Consider the Ka values for the following acids: Cyanic acid, HOCN, 3.5 × 10-4 Formic acid, HCHO2, 1.7 × 10-4 Lactic acid, HC3H5O3, 1.3 × 10-4 Propionic acid, HC3H5O2, 1.3 × 10-5 Benzoic acid, HC7H5O2, 6.3 × 10-5 Which of the following is the strongest acid?

A) Cyanic acid B) Propionic acid C) Bemzoic acid D) Formic acid E) Lactic acid A) Cyanic acid B) Propionic acid C) Bemzoic acid D) Formic acid E) Lactic acid

Which of the following statements about the reaction below is correct? HCO3-(aq) + H2O( $\ell$ ) $\rightleftharpoons$ CO32-(aq) + H3O+(aq)

A) H3O+ is an acid and HCO3- is its conjugate base. B) HCO3- is an acid and CO32- is its conjugate base. C) HCO3- is an acid and H2O is its conjugate base. D) H2O is an acid and CO32- is its conjugate base. E) H3O+ is an acid and CO32- is its conjugate base. A) H3O+ is an acid and HCO3- is its conjugate base. B) HCO3- is an acid and CO32- is its conjugate base. C) HCO3- is an acid and H2O is its conjugate base. D) H2O is an acid and CO32- is its conjugate base. E) H3O+ is an acid and CO32- is its conjugate base.

Which of the following is the correct hydronium ion ,H3O+,concentration of 0.0013 M KOH(aq) at 25 °C? (Kw = 1.01 × 10-14)

A) 7.7 × 10-12 M B) 1.3 × 10-3 M C) 1.0 × 10-14 M D) 1.0 × 10-7 M E) 1.3 × 10-17 M A) 7.7 × 10-12 M B) 1.3 × 10-3 M C) 1.0 × 10-14 M D) 1.0 × 10-7 M E) 1.3 × 10-17 M

Which of the following equations shows that isoquinoline, C9H7N, behaves as a Brønsted-Lowry base in water?

A) C9H7N(aq) + H2O(l) $\rightleftharpoons$ C9H7NH+(aq) + OH-(aq) B) C9H7N(aq) + H2O(l) $\rightleftharpoons$ C9H6N-(aq) + H3O+(aq) C) C9H7N(aq) + OH?(aq) $\rightleftharpoons$ C9H6N?(aq) + H2O(l) D) C9H7N(aq) + H3O+(aq) $\rightleftharpoons$ C9H7NH+(aq) + H2O(l) E) C9H7NH+(aq) + H2O(l) $\rightleftharpoons$ C9H7N(aq) + H3O+(aq) A) C9H7N(aq) + H2O(l) $\rightleftharpoons$ C9H7NH+(aq) + OH-(aq) B) C9H7N(aq) + H2O(l) $\rightleftharpoons$ C9H6N-(aq) + H3O+(aq) C) C9H7N(aq) + OH?(aq) $\rightleftharpoons$ C9H6N?(aq) + H2O(l) D) C9H7N(aq) + H3O+(aq) $\rightleftharpoons$ C9H7NH+(aq) + H2O(l) E) C9H7NH+(aq) + H2O(l) $\rightleftharpoons$ C9H7N(aq) + H3O+(aq)

What is the H3O+ concentration in 0.0055 M Ba(OH)2(aq) at 25 °C? (Kw = 1.01 × 10-14)?

A) 1.1 × 10-2 M B) 5.5 × 10-3 M C) 9.1 × 10-13 M D) 1.8 × 10-12 M E) 1.0 × 10-7 M A) 1.1 × 10-2 M B) 5.5 × 10-3 M C) 9.1 × 10-13 M D) 1.8 × 10-12 M E) 1.0 × 10-7 M

What is Ka at 25°C for the following equilibrium given Kb (CH3NH2) = 4.4 × 10-4 at 25°C.? CH3NH3+(aq) + H2O(l) $\rightleftharpoons$ CH3NH2(aq) + H3O+(aq)

A) 4.4 × 10-4 B) 2.3 × 103 C) 4.4 × 10-10 D) 4.4 × 104 E) 2.3 × 10-11 A) 4.4 × 10-4 B) 2.3 × 103 C) 4.4 × 10-10 D) 4.4 × 104 E) 2.3 × 10-11

At 50°C the autoionization constant for pure water, Kw, is $5.48 \times 10 ^ { - 14 }$ . What is the H3O+ concentration in pure water at 50°C?

A) $5.48 \times 10 ^ { - 14 }$ M B) 1.01 × 10-7 M C) $1.17 \times 10 ^ { - 7 }$ M D) $2.34 \times 10 ^ { - 7 }$ M E) 1.01 × 10-14 M A) $5.48 \times 10 ^ { - 14 }$ M B) 1.01 × 10-7 M C) $1.17 \times 10 ^ { - 7 }$ M D) $2.34 \times 10 ^ { - 7 }$ M E) 1.01 × 10-14 M

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

Explore all topics

What is the equilibrium constant for the following reaction, HCO₂H(aq) + CN^-(aq) $\rightleftharpoons$ HCO₂^-(aq) + HCN(aq) And does the reaction favor the formation of reactants or products? The acid dissociation constant, K_a, for HCO₂H is 1.8 × 10^-4 and the acid dissociation constant for HCN is 4.0 × 10^-10.

(Multiple Choice)

4.9/5

(35)

Question 41

Consider the K_a values for the following acids: Cyanic acid, HOCN, 3.5 × 10^-4Formic acid, HCHO₂, 1.7 × 10^-4Lactic acid, HC₃H₅O₃, 1.3 × 10^-4Propionic acid, HC₃H₅O₂, 1.3 × 10^-5 Benzoic acid, HC₇H₅O₂, 6.3 × 10^-5 Which of the following is the strongest acid?

(Multiple Choice)

4.9/5

(28)

Question 42

Hydrofluoric acid has a pK_a value of 3.14. What is the value of pK_b for fluoride ion?

(Multiple Choice)

4.8/5

(34)

Question 43

Which of the following statements about the reaction below is correct? HCO₃^-(aq) + H₂O( $\ell$ ) $\rightleftharpoons$ CO₃^2-(aq) + H₃O⁺(aq)

(Multiple Choice)

4.9/5

(42)

Question 44

H₃PO₃ is a diprotic weak acid. What is the balanced equilibrium defined as K_b2 of H₃PO₃?

(Multiple Choice)

4.8/5

(42)

Question 45

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

(Multiple Choice)

4.8/5

(35)

Question 46

When a Lewis acid combines with a Lewis base, the base supplies both the electrons to the bond. This type of chemical bond is called a(n) _____ covalent bond.

(Short Answer)

4.7/5

(31)

Question 47

What is the hydroxide-ion concentration in a solution formed by combining 200. mL of 0.15 M HCl with 300. mL of 0.090 M NaOH at 25°C? HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)

(Multiple Choice)

4.9/5

(44)

Question 48

Which of the following is the correct hydronium ion ,H₃O⁺,concentration of 0.0013 M KOH(aq) at 25 °C? (K_w = 1.01 × 10^-14)

(Multiple Choice)

4.9/5

(35)

Question 49

What is the OH^- concentration of an aqueous solution with a pH of 9.83? (K_w = 1.01 × 10^-14)

(Multiple Choice)

4.8/5

(39)

Question 50

A solution has a hydroxide ion concentration of 0.0040 M. Calculate the pOH of the solution at 25 °C. (K_w = 1.01 × 10^-14)

(Multiple Choice)

4.9/5

(37)

Question 51

Which of the following equations shows that isoquinoline, C₉H₇N, behaves as a Brønsted-Lowry base in water?

(Multiple Choice)

4.7/5

(39)

Question 52

Which equation depicts the hydrogen phosphate ion behaving as a Brønsted-Lowry base in water?

(Multiple Choice)

4.8/5

(40)

Question 53

Which of the following is the correct hydroxide ion concentration in 0.48 M CH₃CO₂^-(aq)? (K_b of CH₃CO₂^- = 5.6 × 10^-10)

(Multiple Choice)

4.7/5

(39)

Question 54

Carbonic acid is a diprotic acid, H₂CO₃, with K_a1 = 4.2 × 10^-7 and K_a2 = 4.8 × 10^-11 at 25°C. The ion product for water is K_w = 1.0 × 10^-14 at 25°C. What is the OH^- concentration of a solution that is 0.39 M in Na₂CO₃?

(Multiple Choice)

4.9/5

(43)

Question 55

What is the H₃O⁺ concentration in 0.0055 M Ba(OH)₂(aq) at 25 °C? (K_w = 1.01 × 10^-14)?

(Multiple Choice)

4.8/5

(30)

Question 56

Which of the following expressions is not equivalent to the formula of pH?

(Multiple Choice)

4.8/5

(40)

Question 57

What is K_a at 25°C for the following equilibrium given K_b (CH₃NH₂) = 4.4 × 10^-4 at 25°C.? CH₃NH₃⁺(aq) + H₂O(l) $\rightleftharpoons$ CH₃NH₂(aq) + H₃O⁺(aq)

(Multiple Choice)

4.8/5

(34)

Question 58

When a Lewis acid and a Lewis base combine, the product may be referred to as an acid-base ________.

(Short Answer)

4.8/5

(46)

Question 59

At 50°C the autoionization constant for pure water, K_w, is $5.48 \times 10 ^ { - 14 }$ . What is the H₃O⁺ concentration in pure water at 50°C?

(Multiple Choice)

4.9/5

(40)

Question 60

Showing 41 - 60 of 97

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

Consider the Ka values for the following acids: Cyanic acid, HOCN, 3.5 × 10-4 Formic acid, HCHO2, 1.7 × 10-4 Lactic acid, HC3H5O3, 1.3 × 10-4 Propionic acid, HC3H5O2, 1.3 × 10-5 Benzoic acid, HC7H5O2, 6.3 × 10-5 Which of the following is the strongest acid?

Hydrofluoric acid has a pKa value of 3.14. What is the value of pKb for fluoride ion?

Which of the following statements about the reaction below is correct? HCO3-(aq) + H2O( ℓ\ellℓ ) ⇌\rightleftharpoons⇌ CO32-(aq) + H3O+(aq)

H3PO3 is a diprotic weak acid. What is the balanced equilibrium defined as Kb2 of H3PO3?

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

When a Lewis acid combines with a Lewis base, the base supplies both the electrons to the bond. This type of chemical bond is called a(n) _____ covalent bond.

What is the hydroxide-ion concentration in a solution formed by combining 200. mL of 0.15 M HCl with 300. mL of 0.090 M NaOH at 25°C? HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

Which of the following is the correct hydronium ion ,H3O+,concentration of 0.0013 M KOH(aq) at 25 °C? (Kw = 1.01 × 10-14)

What is the OH- concentration of an aqueous solution with a pH of 9.83? (Kw = 1.01 × 10-14)

A solution has a hydroxide ion concentration of 0.0040 M. Calculate the pOH of the solution at 25 °C. (Kw = 1.01 × 10-14)

Which of the following equations shows that isoquinoline, C9H7N, behaves as a Brønsted-Lowry base in water?

Which equation depicts the hydrogen phosphate ion behaving as a Brønsted-Lowry base in water?

Which of the following is the correct hydroxide ion concentration in 0.48 M CH3CO2-(aq)? (Kb of CH3CO2- = 5.6 × 10-10)

Carbonic acid is a diprotic acid, H2CO3, with Ka1 = 4.2 × 10-7 and Ka2 = 4.8 × 10-11 at 25°C. The ion product for water is Kw = 1.0 × 10-14 at 25°C. What is the OH- concentration of a solution that is 0.39 M in Na2CO3?

What is the H3O+ concentration in 0.0055 M Ba(OH)2(aq) at 25 °C? (Kw = 1.01 × 10-14)?

Which of the following expressions is not equivalent to the formula of pH?

What is Ka at 25°C for the following equilibrium given Kb (CH3NH2) = 4.4 × 10-4 at 25°C.? CH3NH3+(aq) + H2O(l) ⇌\rightleftharpoons⇌ CH3NH2(aq) + H3O+(aq)

When a Lewis acid and a Lewis base combine, the product may be referred to as an acid-base ________.

At 50°C the autoionization constant for pure water, Kw, is 5.48×10−145.48 \times 10 ^ { - 14 }5.48×10−14 . What is the H3O+ concentration in pure water at 50°C?

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

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

Consider the K_a values for the following acids: Cyanic acid, HOCN, 3.5 × 10^-4Formic acid, HCHO₂, 1.7 × 10^-4Lactic acid, HC₃H₅O₃, 1.3 × 10^-4Propionic acid, HC₃H₅O₂, 1.3 × 10^-5 Benzoic acid, HC₇H₅O₂, 6.3 × 10^-5 Which of the following is the strongest acid?

Hydrofluoric acid has a pK_a value of 3.14. What is the value of pK_b for fluoride ion?

Which of the following statements about the reaction below is correct? HCO₃^-(aq) + H₂O( $\ell$ ) $\rightleftharpoons$ CO₃^2-(aq) + H₃O⁺(aq)

H₃PO₃ is a diprotic weak acid. What is the balanced equilibrium defined as K_b2 of H₃PO₃?

What is the hydroxide-ion concentration in a solution formed by combining 200. mL of 0.15 M HCl with 300. mL of 0.090 M NaOH at 25°C? HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)

Which of the following is the correct hydronium ion ,H₃O⁺,concentration of 0.0013 M KOH(aq) at 25 °C? (K_w = 1.01 × 10^-14)

What is the OH^- concentration of an aqueous solution with a pH of 9.83? (K_w = 1.01 × 10^-14)

A solution has a hydroxide ion concentration of 0.0040 M. Calculate the pOH of the solution at 25 °C. (K_w = 1.01 × 10^-14)

Which of the following equations shows that isoquinoline, C₉H₇N, behaves as a Brønsted-Lowry base in water?

Which of the following is the correct hydroxide ion concentration in 0.48 M CH₃CO₂^-(aq)? (K_b of CH₃CO₂^- = 5.6 × 10^-10)

Carbonic acid is a diprotic acid, H₂CO₃, with K_a1 = 4.2 × 10^-7 and K_a2 = 4.8 × 10^-11 at 25°C. The ion product for water is K_w = 1.0 × 10^-14 at 25°C. What is the OH^- concentration of a solution that is 0.39 M in Na₂CO₃?

What is the H₃O⁺ concentration in 0.0055 M Ba(OH)₂(aq) at 25 °C? (K_w = 1.01 × 10^-14)?

What is K_a at 25°C for the following equilibrium given K_b (CH₃NH₂) = 4.4 × 10^-4 at 25°C.? CH₃NH₃⁺(aq) + H₂O(l) $\rightleftharpoons$ CH₃NH₂(aq) + H₃O⁺(aq)

At 50°C the autoionization constant for pure water, K_w, is $5.48 \times 10 ^ { - 14 }$ . What is the H₃O⁺ concentration in pure water at 50°C?