Question 1

What is the pH of the final solution when 25 mL of 0.023 M HCl has been added to 35 mL of 0.040 M HCl at 25°C?

Accepted Answer

A)  3.22
B)  1.81
C)  1.48
D)  2.70
E)  3.41F) A) and B)
G) A) and C)

Question 2

A solution has a pH value of 3.66.What is the pOH for this solution?

Accepted Answer

A)  7.00
B)  3.83
C)  3.66
D)  2.19
E)  10.34F) A) and D)
G) A) and C)

Question 3

Which of the following reactions is not product-favored?

Accepted Answer

A)  NaOH(aq) → Na+(aq) + OH-(aq) 
B)  NH3(aq) + H2O(l) → NH4+(aq) + OH-(aq) 
C)  HClO4(aq) + H2O(l) → H3O+(aq) + ClO4-(aq) 
D)  HCl(aq) + H2O(l) → H3O+(aq) + Cl-(aq) 
E)  H2SO4(aq) + H2O(l) → H3O+(aq) + HSO4-(aq) F) B) and D)
G) A) and D)

Question 4

A solution in which the pH is 1.5 would be described as

Accepted Answer

A)  neutral.
B)  very acidic.
C)  slightly basic.
D)  slightly acidic.
E)  very basic.F) A) and B)
G) D) and E)

Question 5

The pOH of a solution is 5.72 .What is its hydronium-ion concentration?

Accepted Answer

A)  5.2 × 105 M
B)  5.2 × 10-9 M
C)  1.9 × 10-6 M
D)  5.72 M
E)  3.3 × 10-3 MF) A) and B)
G) D) and E)

Question 6

Which solution has the highest pH?

Accepted Answer

A)  0.10 M HBr(aq) 
B)  0.10 M HI(aq) 
C)  0.10 M HF(aq) 
D)  0.10 M HCl(aq) 
E)  0.10 M HClO4(aq) F) B) and E)
G) A) and E)

Question 7

What is the pOH of a solution prepared by dissolving 0.591 g of KOH(s) in 7.50 L of water?

Accepted Answer

A)  11.148
B)  2.852
C)  1.977
D)  12.023
E)  7.000F) A) and B)
G) A) and C)

Question 8

Which of the following species is amphiprotic in aqueous solution?

Accepted Answer

A)  CH3NH2
B)  H3O+
C)  NH4+
D)  F−
E)  HSO4-F) None of the above
G) A) and E)

Question 9

What is the pH of a 0.0072 M hydrochloric acid solution?

Accepted Answer

A)  4.93
B)  11.86
C)  7.00
D)  9.07
E)  2.14F) None of the above
G) C) and D)

Question 10

Which of the following statements is incorrect?

Accepted Answer

A)  One reason why HCl is a stronger acid than HF is that the H-Cl bond is weaker than the H-F bond.
B)  F- is a stronger base than Cl-.
C)  One reason why HCl is a stronger acid than HF is that Cl is more electronegative than F.
D)  The acids HBr and HI both appear equally strong in water.
E)  One reason why HCl is a stronger acid than HF is that Cl has a larger atomic radius than F.F) C) and D)
G) All of the above

Question 11

Which of the following pairs of species is not a conjugate acid-base pair?

Accepted Answer

A)  HOCl,OCl-
B)  HNO2,NO2+
C)  O2-,OH-
D)  HSO4-,SO42-
E)  H2CO3,HCO3-F) C) and D)
G) A) and B)

Question 12

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

Accepted Answer

A)  HBr > HClO > HBrO > HIO
B)  HIO > HBrO > HClO > HBr
C)  HBr > HIO > HBrO > HClO
D)  HClO > HBr > HBrO > HIO
E)  HClO > HBrO > HBr > HIOF) A) and B)
G) A) and C)

Question 13

What is the concentration of H3O+ and OH− ion in pure water at 25 °C?​

Accepted Answer

A)  ​1.8 × 10−7 M,3.2 × 10−7 M
B)  ​2.0 × 10−7 M,4.0 × 10−7 M
C)  ​3.0 × 10−7 M,2.0 × 10−7 M
D)  ​2.0 × 10−7 M,1.5 × 10−7 M
E)  ​1.0 × 10−7 M,1.0 × 10−7 MF) All of the above
G) A) and B)

Question 14

Rank the following in order of decreasing acid strength: H2O,H2S,H2Se,H2Te

Accepted Answer

A)  H2Te > H2Se > H2S > H2O
B)  H2O > H2S > H2Se > H2Te
C)  H2Se > H2Te > H2S > H2O
D)  H2S > H2Te > H2Se > H2O
E)  H2Se > H2S > H2Te > H2OF) A) and B)
G) A) and C)

Question 15

Which are the Brønsted-Lowry bases in the following equilibrium?
HCOO-(aq) + H2O(l)  -(aq) + H2O(l)    HCOOH(aq) + OH-(aq)  A) HCOO- and OH- B) H2O and OH- C) H2O,HCOOH,and OH- D) HCOO- and HCOOH E) H2O and HCOOH" class="answers-bank-image d-inline" rel="preload" >
HCOOH(aq) + OH-(aq)

Accepted Answer

A)  HCOO- and OH-
B)  H2O and OH-
C)  H2O,HCOOH,and OH-
D)  HCOO- and HCOOH
E)  H2O and HCOOHF) C) and E)
G) A) and C)

Question 16

What is the equilibrium concentration of amide ion (NH2-) in liquid ammonia at 25°C? ("am" = dissolved in ammonia) 
2NH3(l)  2-) in liquid ammonia at 25°C? ( am  = dissolved in ammonia)  2NH3(l)    NH4+(am) + NH2-(am) ; Kc = 1.8 × 10-24 at 25°C A) 2.6 × 10-12 M B) 3.6 × 10-24 M C) 1.3 × 10-12 M D) 1.8 × 10-24 M E) 9.0 × 10-25 M" class="answers-bank-image d-inline" rel="preload" >
NH4+(am) + NH2-(am) ; Kc = 1.8 × 10-24 at 25°C

Accepted Answer

A)  2.6 × 10-12 M
B)  3.6 × 10-24 M
C)  1.3 × 10-12 M
D)  1.8 × 10-24 M
E)  9.0 × 10-25 MF) A) and B)
G) A) and C)

Question 17

Which of the following is not an example of an acid-base reaction?

Accepted Answer

A)  Al(OH) 3(s) + 3H+(aq) →→ Al3+(aq) + 3H2O(l) 
B)  C2H6(g) → →→→→→C2H4(g) + H2(g) 
C)  MgO(s) + CO2(g) →→ MgCO3(s) 
D)  Al(OH) 3(s) + OH-(aq) →→→→→ Al(OH) 4-(aq) 
E)  CN-(aq) + H2O(l)  3(s) + 3H+(aq) →→ Al3+(aq) + 3H2O(l)  
B)  C2H6(g) → →→→→→C2H4(g) + H2(g)  
C)  MgO(s) + CO2(g) →→ MgCO3(s)  
D)  Al(OH) 3(s) + OH-(aq) →→→→→ Al(OH) 4-(aq)  
E)  CN-(aq) + H2O(l)    HCN(aq) + OH-(aq) " class="answers-bank-image d-inline" rel="preload" > HCN(aq) + OH-(aq) F) A) and E)
G) B) and C)

Question 18

What is the pH of a 0.0052 M CaOH solution?

Accepted Answer

A)  8.74
B)  11.72
C)  2.28
D)  5.26
E)  16.28F) A) and E)
G) B) and C)

Question 19

The equilibrium constant for the autonionization of water (shown below) increases with increasing temperature,from 1.01 x10-14 at 25°C to 5.31 x10-14 at 50°C.
H2O(l) + H2O(l)  -14 at 25°C to 5.31 x10-14 at 50°C. H2O(l) + H2O(l)    H3O+(aq) + OH-(aq)  Which of the following statements is consistent with this behaviour? A) The autoionization of water is an endothermic reaction. B) The autoionization of water is an exothermic reaction. C) The hydronium ion concentration at equilibrium increases with increasing temperature. D) The hydronium ion concentration at equilibrium decreases with increasing temperature. E) Both A and C." class="answers-bank-image d-inline" rel="preload" >
H3O+(aq) + OH-(aq) 
Which of the following statements is consistent with this behaviour?

Accepted Answer

A)  The autoionization of water is an endothermic reaction.
B)  The autoionization of water is an exothermic reaction.
C)  The hydronium ion concentration at equilibrium increases with increasing temperature.
D)  The hydronium ion concentration at equilibrium decreases with increasing temperature.
E)  Both A and C.F) C) and D)
G) B) and D)

Question 20

Which of the following is the strongest acid in aqueous solution?

Accepted Answer

A)  H3AsO4
B)  H3PO4
C)  H3PO3
D)  H3SbO4
E)  H3AsO3F) C) and E)
G) C) and D)

Exam 15: Acids and Bases

What is the pH of the final solution when 25 mL of 0.023 M HCl has been added to 35 mL of 0.040 M HCl at 25°C?

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Which are the Brønsted-Lowry bases in the following equilibrium? HCOO-(aq) + H2O(l) HCOOH(aq) + OH-(aq)

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Which solution has the highest pH?

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The equilibrium constant for the autonionization of water (shown below) increases with increasing temperature,from 1.01 x10-14 at 25°C to 5.31 x10-14 at 50°C. H2O(l) + H2O(l) H3O+(aq) + OH-(aq) Which of the following statements is consistent with this behaviour?

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Rank the following in order of decreasing acid strength: H2O,H2S,H2Se,H2Te

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Which of the following statements is incorrect?

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The pOH of a solution is 5.72 .What is its hydronium-ion concentration?

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What is the pH of a 0.0052 M CaOH solution?

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Which of the following is not an example of an acid-base reaction?

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Which of the following is the strongest acid in aqueous solution?

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What is the pH of a 0.0072 M hydrochloric acid solution?

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Which of the following reactions is not product-favored?

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What is the concentration of H3O+ and OH− ion in pure water at 25 °C?​

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A solution has a pH value of 3.66.What is the pOH for this solution?

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

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What is the pOH of a solution prepared by dissolving 0.591 g of KOH(s) in 7.50 L of water?

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Which of the following pairs of species is not a conjugate acid-base pair?

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What is the equilibrium concentration of amide ion (NH2-) in liquid ammonia at 25°C? ("am" = dissolved in ammonia) 2NH3(l) NH4+(am) + NH2-(am) ; Kc = 1.8 × 10-24 at 25°C

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A solution in which the pH is 1.5 would be described as

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Which of the following species is amphiprotic in aqueous solution?

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Which are the Brønsted-Lowry bases in the following equilibrium? HCOO^-(aq) + H₂O(l) HCOOH(aq) + OH^-(aq)

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The equilibrium constant for the autonionization of water (shown below) increases with increasing temperature,from 1.01 x10^-14 at 25°C to 5.31 x10^-14 at 50°C. H₂O(l) + H₂O(l) H₃O⁺(aq) + OH^-(aq) Which of the following statements is consistent with this behaviour?

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Rank the following in order of decreasing acid strength: H₂O,H₂S,H₂Se,H₂Te

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What is the concentration of H₃O⁺ and OH⁻ ion in pure water at 25 °C?

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What is the equilibrium concentration of amide ion (NH₂^-) in liquid ammonia at 25°C? ("am" = dissolved in ammonia) 2NH₃(l) NH₄⁺(am) + NH₂^-(am) ; K_c = 1.8 × 10^-24 at 25°C

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