Question 1

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

Accepted Answer

A)    5.48×10−145.48 	imes 10 ^ { - 14 }5.48×10−14  M
B)   1.01 × 10-7 M
C)    1.17×10−71.17 	imes 10 ^ { - 7 }1.17×10−7  M
D)    2.34×10−72.34 	imes 10 ^ { - 7 }2.34×10−7  M
E)   1.01 × 10-14 M F) None of the above
G) A) and B)

Question 2

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

Accepted Answer

The answer of When a Lewis acid and a Lewis...

Question 3

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)

Accepted Answer

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 MF) B) and E)
G) A) and D)

Question 4

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

Accepted Answer

A)   1.4 × 10-11
B)   7.2 × 10-4
C)   3.14
D)   10.86
E)   17.14F) None of the above
G) All of the above

Question 5

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

Accepted Answer

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 MF) A) and D)
G) None of the above

Question 6

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

Accepted Answer

A)   1.3 × 10-10 M
B)   6.8 × 10-5 M
C)   6.8 × 10-1 M
D)   1.5 × 10-2 M
E)   7.4 × 109 MF) C) and D)
G) B) and D)

Question 7

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?

Accepted Answer

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

Question 8

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

Accepted Answer

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)  F) A) and E)
G) A) and D)

Question 9

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?

Accepted Answer

A)   9.0 × 10-3 M
B)   2.1 × 10-4 M
C)   9.6 × 10-5 M
D)   4.3 × 10-6 M
E)   4.0 × 10-4 MF) C) and E)
G) A) and E)

Question 10

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

Accepted Answer

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. F) C) and D)
G) A) and E)

Question 11

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)

Accepted Answer

A)   1.7 × 10-13 M
B)   0.090 M
C)   1.7 × 10-12 M
D)   0.054 M
E)   1.0 × 10-7 MF) B) and D)
G) A) and E)

Question 12

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

Accepted Answer

A)   sodium dihydrogen phosphate, NaH2PO4(s) 
B)   sodium acetate, NaCH3CO2(s) 
C)   ammonium nitrate, NH4NO3(s) 
D)   hydrogen bromide, HCl(g) 
E)   sodium bicarbonate, NaHCO3(s) F) A) and C)
G) A) and E)

Question 13

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

Accepted Answer

A)   HPO42-(aq)  + H2O(  ℓ\ellℓ  )   ⇌\rightleftharpoons⇌  H2PO4-(aq)  + OH-(aq) 
B)   HPO42-(aq)  + OH-(aq)   ⇌\rightleftharpoons⇌  PO43-(aq)  + H2O(  ℓ\ellℓ  ) 
C)   HPO42-(aq)  + H2O(  ℓ\ellℓ  )   ⇌\rightleftharpoons⇌  PO43-(aq)  + H3O+(aq) 
D)   2 HPO42-(aq)  + O2-(aq)   ⇌\rightleftharpoons⇌  PO43-(aq)  + H2O(  ℓ\ellℓ  ) 
E)   2 HPO42-(aq)  + H2O(  ℓ\ellℓ  )   ⇌\rightleftharpoons⇌  2 H2O(  ℓ\ellℓ  )  + P2O7(s)  F) B) and E)
G) A) and E)

Question 14

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

Accepted Answer

A)   H3PO3(aq)  + H2O(l)   ⇌\rightleftharpoons⇌  H3O+(aq)  + H2PO3-(aq) 
B)   H2PO3-(aq)  + H2O(l)   ⇌\rightleftharpoons⇌  H3O+(aq)  + HPO32-(aq) 
C)   HPO32-(aq)  + H2O(l)   ⇌\rightleftharpoons⇌  OH-(l)  + H2PO3-(aq) 
D)   H2PO3-(aq)  + H2O(l)   ⇌\rightleftharpoons⇌  OH-(l)  + H3PO3(aq) 
E)   HPO32-(aq)  + H2O(l)   ⇌\rightleftharpoons⇌  OH-(aq)  + H3PO3(aq)  F) B) and C)
G) All of the above

Question 15

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, Ka, for HCO2H is 1.8 × 10-4 and the acid dissociation constant for HCN is 4.0 × 10-10.

Accepted Answer

A)   K = 1.00. The reaction favors neither the formation of reactants nor products.
B)   K = 2.2 × 10-6. The reaction favors the formation of products.
C)   K = 2.2 × 10-6. The reaction favors the formation of reactants.
D)   K = 4.5 × 105. The reaction favors the formation of products.
E)   K = 4.5 × 105. The reaction favors the formation of reactants. F) A) and D)
G) A) and B)

Question 16

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.

Accepted Answer

The answer of When a Lewis acid combines with a...

Question 17

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

Accepted Answer

A)   2.7 × 10-10 M
B)   6.2 × 10-10 M
C)   1.1 × 10-5 M
D)   1.6 × 10-5 M
E)   2.4 × 10-5 MF) B) and D)
G) A) and B)

Question 18

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)

Accepted Answer

A)   11.60
B)   2.40
C)   7.00
D)   8.48
E)   5.52F) All of the above
G) C) and D)

Question 19

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)

Accepted Answer

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

Question 20

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

Accepted Answer

A)   -log [H+(aq) ]
B)    log⁡1[H+(aq) ]\log \frac { 1 } { \left[ H ^ { + } ( a q )  \right] }log[H+(aq) ]1​ 
C)   14.0 - pOH
D)    −log⁡Kw[OH−]- \log \frac { K _ { w } } { \left[ \mathrm { OH } ^ { - } \right] }−log[OH−]Kw​​ 
E)   -log Kw F) A) and B)
G) B) and C)

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

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.

Correct Answer
verified

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

Correct Answer
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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)

Correct Answer
verified

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

Correct Answer
verified

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?

Correct Answer
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Correct Answer
verified

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?

Correct Answer
verified

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

Correct Answer
verified

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?

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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)

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

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)

Correct Answer
verified

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)

Correct Answer
verified

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

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.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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)

Correct AnswerverifiedShow Answer

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)

Correct AnswerverifiedShow Answer

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

Correct Answer
verified

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)

Correct Answer
verified

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

Correct Answer
verified

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?

Correct Answer
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Correct Answer
verified

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?

Correct Answer
verified

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

Correct Answer
verified

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?

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

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

Correct Answer
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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)

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

Correct Answer
verified

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

Correct Answer
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Correct Answer
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Correct Answer
verified

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)

Correct Answer
verified

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)

Correct Answer
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