w = 1.0 × 10^-14)

Identify from the following list of molecules and ions which behave as Lewis acids: CO₂, NH₃, BCl₃, and Fe³⁺.

Given that K_a for the weak acid HA is 3.49 × 10^-8, calculate K for the reaction of HA with OH^-. HA(aq) + OH?(aq) D A?(aq) + H₂O( $\ell$ )

What is the pH of the solution which results from mixing 50.0 mL of 0.30 M HF(aq) and 50.0 mL of 0.30 M NaOH(aq) at 25 °C? (K_a of HF = 7.2 × 10^-4)

What is the conjugate base of [Fe(H₂O)₆]³⁺(aq)?

What volume of water must be added to 14.4 mL of a pH 2.0 solution of HNO₃ in order to change the pH to 4.0?

What is the hydronium-ion concentration of a 0.25 M solution of HCN (K_a = 4.9 × 10^-10) at 25°C?

The autoionization of pure water, as represented by the equation below, is known to be endothermic (?_r? > 0). Which of the following correctly states what occurs as the temperature of pure water is raised? H₂O(l) + H₂O(l) $\rightleftharpoons$ H₃O⁺(aq) + OH^-(aq) ?_r? > 0

The concentration of H₃O⁺ in a solution is 5 × 10^-4 M at 25°C. What is its hydroxide-ion concentration? (K_w = 1.01 × 10^-14)

What is the pH of a 0.33 M solution of methylamine (CH₃NH₂, K_b = 4.4 × 10^-4) at 25^oC? (K_w = 1.01 × 10^-14)

What is the equilibrium hydronium ion concentration of an initially 4.5 M solution of hypoiodous acid, HOI, at 25°C (K_a = $2.3 \times 10 ^ { - 11 }$ )?

Calculate the pH of a 1.7 M solution of H₂A (K_a1= 1.0 × 10^-6 and K_a2 is 1.0 × 10^-10).