Question 1

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) 10.34 
A) 7.00 
B) 3.83 
C) 3.66 
D) 2.19 
E) 10.34

Question 2

Which of the following species is amphiprotic in aqueous solution?

Accepted Answer

A) CH3NH2 
B) H3O+ 
C) NH4+ 
D) F− 
E) HSO4- 
A) CH3NH2 
B) H3O+ 
C) NH4+ 
D) F− 
E) HSO4-

Question 3

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) 7.000 
A) 11.148 
B) 2.852 
C) 1.977 
D) 12.023 
E) 7.000

Question 4

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 M 
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 M

Question 5

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 > H2O 
A) H2Te > H2Se > H2S > H2O 
B) H2O > H2S > H2Se > H2Te 
C) H2Se > H2Te > H2S > H2O 
D) H2S > H2Te > H2Se > H2O 
E) H2Se > H2S > H2Te > H2O

Question 6

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 > HIO 
A) HBr > HClO > HBrO > HIO 
B) HIO > HBrO > HClO > HBr 
C) HBr > HIO > HBrO > HClO 
D) HClO > HBr > HBrO > HIO 
E) HClO > HBrO > HBr > HIO

Question 7

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) 
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)

Question 8

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) 16.28 
A) 8.74 
B) 11.72 
C) 2.28 
D) 5.26 
E) 16.28

Question 9

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) 
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)

Question 10

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

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 M 
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

Question 11

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

Accepted Answer

A) H3AsO4 
B) H3PO4 
C) H3PO3 
D) H3SbO4 
E) H3AsO3 
A) H3AsO4 
B) H3PO4 
C) H3PO3 
D) H3SbO4 
E) H3AsO3

Question 12

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) 2.14 
A) 4.93 
B) 11.86 
C) 7.00 
D) 9.07 
E) 2.14

Question 13

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?

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. 
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.

Question 14

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)   HCN(aq)+ OH-(aq) 
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)   HCN(aq)+ OH-(aq)

Question 15

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

Question 16

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

Question 17

Which are the Brønsted-Lowry bases in the following equilibrium?
HCOO-(aq)+ H2O(l)  
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 HCOOH 
A) HCOO- and OH- 
B) H2O and OH- 
C) H2O,HCOOH,and OH- 
D) HCOO- and HCOOH 
E) H2O and HCOOH

Question 18

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) 3.41 
A) 3.22 
B) 1.81 
C) 1.48 
D) 2.70 
E) 3.41

Question 19

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 M 
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 M

Question 20

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. 
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.

Exam 15: Acids and Bases

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

Which of the following species is amphiprotic in aqueous solution?

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

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

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

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

Which of the following reactions is not product-favored?

What is the pH of a 0.0052 M CaOH solution?

Which solution has the highest pH?

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

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

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

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?

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

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

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

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

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?

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

Which of the following statements is incorrect?

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Thermochemistry

Quantum Theory of the Atom

Electron Configurations and Periodicity

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Filters

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

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

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?

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

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