Question 1

Which of the following solutions would have a pH greater than 7.0?

Accepted Answer

A)  NH4Cl 
B)  NaCl 
C)  CH3COOH 
D)  CH3COONa 
E)  HCl 
A)  NH4Cl 
B)  NaCl 
C)  CH3COOH 
D)  CH3COONa 
E)  HCl

Question 2

The hydride ion, (H-), is a stronger base than the hydroxide ion, (OH-). The products of the reaction between H- (aq) and H2O(l) would be.

Accepted Answer

A)  H2O(aq) 
B)  OH- (aq) + H2(g) 
C)  OH- (aq) + 2H+(aq) 
D)  H2O2(aq) 
E)  No reaction would occur. 
A)  H2O(aq) 
B)  OH- (aq) + H2(g) 
C)  OH- (aq) + 2H+(aq) 
D)  H2O2(aq) 
E)  No reaction would occur.

Question 3

Consider the following reaction:
H2PO4-(aq) + HCO3-(aq)   H2CO3(aq) + HPO42-(aq)
Brønsted would identify the acidic species as:

Accepted Answer

A)  H2PO4- and H2CO3 
B)  H2PO4- and HPO42- 
C)  HCO3- and H2CO3  
D)  HCO3- and HPO42- 
E)  H2CO3 and HPO42- 
A)  H2PO4- and H2CO3 
B)  H2PO4- and HPO42- 
C)  HCO3- and H2CO3  
D)  HCO3- and HPO42- 
E)  H2CO3 and HPO42-

Question 4

What would happen if more formic acid (HCO2H) was added to the following solution at equilibrium?
HCO2H(aq) + H2O(l)   H3O+(aq) + HCO2-(aq)

Accepted Answer

A)  [H2O] should increase. 
B)  [H3O+] and [HCO2-] should both increase. 
C)  [H3O+] and [HCO2-] should both decrease. 
D)  [H3O+] should increase but [HCO2-] should decrease. 
E)  [H3O+] should decrease but [HCO2-] should increase. 
A)  [H2O] should increase. 
B)  [H3O+] and [HCO2-] should both increase. 
C)  [H3O+] and [HCO2-] should both decrease. 
D)  [H3O+] should increase but [HCO2-] should decrease. 
E)  [H3O+] should decrease but [HCO2-] should increase.

Question 5

Which of the following groups contains salts that all form basic solutions in water?

Accepted Answer

A)  NaNO3, NH4CN, NaOAc, NH4Cl 
B)  Na2CO3, KCl, NaOAc, NH4Cl 
C)  Na2CO3, NaF, NaOAc, NaCN 
D)  NaHCO3, NaF, NH4Cl, Na2SO3 
E)  none of the above 
A)  NaNO3, NH4CN, NaOAc, NH4Cl 
B)  Na2CO3, KCl, NaOAc, NH4Cl 
C)  Na2CO3, NaF, NaOAc, NaCN 
D)  NaHCO3, NaF, NH4Cl, Na2SO3 
E)  none of the above

Question 6

A solution of weak base is added to a beaker of water. Which of the following will be true as the base is added to the water?

Accepted Answer

A)  [H3O+] increases [OH - ] decreases pH increases 
B)  [H3O+] decreases [OH -F ] increases pH decreases 
C)  [H3O+] decreases [OH - ] decreases pH increases 
D)  [H3O+] remains constant [OH - ] increases pH increases 
E)  none of these 
A)  [H3O+] increases [OH - ] decreases pH increases 
B)  [H3O+] decreases [OH -F ] increases pH decreases 
C)  [H3O+] decreases [OH - ] decreases pH increases 
D)  [H3O+] remains constant [OH - ] increases pH increases 
E)  none of these

Question 7

Which of the following is correct (assume all solutions have the same concentration)?

Accepted Answer

A)  A solution of K2SO3 is more basic than a solution of KHSO3. 
B)  A solution of K2CO3 is less basic than a solution of KHCO3. 
C)  A solution of NaHSO3 is more acidic than a solution of NaHSO4. 
D)  A solution of Na2HPO4 is less basic than a solution of NaH2PO4. 
E)  All of these are correct. 
A)  A solution of K2SO3 is more basic than a solution of KHSO3. 
B)  A solution of K2CO3 is less basic than a solution of KHCO3. 
C)  A solution of NaHSO3 is more acidic than a solution of NaHSO4. 
D)  A solution of Na2HPO4 is less basic than a solution of NaH2PO4. 
E)  All of these are correct.

Question 8

Use the following information to answer 
HS1U1B12S1U1B0Se: KS1U1B1a1S1U1B0 = 1.0 x 10S1U1P1-4S1S1P0, KS1U1B1a2S1U1B0 = 1.0 x 10S1U1P1-10S1S1P0
-The base-ionization constant for the Se2- ion would be:

Accepted Answer

A)  Kb1 = Ka1 = 1.7 x 10-4 
B)  Kb1 = Ka2 = 1.0 x 10-10 
C)  Kb1 = Kw/Ka1 = 5.9 x 10-11 
D)  Kb1 = Kw/Ka2 = 1.0 x 10-4 
E)  none of the above 
A)  Kb1 = Ka1 = 1.7 x 10-4 
B)  Kb1 = Ka2 = 1.0 x 10-10 
C)  Kb1 = Kw/Ka1 = 5.9 x 10-11 
D)  Kb1 = Kw/Ka2 = 1.0 x 10-4 
E)  none of the above

Question 9

What reaction would take place to limit the change in pH when NaOH is added to a mixture of acetic acid (CH3CO2H) and acetate ion (CH3CO2-)?

Accepted Answer

A)  H3O+(aq) + CH3CO2-(aq)  $\rightarrow$  CH3CO2H(aq) + H2O(l) 
B)  OH-(aq) + CH3CO2H(aq) $\rightarrow$  CH3CO2-(aq) + H2O(l) 
C)  H2O(l) + CH3CO2-(aq)  $\rightarrow$ CH3CO2H(aq) + OH-(aq) 
D)  H2O(l) + CH3CO2H(aq) $\rightarrow$ CH3CO2-(aq) + H3O+(aq) 
E)  none of the above 
A)  H3O+(aq) + CH3CO2-(aq)  $\rightarrow$  CH3CO2H(aq) + H2O(l) 
B)  OH-(aq) + CH3CO2H(aq) $\rightarrow$  CH3CO2-(aq) + H2O(l) 
C)  H2O(l) + CH3CO2-(aq)  $\rightarrow$ CH3CO2H(aq) + OH-(aq) 
D)  H2O(l) + CH3CO2H(aq) $\rightarrow$ CH3CO2-(aq) + H3O+(aq) 
E)  none of the above

Question 10

Which of the following isn't a Brønsted base?

Accepted Answer

A)  PF5 
B)  H2O 
C)  NH3 
D)  S2- 
E)  CN- 
A)  PF5 
B)  H2O 
C)  NH3 
D)  S2- 
E)  CN-

Question 11

The addition of sodium formate (HCO2Na) to a solution containing formic acid (HCO2H: Ka = 1.8 x 10-4) will cause

Accepted Answer

A)  the pH to increase. 
B)  the pH to decrease. 
C)  no change in pH. 
D)  a change in the pH, the direction of which cannot be predicted. 
A)  the pH to increase. 
B)  the pH to decrease. 
C)  no change in pH. 
D)  a change in the pH, the direction of which cannot be predicted.

Question 12

Calculate the pH of a solution prepared by dissolving 1.00 x 10-2 moles of sodium hypochlorite (NaOCl) in enough water to produce a 1.00 L of solution. Hypochlorous acid is a weak monoprotic acid with Ka = 3.2 x 10-8.

Accepted Answer

A)  4.3 
B)  4.7 
C)  7.5 
D)  9.3 
E)  9.7 
A)  4.3 
B)  4.7 
C)  7.5 
D)  9.3 
E)  9.7

Question 13

What is the conjugate base of HSO4-?

Accepted Answer

A)  H2O 
B)  H2SO4 
C)  HSO4- 
D)  SO3 
E)  none of the above 
A)  H2O 
B)  H2SO4 
C)  HSO4- 
D)  SO3 
E)  none of the above

Question 14

Calculate the pH of a buffer prepared by mixing 0.10 mol of sodium formate and 0.05 mol of formic acid in 1.0 L of solution. (HCO2H: Ka = 1.8 x 10-4)

Accepted Answer

A)  1.8 x 10-4 
B)  3.44 
C)  4.05 
D)  5.31 
E)  none of the above 
A)  1.8 x 10-4 
B)  3.44 
C)  4.05 
D)  5.31 
E)  none of the above

Question 15

At what point in the following titration curve would the pH of the solution be equal to the pKa of the acid?

Accepted Answer

A)  0 mL 
B)  50 mL 
C)  95 mL 
D)  100 mL 
E)  120 mL 
A)  0 mL 
B)  50 mL 
C)  95 mL 
D)  100 mL 
E)  120 mL

Question 16

Calculate the approximate pH of a 0.100 M solution of formic acid (HCO2H) in water. (HCO2H: Ka = 1.8 x 10-4)

Accepted Answer

A)  2.4 
B)  3.7 
C)  4.7 
D)  7 
E)  11.6 
A)  2.4 
B)  3.7 
C)  4.7 
D)  7 
E)  11.6

Question 17

Which of the following equations is valid for a 0.10 M solution of formic acid, HCO2H?
HCO2H(aq) + H2O(l)   HCO2-(aq) + H3O+(aq) &emsp; Ka = 1.8 x 10-4

Accepted Answer

A)  [H3O+] -] 
B)  [H3O+] = [HCO2H] 
C)  [H3O+] = [HCO2-] 
D)  [H3O+] = [H2O] 
E)  [OH-] = [H2O] 
A)  [H3O+] -] 
B)  [H3O+] = [HCO2H] 
C)  [H3O+] = [HCO2-] 
D)  [H3O+] = [H2O] 
E)  [OH-] = [H2O]

Question 18

What is the H3O+ ion concentration in a 0.10 M NH3 solution?
(Kb = 1.8 x 10-5)

Accepted Answer

A)  7.5 x 10-10 
B)  3.0 x 10-10 
C)  1.8 x 10-6 
D)  1.3 x 10-3 
E)  none of these 
A)  7.5 x 10-10 
B)  3.0 x 10-10 
C)  1.8 x 10-6 
D)  1.3 x 10-3 
E)  none of these

Question 19

Ammonia and the ammonium ion form a conjugate acid-base pair.
NH3(aq) + H2O(l)   NH4+(aq) + OH-(aq)
Calculate the pH of 0.10 M NH3 if Ka for the NH4+ ion is 5.6 x 10-10.

Accepted Answer

A)  4.7 
B)  5.1 
C)  5.7 
D)  8.9 
E)  11.1 
A)  4.7 
B)  5.1 
C)  5.7 
D)  8.9 
E)  11.1

Question 20

Use the following acid-dissociation equilibrium constants for 
  
-A solution is prepared with initial concentrations of HA and NaA of 0.50 M and 1.00 M respectively. What is the pH of the solution?

Accepted Answer

A)  3.70 
B)  4.00 
C)  4.30 
D)  9.70 
E)  10.30 
A)  3.70 
B)  4.00 
C)  4.30 
D)  9.70 
E)  10.30

Which of the following solutions would have a pH greater than 7.0?

The hydride ion, (H^-), is a stronger base than the hydroxide ion, (OH^-). The products of the reaction between H^- (aq) and H₂O(l) would be.

Consider the following reaction: H₂PO₄^-(aq) + HCO₃^-(aq) H₂CO₃(aq) + HPO₄^2-(aq) Brønsted would identify the acidic species as:

What would happen if more formic acid (HCO₂H) was added to the following solution at equilibrium? HCO₂H(aq) + H₂O(l) H₃O⁺(aq) + HCO₂^-(aq)

Which of the following groups contains salts that all form basic solutions in water?

A solution of weak base is added to a beaker of water. Which of the following will be true as the base is added to the water?

Which of the following is correct (assume all solutions have the same concentration)?

Use the following information to answer H₂Se: K_a1 = 1.0 x 10^-4, K_a2 = 1.0 x 10^-10 -The base-ionization constant for the Se^2- ion would be:

What reaction would take place to limit the change in pH when NaOH is added to a mixture of acetic acid (CH₃CO₂H) and acetate ion (CH₃CO₂^-)?

Which of the following isn't a Brønsted base?

The addition of sodium formate (HCO₂Na) to a solution containing formic acid (HCO₂H: K_a = 1.8 x 10^-4) will cause

Calculate the pH of a solution prepared by dissolving 1.00 x 10^-2moles of sodium hypochlorite (NaOCl) in enough water to produce a 1.00 L of solution. Hypochlorous acid is a weak monoprotic acid with K_a = 3.2 x 10^-8.

What is the conjugate base of HSO₄^-?

Calculate the pH of a buffer prepared by mixing 0.10 mol of sodium formate and 0.05 mol of formic acid in 1.0 L of solution. (HCO₂H: K_a = 1.8 x 10^-4)

At what point in the following titration curve would the pH of the solution be equal to the pK_a of the acid?

Calculate the approximate pH of a 0.100 M solution of formic acid (HCO₂H) in water. (HCO₂H: K_a = 1.8 x 10^-4)

Which of the following equations is valid for a 0.10 M solution of formic acid, HCO₂H? HCO₂H(aq) + H₂O(l) HCO₂^-(aq) + H₃O⁺(aq) K_a = 1.8 x 10^-4

What is the H₃O⁺ ion concentration in a 0.10 M NH₃ solution? (K_b = 1.8 x 10^-5)

Ammonia and the ammonium ion form a conjugate acid-base pair. NH₃(aq) + H₂O(l) NH₄⁺(aq) + OH^-(aq) Calculate the pH of 0.10 M NH₃ if K_a for the NH₄⁺ ion is 5.6 x 10^-10.

Use the following acid-dissociation equilibrium constants for -A solution is prepared with initial concentrations of HA and NaA of 0.50 M and 1.00 M respectively. What is the pH of the solution?

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Exam 11: Acids and Bases

Which of the following solutions would have a pH greater than 7.0?

The hydride ion, (H-), is a stronger base than the hydroxide ion, (OH-). The products of the reaction between H- (aq) and H2O(l) would be.

Consider the following reaction: H2PO4-(aq) + HCO3-(aq) H2CO3(aq) + HPO42-(aq) Brønsted would identify the acidic species as:

What would happen if more formic acid (HCO2H) was added to the following solution at equilibrium? HCO2H(aq) + H2O(l) H3O+(aq) + HCO2-(aq)

Which of the following groups contains salts that all form basic solutions in water?

A solution of weak base is added to a beaker of water. Which of the following will be true as the base is added to the water?

Which of the following is correct (assume all solutions have the same concentration)?

Use the following information to answer H2Se: Ka1 = 1.0 x 10-4, Ka2 = 1.0 x 10-10 -The base-ionization constant for the Se2- ion would be:

What reaction would take place to limit the change in pH when NaOH is added to a mixture of acetic acid (CH3CO2H) and acetate ion (CH3CO2-)?

Which of the following isn't a Brønsted base?

The addition of sodium formate (HCO2Na) to a solution containing formic acid (HCO2H: Ka = 1.8 x 10-4) will cause

Calculate the pH of a solution prepared by dissolving 1.00 x 10-2 moles of sodium hypochlorite (NaOCl) in enough water to produce a 1.00 L of solution. Hypochlorous acid is a weak monoprotic acid with Ka = 3.2 x 10-8.

What is the conjugate base of HSO4-?

Calculate the pH of a buffer prepared by mixing 0.10 mol of sodium formate and 0.05 mol of formic acid in 1.0 L of solution. (HCO2H: Ka = 1.8 x 10-4)

At what point in the following titration curve would the pH of the solution be equal to the pKa of the acid?

Calculate the approximate pH of a 0.100 M solution of formic acid (HCO2H) in water. (HCO2H: Ka = 1.8 x 10-4)

Which of the following equations is valid for a 0.10 M solution of formic acid, HCO2H? HCO2H(aq) + H2O(l) HCO2-(aq) + H3O+(aq) Ka = 1.8 x 10-4

What is the H3O+ ion concentration in a 0.10 M NH3 solution? (Kb = 1.8 x 10-5)

Ammonia and the ammonium ion form a conjugate acid-base pair. NH3(aq) + H2O(l) NH4+(aq) + OH-(aq) Calculate the pH of 0.10 M NH3 if Ka for the NH4+ ion is 5.6 x 10-10.

Use the following acid-dissociation equilibrium constants for -A solution is prepared with initial concentrations of HA and NaA of 0.50 M and 1.00 M respectively. What is the pH of the solution?

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

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The hydride ion, (H^-), is a stronger base than the hydroxide ion, (OH^-). The products of the reaction between H^- (aq) and H₂O(l) would be.

Consider the following reaction: H₂PO₄^-(aq) + HCO₃^-(aq) H₂CO₃(aq) + HPO₄^2-(aq) Brønsted would identify the acidic species as:

What would happen if more formic acid (HCO₂H) was added to the following solution at equilibrium? HCO₂H(aq) + H₂O(l) H₃O⁺(aq) + HCO₂^-(aq)

Use the following information to answer H₂Se: K_a1 = 1.0 x 10^-4, K_a2 = 1.0 x 10^-10 -The base-ionization constant for the Se^2- ion would be:

What reaction would take place to limit the change in pH when NaOH is added to a mixture of acetic acid (CH₃CO₂H) and acetate ion (CH₃CO₂^-)?

The addition of sodium formate (HCO₂Na) to a solution containing formic acid (HCO₂H: K_a = 1.8 x 10^-4) will cause

Calculate the pH of a solution prepared by dissolving 1.00 x 10^-2moles of sodium hypochlorite (NaOCl) in enough water to produce a 1.00 L of solution. Hypochlorous acid is a weak monoprotic acid with K_a = 3.2 x 10^-8.

What is the conjugate base of HSO₄^-?

Calculate the pH of a buffer prepared by mixing 0.10 mol of sodium formate and 0.05 mol of formic acid in 1.0 L of solution. (HCO₂H: K_a = 1.8 x 10^-4)

At what point in the following titration curve would the pH of the solution be equal to the pK_a of the acid?

Calculate the approximate pH of a 0.100 M solution of formic acid (HCO₂H) in water. (HCO₂H: K_a = 1.8 x 10^-4)

Which of the following equations is valid for a 0.10 M solution of formic acid, HCO₂H? HCO₂H(aq) + H₂O(l) HCO₂^-(aq) + H₃O⁺(aq) K_a = 1.8 x 10^-4

What is the H₃O⁺ ion concentration in a 0.10 M NH₃ solution? (K_b = 1.8 x 10^-5)

Ammonia and the ammonium ion form a conjugate acid-base pair. NH₃(aq) + H₂O(l) NH₄⁺(aq) + OH^-(aq) Calculate the pH of 0.10 M NH₃ if K_a for the NH₄⁺ ion is 5.6 x 10^-10.