Question 1

Which of the following statements is true for a 1.0 M solution of the strong acid HCl in water?

Accepted Answer

A)  [Cl - ] > [H3O+] 
B)  The pH is 1.00 
C)  [H3O+] = 1.0 M 
D)  [HCl] = 1.0 M 
E)  [H3O+] = [OH - ] 
A)  [Cl - ] > [H3O+] 
B)  The pH is 1.00 
C)  [H3O+] = 1.0 M 
D)  [HCl] = 1.0 M 
E)  [H3O+] = [OH - ]

Question 2

Rank the following 0.100 M solutions in order of increasing pH (from lowest pH to the highest).
HNO3, KI, HIO3, HIO4

Accepted Answer

A)  HNO3 3 4 
B)  HNO3 3 4 3 4 3 3 3 4 
E)  none of these 
A)  HNO3 3 4 
B)  HNO3 3 4 3 4 3 3 3 4 
E)  none of these

Question 3

Which of the following solutions would have the lowest pH?

(HCO2H: Ka = 1.8 x 10-4; NH4+: Ka = 5.6 x 10-10)

Accepted Answer

A)  0.10 M HCO2H 
B)  0.10 M NaHCO2 
C)  0.10 M NH4+ 
D)  a solution that is 0.10 M in both HCO2H and NaHCO2 
E)  a solution that is 0.10 M in both NH4+ and NH3 
A)  0.10 M HCO2H 
B)  0.10 M NaHCO2 
C)  0.10 M NH4+ 
D)  a solution that is 0.10 M in both HCO2H and NaHCO2 
E)  a solution that is 0.10 M in both NH4+ and NH3

Question 4

Which of the following solutions will show the largest change in pH when
10 mL of 1 M NaOH is added to it?

Accepted Answer

A)  10 mL of 1 M NaOH 
B)  100 mL of water 
C)  10 mL of 1 M NaNO3 
D)  10 mL of 0.01 M HOAc 
E)  100 mL of 0.1 M HOAc and 0.1 M NaOAc 
A)  10 mL of 1 M NaOH 
B)  100 mL of water 
C)  10 mL of 1 M NaNO3 
D)  10 mL of 0.01 M HOAc 
E)  100 mL of 0.1 M HOAc and 0.1 M NaOAc

Question 5

Which compound cannot act as a Brønsted base?

Accepted Answer

A)  NH3 
B)  H2O 
C)  CH4 
D)   F- 
E)  H2S 
A)  NH3 
B)  H2O 
C)  CH4 
D)   F- 
E)  H2S

Question 6

Sodium fluoride, NaF (a soluble salt), is dissolved in water. Which one of the following correctly describes the relationships between the concentrations of the species present at equilibrium?

Accepted Answer

A)  [ F- ] +]     [ F- ] 
B)  [F - ]     [Na+] and [H3O+]     [F - ] 
C)  [ F - ]    0 [HF] and [Na+] - ] 
D)  [OH - ] +]    [ F - ] 
E)  none of these 
A)  [ F- ] +]     [ F- ] 
B)  [F - ]     [Na+] and [H3O+]     [F - ] 
C)  [ F - ]    0 [HF] and [Na+] - ] 
D)  [OH - ] +]    [ F - ] 
E)  none of these

Question 7

What is the value of Kb for the formate (HCO2-) ion if Ka for formic acid (HCO2H) is 1.8x10-4?

Accepted Answer

A)  Kb = Kw x Ka 
B)  Kb = Ka/Kw 
C)  Kb = Kw/Ka 
D)  Kb = Kw + Ka 
E)  Kb = Kw - Ka 
A)  Kb = Kw x Ka 
B)  Kb = Ka/Kw 
C)  Kb = Kw/Ka 
D)  Kb = Kw + Ka 
E)  Kb = Kw - Ka

Question 8

Kb for methylamine (CH3NH2) is the equilibrium constant for which reaction?

Accepted Answer

A)  CH3NH2 + H2O   CH3NH- + H3O+ 
B)  CH3NH2 + H2O   CH3NH3+ + OH- 
C)  CH3NH2 + H3O+   CH3NH3+ + H2O 
D)  CH3NH2 + OH-    CH3NH- + H2O 
E)  None of the above 
A)  CH3NH2 + H2O   CH3NH- + H3O+ 
B)  CH3NH2 + H2O   CH3NH3+ + OH- 
C)  CH3NH2 + H3O+   CH3NH3+ + H2O 
D)  CH3NH2 + OH-    CH3NH- + H2O 
E)  None of the above

Question 9

Of the following, which is the strongest acid (lone pairs omitted for clarity)?

Accepted Answer

A)   
B)     
C)     
D)   
A)   
B)     
C)     
D)

Question 10

Which of the following compounds would give a 0.10 M solution with a pH less than 7?

Accepted Answer

A)  Na2S 
B)  K2CO3 
C)  KCN 
D)  NH4Cl 
E)  Na3PO4 
A)  Na2S 
B)  K2CO3 
C)  KCN 
D)  NH4Cl 
E)  Na3PO4

Question 11

Which of the following structural factors is primarily responsible for H2Se being a stronger acid than H2S?

Accepted Answer

A)  bond polarity 
B)  size of the anion 
C)  electron withdrawing effect of oxygen 
D)  electric charge on the acid 
E)  sulfur has d electrons 
A)  bond polarity 
B)  size of the anion 
C)  electron withdrawing effect of oxygen 
D)  electric charge on the acid 
E)  sulfur has d electrons

Question 12

What is the pOH of a 0.025M solution of hydrobromic acid (Ka = 1 x 109)?

Accepted Answer

A)  0.025 
B)  1.60 
C)  12.40 
D)  9.00 
E)  5.00 
A)  0.025 
B)  1.60 
C)  12.40 
D)  9.00 
E)  5.00

Question 13

Which of the following isn't an acid-base reaction?

Accepted Answer

A)  2 HgCl2(s) + 2 CH3Li(l)   Hg(CH3)2(l) + 2 LiCl2(s) 
B)  2 NaCl(s) + H2SO4(aq)   Na2SO4(aq) + 2 HCl(g) 
C)  Na2CO3(aq) + H2SO4(aq)   Na2SO4(aq) + 2 H2O(l) + CO2(g) 
D)  H2C2O4(aq) + 2 NaOH(aq)   Na2C2O4(aq) + 2 H2O(l) 
E)  All of the above are acid-base reactions. 
A)  2 HgCl2(s) + 2 CH3Li(l)   Hg(CH3)2(l) + 2 LiCl2(s) 
B)  2 NaCl(s) + H2SO4(aq)   Na2SO4(aq) + 2 HCl(g) 
C)  Na2CO3(aq) + H2SO4(aq)   Na2SO4(aq) + 2 H2O(l) + CO2(g) 
D)  H2C2O4(aq) + 2 NaOH(aq)   Na2C2O4(aq) + 2 H2O(l) 
E)  All of the above are acid-base reactions.

Question 14

There are many ways of "fluoridating" water. One approach involves adding a salt of the fluoride ion, such as NaF. Calculate the pH of a 0.15 M NaF solution. (HF: Ka = 7.2 x 10-4)

Accepted Answer

A)  2 
B)  5.8 
C)  8.2 
D)  10.9 
E)  12 
A)  2 
B)  5.8 
C)  8.2 
D)  10.9 
E)  12

Question 15

The compound HB can be represented as  where  represent B- and  represents H+. Given this, ___ would represent the conjugate acid of HB and ____ would represent the conjugate base.

Accepted Answer

A)  1,2 
B)  1,5 
C)  3,4 
D)  1,3 
E)  None of the above. 
A)  1,2 
B)  1,5 
C)  3,4 
D)  1,3 
E)  None of the above.

Question 16

Which of the following statements is true?

Accepted Answer

A)  H2O is a stronger acid than HF(aq). 
B)  H2O is a stronger acid than H2S(aq). 
C)  H2O is a stronger acid than the H3O+(aq) ion. 
D)  H2O is a stronger acid than NH3(aq). 
E)  None of the above are true. 
A)  H2O is a stronger acid than HF(aq). 
B)  H2O is a stronger acid than H2S(aq). 
C)  H2O is a stronger acid than the H3O+(aq) ion. 
D)  H2O is a stronger acid than NH3(aq). 
E)  None of the above are true.

Question 17

Rank the following in order of increasing pH of 0.1M solutions. 
NaI, HI, HIO3, NaIO3

Accepted Answer

HI < HIO₃ <

Question 18

Which of the following is the weakest acid?

Accepted Answer

A)  HClO4 
B)  HCl 
C)  HF 
D)  HI 
E)  HBr 
A)  HClO4 
B)  HCl 
C)  HF 
D)  HI 
E)  HBr

Question 19

Predict the products of the following acid-base reaction.
HOCl(aq) + CH3NH2(aq)

Accepted Answer

Question 20

Using a table of Ka's, determine which of the following is the strongest Brønsted acid.

Accepted Answer

A)  NH4+ 
B)  HCl 
C)  HNO3 
D)  HSO4- 
E)  HClO4 
A)  NH4+ 
B)  HCl 
C)  HNO3 
D)  HSO4- 
E)  HClO4

Which of the following statements is true for a 1.0 M solution of the strong acid HCl in water?

Rank the following 0.100 M solutions in order of increasing pH (from lowest pH to the highest). HNO₃, KI, HIO₃, HIO₄

Which of the following solutions would have the lowest pH? (HCO₂H: K_a = 1.8 x 10^-4; NH₄⁺: K_a = 5.6 x 10^-10)

Which of the following solutions will show the largest change in pH when 10 mL of 1 M NaOH is added to it?

Which compound cannot act as a Brønsted base?

Sodium fluoride, NaF (a soluble salt), is dissolved in water. Which one of the following correctly describes the relationships between the concentrations of the species present at equilibrium?

What is the value of K_b for the formate (HCO₂^-) ion if K_a for formic acid (HCO₂H) is 1.8x10^-4?

K_b for methylamine (CH₃NH₂) is the equilibrium constant for which reaction?

Of the following, which is the strongest acid (lone pairs omitted for clarity)?

Which of the following compounds would give a 0.10 M solution with a pH less than 7?

Which of the following structural factors is primarily responsible for H₂Se being a stronger acid than H₂S?

What is the pOH of a 0.025M solution of hydrobromic acid (K_a = 1 x 10⁹)?

Which of the following isn't an acid-base reaction?

There are many ways of "fluoridating" water. One approach involves adding a salt of the fluoride ion, such as NaF. Calculate the pH of a 0.15 M NaF solution. (HF: K_a = 7.2 x 10^-4)

The compound HB can be represented as where represent B^- and represents H⁺. Given this, _ would represent the conjugate acid of HB and __ would represent the conjugate base.

Which of the following statements is true?

Rank the following in order of increasing pH of 0.1M solutions. NaI, HI, HIO₃, NaIO₃

Which of the following is the weakest acid?

Predict the products of the following acid-base reaction. HOCl(aq) + CH₃NH₂(aq)

Using a table of K_a's, determine which of the following is the strongest Brønsted acid.

Elements Compounds

The Mole

Structure of the Atom

The Covalent Bond

Ionic and Metallic Bonds

Gases

Making and Breaking of Bonds

Liquids and Solutions

Solids

An Introduction to Kinetics and Equilibrium

Oxidation-Reduction Reactions

Chemical Thermodynamics

Kinetics

Nuclear Chemistry

Organic Chemistry

Filters

Exam 11: Acids and Bases

Which of the following statements is true for a 1.0 M solution of the strong acid HCl in water?

Rank the following 0.100 M solutions in order of increasing pH (from lowest pH to the highest). HNO3, KI, HIO3, HIO4

Which of the following solutions would have the lowest pH? (HCO2H: Ka = 1.8 x 10-4; NH4+: Ka = 5.6 x 10-10)

Which of the following solutions will show the largest change in pH when 10 mL of 1 M NaOH is added to it?

Which compound cannot act as a Brønsted base?

Sodium fluoride, NaF (a soluble salt), is dissolved in water. Which one of the following correctly describes the relationships between the concentrations of the species present at equilibrium?

What is the value of Kb for the formate (HCO2-) ion if Ka for formic acid (HCO2H) is 1.8x10-4?

Kb for methylamine (CH3NH2) is the equilibrium constant for which reaction?

Of the following, which is the strongest acid (lone pairs omitted for clarity)?

Which of the following compounds would give a 0.10 M solution with a pH less than 7?

Which of the following structural factors is primarily responsible for H2Se being a stronger acid than H2S?

What is the pOH of a 0.025M solution of hydrobromic acid (Ka = 1 x 109)?

Which of the following isn't an acid-base reaction?

There are many ways of "fluoridating" water. One approach involves adding a salt of the fluoride ion, such as NaF. Calculate the pH of a 0.15 M NaF solution. (HF: Ka = 7.2 x 10-4)

The compound HB can be represented as where represent B- and represents H+. Given this, ___ would represent the conjugate acid of HB and ____ would represent the conjugate base.

Which of the following statements is true?

Rank the following in order of increasing pH of 0.1M solutions. NaI, HI, HIO3, NaIO3

Which of the following is the weakest acid?

Predict the products of the following acid-base reaction. HOCl(aq) + CH3NH2(aq)

Using a table of Ka's, determine which of the following is the strongest Brønsted acid.

Elements Compounds

The Mole

Structure of the Atom

The Covalent Bond

Ionic and Metallic Bonds

Gases

Making and Breaking of Bonds

Liquids and Solutions

Solids

An Introduction to Kinetics and Equilibrium

Oxidation-Reduction Reactions

Chemical Thermodynamics

Kinetics

Nuclear Chemistry

Organic Chemistry

Filters

Rank the following 0.100 M solutions in order of increasing pH (from lowest pH to the highest). HNO₃, KI, HIO₃, HIO₄

Which of the following solutions would have the lowest pH? (HCO₂H: K_a = 1.8 x 10^-4; NH₄⁺: K_a = 5.6 x 10^-10)

What is the value of K_b for the formate (HCO₂^-) ion if K_a for formic acid (HCO₂H) is 1.8x10^-4?

K_b for methylamine (CH₃NH₂) is the equilibrium constant for which reaction?

Which of the following structural factors is primarily responsible for H₂Se being a stronger acid than H₂S?

What is the pOH of a 0.025M solution of hydrobromic acid (K_a = 1 x 10⁹)?

There are many ways of "fluoridating" water. One approach involves adding a salt of the fluoride ion, such as NaF. Calculate the pH of a 0.15 M NaF solution. (HF: K_a = 7.2 x 10^-4)

The compound HB can be represented as where represent B^- and represents H⁺. Given this, _ would represent the conjugate acid of HB and __ would represent the conjugate base.

Rank the following in order of increasing pH of 0.1M solutions. NaI, HI, HIO₃, NaIO₃

Predict the products of the following acid-base reaction. HOCl(aq) + CH₃NH₂(aq)

Using a table of K_a's, determine which of the following is the strongest Brønsted acid.