Question 1

All of the following species are amphiprotic EXCEPT

Accepted Answer

A)  H2O. 
B)  HSO4−. 
C)  HPO42−. 
D)  SO42−. 
E)  H2PO4−. 
A)  H2O. 
B)  HSO4−. 
C)  HPO42−. 
D)  SO42−. 
E)  H2PO4−.

Question 2

Lactic acid,HC3H5O3,is found in sour milk.What is the pH of 0.30 M lactic acid? (Ka = 1.4 × 10−4)

Accepted Answer

A)  0.52 
B)  1.07 
C)  2.19 
D)  4.00 
E)  5.12 
A)  0.52 
B)  1.07 
C)  2.19 
D)  4.00 
E)  5.12

Question 3

Which of the following solutions will have a pH of 3.0?

Accepted Answer

A)  1 × 10−3 M CH3CO2H 
B)  1 × 10−3 M NH3 
C)  1 × 10−3 M NH4+ 
D)  1 × 10−3 M HI 
E)  Answers b and c are correct. 
A)  1 × 10−3 M CH3CO2H 
B)  1 × 10−3 M NH3 
C)  1 × 10−3 M NH4+ 
D)  1 × 10−3 M HI 
E)  Answers b and c are correct.

Question 4

The pH of a human blood sample is 7.30.What is concentration of OH− in blood?

Accepted Answer

A)  5.01 × 10−8 M 
B)  2.0 × 10−7 M 
C)  7.3 × 10−7 M 
D)  5.01 × 10−5 M 
E)  2.0 × 107 M 
A)  5.01 × 10−8 M 
B)  2.0 × 10−7 M 
C)  7.3 × 10−7 M 
D)  5.01 × 10−5 M 
E)  2.0 × 107 M

Question 5

The anions derived from strong acids are

Accepted Answer

A)  spectator ions. 
B)  strong bases. 
C)  amphiprotic. 
D)  weak acids. 
E)  weak bases. 
A)  spectator ions. 
B)  strong bases. 
C)  amphiprotic. 
D)  weak acids. 
E)  weak bases.

Question 6

The pH of aqueous 0.50 M hypobromous acid,HBrO,is 4.45.What is the Ka of this acid?

Accepted Answer

A)  2.5 × 10-9 
B)  5.0 × 10-9 
C)  3.4 × 10-7 
D)  3.5 × 10-5 
E)  7.1 × 10-5 
A)  2.5 × 10-9 
B)  5.0 × 10-9 
C)  3.4 × 10-7 
D)  3.5 × 10-5 
E)  7.1 × 10-5

Question 7

A species that can either accept or donate a proton is called

Accepted Answer

A)  a Brønsted-Lowry compound. 
B)  a Lewis base. 
C)  an Arrhenius acid. 
D)  amphiprotic. 
E)  a conjugate pair. 
A)  a Brønsted-Lowry compound. 
B)  a Lewis base. 
C)  an Arrhenius acid. 
D)  amphiprotic. 
E)  a conjugate pair.

Question 8

Which of the following chemical equations corresponds to Ka3 for phosphoric acid,H3PO4?

Accepted Answer

A)  H3PO4(aq)+ H2O(l)  ? H2PO4?(aq)+ H3O+(aq) 
B)  H2PO4?(aq)+ H2O(l)  ? HPO42?(aq)+ H3O+(aq) 
C)  HPO42?(aq)+ H2O(l)  ? PO43?(aq)+ H3O+(aq) 
D)  H3PO4(aq)+ 2H2O(l)  ? HPO42?(aq)+ 2H3O+(aq) 
E)  H2PO4?(aq)+ 2H2O(l)  ? PO43?(aq)+ H3O+(aq) 
A)  H3PO4(aq)+ H2O(l)  ? H2PO4?(aq)+ H3O+(aq) 
B)  H2PO4?(aq)+ H2O(l)  ? HPO42?(aq)+ H3O+(aq) 
C)  HPO42?(aq)+ H2O(l)  ? PO43?(aq)+ H3O+(aq) 
D)  H3PO4(aq)+ 2H2O(l)  ? HPO42?(aq)+ 2H3O+(aq) 
E)  H2PO4?(aq)+ 2H2O(l)  ? PO43?(aq)+ H3O+(aq)

Question 9

Which of the following solutions will have a pH of 11.0?

Accepted Answer

A)  1 × 1011 M Sr(OH)2 
B)  1 × 10−11 M NH3 
C)  1 × 10−11 M HCl 
D)  1 × 10−3 M NH4+ 
E)  1 × 10−3 M NaOH 
A)  1 × 1011 M Sr(OH)2 
B)  1 × 10−11 M NH3 
C)  1 × 10−11 M HCl 
D)  1 × 10−3 M NH4+ 
E)  1 × 10−3 M NaOH

Question 10

The conjugate acid of a weak base is

Accepted Answer

A)  amphiprotic. 
B)  a weak base. 
C)  a weak acid. 
D)  a strong acid. 
E)  a strong base. 
A)  amphiprotic. 
B)  a weak base. 
C)  a weak acid. 
D)  a strong acid. 
E)  a strong base.

Question 11

What is the pH of 6.5 × 10-5 M KOH(aq)at 25°C?

Accepted Answer

A)  -4.19 
B)  1.54 
C)  4.19 
D)  9.81 
E)  12.46 
A)  -4.19 
B)  1.54 
C)  4.19 
D)  9.81 
E)  12.46

Question 12

A salt solution can be acidic,basic,or neutral.When dissolved in water,which of the following salts will make the solution acidic: NaCl,Al2(SO4)3,NaNO3,Na2CO3,KF,and NH4Br?

Accepted Answer

A)  Al2(SO4)3 and NH4Br 
B)  Al2(SO4)3,Na2CO3 and NH4Br 
C)  Al2(SO4)3 and NaNO3 
D)  NaCl,NaNO3 and NH4Br 
E)  Na2CO3,KF,and NH4Br 
A)  Al2(SO4)3 and NH4Br 
B)  Al2(SO4)3,Na2CO3 and NH4Br 
C)  Al2(SO4)3 and NaNO3 
D)  NaCl,NaNO3 and NH4Br 
E)  Na2CO3,KF,and NH4Br

Question 13

A salt solution can be acidic,basic,or neutral.When dissolved in water,which of the following salts will not affect the pH: KCl,FeCl3,NaNO3,CaCO3,LiF,and NH4Br?

Accepted Answer

A)  KCl and FeCl3 
B)  KCl,FeCl3 and NaNO3 
C)  CaCO3 and LiF 
D)  KCl and NaNO3 
E)  CaCO3,LiF,and NH4Br 
A)  KCl and FeCl3 
B)  KCl,FeCl3 and NaNO3 
C)  CaCO3 and LiF 
D)  KCl and NaNO3 
E)  CaCO3,LiF,and NH4Br

Question 14

Determine the equilibrium constant for the reaction HF(aq)+ NH3(aq)  ? F?(aq)+ NH4+(aq)
Given the equilibrium constants for the following reactions.
$\begin{array}{ll}
\mathrm{HF}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{F}-(a q)+\mathrm{H}_{3} \mathrm{O}^{-}(a q) & K_{\mathrm{a}}=6.9 \times 10^{-4} \
\mathrm{NH}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{NH}_{4}^{+}(a q)+\mathrm{OH}-(a q) & K_{\mathrm{b}}=1.8 \times 10^{-5} \
2 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{OH}-(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q) & K_{\mathrm{W}}=1.0 \times 10^{-14}
\end{array}$

Accepted Answer

A)  1.2 × 10?8 
B)  1.2 × 106 
C)  8.1 × 107 
D)  1.0 × 1014 
E)  3.8 × 1015 
A)  1.2 × 10?8 
B)  1.2 × 106 
C)  8.1 × 107 
D)  1.0 × 1014 
E)  3.8 × 1015

Question 15

What is the conjugate acid of ammonia?

Accepted Answer

A)  H+ 
B)  H− 
C)  NH4+ 
D)  NH3 
E)  NH2− 
A)  H+ 
B)  H− 
C)  NH4+ 
D)  NH3 
E)  NH2−

Question 16

What is the conjugate base of [Fe(H2O)6]3+(aq)?

Accepted Answer

A)  H3O+ 
B)  [Fe(H2O)6]2+ 
C)  [Fe(H2O)5H3O]4+ 
D)  [Fe(H2O)5OH]2+ 
E)  [Fe(H2O)5]3+ 
A)  H3O+ 
B)  [Fe(H2O)6]2+ 
C)  [Fe(H2O)5H3O]4+ 
D)  [Fe(H2O)5OH]2+ 
E)  [Fe(H2O)5]3+

Question 17

Ammonia is a weak base (Kb = 1.8 × 10−5).What is the pH of 1.2 M ammonia?

Accepted Answer

A)  2.33 
B)  4.74 
C)  9.26 
D)  10.14 
E)  11.67 
A)  2.33 
B)  4.74 
C)  9.26 
D)  10.14 
E)  11.67

Question 18

The pH of 0.400 M sodium nitrite,NaNO2,is 8.42.What is the Kb for this base?

Accepted Answer

A)  1.7 × 10−11 
B)  3.6 × 10−10 
C)  3.8 × 10−9 
D)  9.5 × 10−9 
E)  8.8 × 10−7 
A)  1.7 × 10−11 
B)  3.6 × 10−10 
C)  3.8 × 10−9 
D)  9.5 × 10−9 
E)  8.8 × 10−7

Question 19

If the OH− concentration in a bottle of an ammonia based cleaner is 3.8 × 10−2 M,what is the H+ concentration? (Kw = 1.0 × 10−14)

Accepted Answer

A)  3.8 × 10−16 M 
B)  2.6 × 10−13 M 
C)  6.8 × 10−2 M 
D)  2.6 × 101 M 
E)  3.8 × 1012 M 
A)  3.8 × 10−16 M 
B)  2.6 × 10−13 M 
C)  6.8 × 10−2 M 
D)  2.6 × 101 M 
E)  3.8 × 1012 M

Question 20

What is the conjugate base of water?

Accepted Answer

A)  H+ 
B)  O2− 
C)  OH− 
D)  H2O 
E)  H3O+ 
A)  H+ 
B)  O2− 
C)  OH− 
D)  H2O 
E)  H3O+

Exam 13: Acids and Bases

All of the following species are amphiprotic EXCEPT

Lactic acid,HC3H5O3,is found in sour milk.What is the pH of 0.30 M lactic acid? (Ka = 1.4 × 10−4)

Which of the following solutions will have a pH of 3.0?

The pH of a human blood sample is 7.30.What is concentration of OH− in blood?

The anions derived from strong acids are

The pH of aqueous 0.50 M hypobromous acid,HBrO,is 4.45.What is the Ka of this acid?

A species that can either accept or donate a proton is called

Which of the following chemical equations corresponds to Ka3 for phosphoric acid,H3PO4?

Which of the following solutions will have a pH of 11.0?

The conjugate acid of a weak base is

What is the pH of 6.5 × 10-5 M KOH(aq)at 25°C?

A salt solution can be acidic,basic,or neutral.When dissolved in water,which of the following salts will make the solution acidic: NaCl,Al2(SO4)3,NaNO3,Na2CO3,KF,and NH4Br?

A salt solution can be acidic,basic,or neutral.When dissolved in water,which of the following salts will not affect the pH: KCl,FeCl3,NaNO3,CaCO3,LiF,and NH4Br?

Determine the equilibrium constant for the reaction HF(aq)+ NH3(aq) ? F?(aq)+ NH4+(aq) Given the equilibrium constants for the following reactions. (aq)+(l)\rightleftharpoons-(aq)+(aq) =6.9\times1 (aq)+(l)\rightleftharpoons(aq)+-(aq) =1.8\times1 2\rightleftharpoons-(aq)+(aq) =1.0\times1

What is the conjugate acid of ammonia?

What is the conjugate base of [Fe(H2O)6]3+(aq)?

Ammonia is a weak base (Kb = 1.8 × 10−5).What is the pH of 1.2 M ammonia?

The pH of 0.400 M sodium nitrite,NaNO2,is 8.42.What is the Kb for this base?

If the OH− concentration in a bottle of an ammonia based cleaner is 3.8 × 10−2 M,what is the H+ concentration? (Kw = 1.0 × 10−14)

What is the conjugate base of water?

Matter and Measurements

Atoms, molecules, and Ions

Mass Relations in Chemistry;stoichiometry

Reactions in Aqueous Solution

Gases

Electronic Structure and the Periodic Table

Covalent Bonding

Thermochemistry

Liquids and Solids

Solutions

Rate of Reaction

Gaseous Chemical Equilibrium

Equilibria in Acid-Base Solutions

Complex Ion and Precipitation Equilibria

Spontaneity of Reaction

Electrochemistry

Nuclear Reactions

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Chemistry of the Metals

Chemistry of the Nonmetals

Organic Chemistry

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Filters

Lactic acid,HC₃H₅O₃,is found in sour milk.What is the pH of 0.30 M lactic acid? (K_a = 1.4 × 10−⁴)

The pH of aqueous 0.50 M hypobromous acid,HBrO,is 4.45.What is the K_a of this acid?

Which of the following chemical equations corresponds to K_a3 for phosphoric acid,H₃PO₄?

What is the pH of 6.5 × 10^-5 M KOH(aq)at 25°C?

A salt solution can be acidic,basic,or neutral.When dissolved in water,which of the following salts will make the solution acidic: NaCl,Al₂(SO₄)₃,NaNO₃,Na₂CO₃,KF,and NH₄Br?

A salt solution can be acidic,basic,or neutral.When dissolved in water,which of the following salts will not affect the pH: KCl,FeCl₃,NaNO₃,CaCO₃,LiF,and NH₄Br?

Determine the equilibrium constant for the reaction HF(aq)+ NH₃(aq) ? F?(aq)+ NH₄⁺(aq) Given the equilibrium constants for the following reactions. (aq)+(l)\rightleftharpoons-(aq)+(aq) =6.9\times1 (aq)+(l)\rightleftharpoons(aq)+-(aq) =1.8\times1 2\rightleftharpoons-(aq)+(aq) =1.0\times1

What is the conjugate base of [Fe(H₂O)₆]³⁺(aq)?

Ammonia is a weak base (K_b = 1.8 × 10−⁵).What is the pH of 1.2 M ammonia?

The pH of 0.400 M sodium nitrite,NaNO₂,is 8.42.What is the K_b for this base?

If the OH− concentration in a bottle of an ammonia based cleaner is 3.8 × 10−² M,what is the H⁺ concentration? (K_w = 1.0 × 10−¹⁴)