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Homework answers / question archive / Chapter 15  Acids and Bases:  A Second Look  Multiple Choice 1)The conjugate acid of HPO42- is   H2PO4 H3PO4 PO43- PO42-   e

Chapter 15  Acids and Bases:  A Second Look  Multiple Choice 1)The conjugate acid of HPO42- is   H2PO4 H3PO4 PO43- PO42-   e

Chemistry

Chapter 15  Acids and Bases:  A Second Look

 Multiple Choice

1)The conjugate acid of HPO42- is

 

      1. H2PO4
      2. H3PO4
      3. PO43-
      4. PO42-   e. H2PO4-

 

  1. The conjugate base of HPO42- is

 

      1. H2PO4
      2. H3PO4

c. PO43-    d. PO42-

      1. H2PO4-

 

  1. The conjugate base of H2SO4 is

 

      1. SO42-
      2. H3O+
      3. OH-   d. HSO4-

                    e. H2SO3

 

  1. The conjugate base of H2AsO4- is

 

      1. H2AsO4
      2. H3AsO4
      3. HAsO4-   d. HAsO42-    e. AsO43-

 

  1. The conjugate acid of NH3 is

 

      1. NH4
      2. NH3+
      3. H+
      4. H3O+   e. NH4+
  1. The conjugate acid of H2AsO4- is

 

   a. H2AsO4   b. H3AsO4    c. HAsO4-

      1. HAsO42-
      2. AsO43-

 

  1. Which species is amphiprotic?

 

      1. PO43-(aq)
      2. HCl(g)    c. HSO4-(aq)    d. Cl-(aq)

                     e. CO32-(aq)

 

  1. Which species is amphoteric?

 

      1. HNO3(aq)
      2. Cl-(g
      3. CO32-(aq)   d. HSO3-(aq)    e. PO43-(aq)

 

 

  1. Which species is amphiprotic?

 

      1. AsO43-(aq)
      2. HBr(aq
      3. HF(aq)
      4. SO42-(aq)
    1. e. HCO3-(aq)

 

 

  1. Which species does not have a conjugate base?

 

      1. H2O
      2. H3O+
      3. NH2-
      4. OH-   e. F-

 

 

 

 

 

  1. Which species has a conjugate base?

 

      1. Cl- 
      2. SO42-
      3. CN-   d. OH-

                     e. CO32-

 

 

  1. In the reaction, HClO3  +  N2H  ClO3-  +  N2H5+, which species are an acid-base pair?

 

      1. HClO3, N2H4  
      2. N2H4, ClO3-  
      3. HClO3, N2H5+  
    1. d. N2H4, N2H5+  
      1. ClO3-, N2H5+  

 

 

  1. In the reaction, HClO3  +  N2H  ClO3-  +  N2H5+, two species are both acids?

 

      1. HClO3, N2H4  
      2. HClO3, ClO3-   c. HClO3, N2H5+    d. N2H4, N2H5+

                    e. ClO3-, N2H5+

 

 

  1. In the reaction, HClO3  +  N2H  ClO3-  +  N2H5+, which two species are both bases?

 

      1. HClO3, N2H4  
      2. HClO3, ClO3- 
      3. HClO3, N2H5+ 
      4. N2H4, N2H5+ 
    1. e. ClO3-, N2H4 

 

 

  1. In the reaction, H2PO4-  +  HAsO42-  HPO42-  +  H2AsO4-, which species are a conjugate acidbase pair?

 

      1. H2PO4-, HAsO42-
      2. H2PO4-, H2AsO4-
    1. c. H2PO4-, HPO42-
      1. HAsO42-, HPO42-
      2. HPO42-, H2AsO4-

 

 

 

 

 

16. In the reaction, H2PO4  +  HAsO4

 

   a. H2PO4-, HAsO42-   b. H2PO4-, H2AsO4-    c. H2PO4-, HPO42-

  1. HAsO42-, HPO42-
  2. HPO42-, H2AsO4-

 

 

HPO4  +  H2AsO4 , which two species are both acids?

        • 2-               2-             -

17. In the reaction, H2PO4  +  HAsO4

 

  1. H2PO4-, HAsO42-
  2. H2PO4-, H2AsO4-
  3. H2PO4-, HPO42-   d. HAsO42-, HPO42-    e. HPO42-, H2AsO4-

 

 

HPO4  +  H2AsO4 , which two species are both bases?

        • 2-               2-             -

18. In the reaction, HSO4  +  HS

 

    1. HSO4-, HS-
    2. HSO4-, H2S

                  c. HS-, H2S

  1. HS-, SO42-
  2. H2S, SO42-

 

 

H2S  +  SO4 , which species are a conjugate acid-base pair?

        • -                 2-
  1. In the reaction, HSO4-  +  HS-       H2S  +  SO42-, which two species are both acids?

 

 

   a. HSO4-, HS-   b. HSO4-, H2S    c. HS-, H2S

    1. HS-, SO42-
    2. H2S, SO42-

 

 

  1. In the reaction, HSO4-  +  HS-     

 

    1. HSO4-, HS--
    2. HSO4-, H2S
    3. HS-, H2S   d. HS-, SO42-

                     e. H2S, SO42-

 

 

 

 

 

 

H2S  +  SO42-, two species are both bases?

 

 

  1. In the reaction, HSO4-  +  CN-HCN  +  SO42-, which species are a conjugate acid-base pair?

 

   a. HSO4-, CN-   b. CN-, HCN     c. CN-, SO42-

    1. HCN, SO42-
    2. HCN, HSO4-

 

 

  1. In the reaction, HSO4-  +  CN-       HCN  +  SO42-, which two species are both acids?

 

   a. HSO4-, CN-   b. HSO4-, HCN     c. CN-, HCN 

    1. CN-, SO42-
    2. SO42-, HCN

 

 

 

  1. In the reaction, HSO4-  +  CN-HCN  +  SO42-, which two species are both bases?

 

    1. HSO4-, CN-
    2. HSO4-, HCN 
    3. SO42-, HCN
    4. CN-, HCN    e. CN-, SO42-

             

 

  1. Which is the strongest oxyacid?

 

    1. O

                                       ?

                          H?O?X?O?H

 

    1. O                                               ?

                            H?O?X?O?H

                                       ?

                                        O?H

 

                  c. O

                       ?

                          X?O?H

                                     ?                                                   O

 

 

                    d.                O

                                                                   ?                                          H?O?X?O?H

                                                                    ?                                                          H

 

                                    e.                O                                                                 ?

                            H?O?X?H

                                                                    ?                                                          H

 

 

25.  Which is the strongest oxyacid?

 

  1. O

                                        ?

                            H?O?X?O?H

 

  1. O

                       ?

                          X?O?H

                                     ?                                                   O

 

  1. O                                                                     ?

                            H?O?X?O?H

                                                                    ?                                                          O

 

                 d.                   O

                                      ?

                        H?O?X?O

                                      ?                                       O

 

                    e.                O

                                      ?

                        H?O?X?O?H

                                      ?                                       H

26. For the system

 

NH2OH  +  CH3NH3+CH3NH2  +  NH3OH+

                           

        the position of the equilibrium lies to the left.  Which is the strongest acid in the system?  

 

  1. NH2OH 
  2. CH3NH3+ 
  3. CH3NH2 

                  d. NH3OH+

                    e. NH2OH and CH3NH3+ are equal in acid strength, and are the strongest acids in the system  

 

 

  1. Which is the weakest oxyacid?

 

                     a.                 O

                                        ?

                            H?O?X?O?H

 

                 b.                   O?H

                                       ?

                            H?O?X?O?H

                                       ?

                                        O?H

 

    1. O

                       ?

                          X?O?H

                                     ?                                                   O

 

    1. O                                                                     ?

                            H?O?X?O?H

                                        ?

                                         O

 

    1. O

                                        ?

                           H?O?X?O

                                        ?

                                         O

 

 

  1. For the system

 

NH2OH  +  CH3NH3+CH3NH2  +  NH3OH+

 

        the position of the equilibrium lies to the left.  Which is the weakest base in the system?  

 

                  a. NH2OH 

  1. CH3NH3+ 
  2. CH3NH2 
  3. NH3OH+
  4. CH3NH2 and NH3OH+ are equal in base strength and are the weakest bases in the system

 

 

  1. Which is the strongest oxyacid?

 

      1. O

                       ?

                          X?O?H

                                     ?                                                   O

 

      1. O                                                             ?

                            H?O?X?O?H

                                                                     ?                                                                       O

 

c.             O                                                                     ?

                           H?O?X?O

                                                                     ?                                                                       O

 

      1. O                                               ?

                            H?O?X?O?H

                                                                     ?                                                                       H

 

      1. O                                               ?

                            H?O?X?H

                                                                     ?                                                                       H

 

 

  1. Which species is the most acidic?

 

      1. HClO
      2. HClO2
      3. HClO3   d. HClO4    e. Cl-
  1. Given the following substances in order of increasing acid strength,

HOCl(aq) < HC2H3O2(aq) < HC2O4-(aq) < HOCN(aq) < HNO2(aq) < HCl(aq)

             

        Which species listed below is the strongest base?

 

   a. Cl-(aq)   b. OCl-(aq)

      1. H2C2O4(aq)
      2. NO2-(aq)
      3. OCN-(aq)

 

 

  1. Given the following substances in order of increasing acid strength,

HOCl(aq) < HC2H3O2(aq) < HC2O4-(aq) < HOCN(aq) < HNO2(aq) < HCl(aq)

             

        Which species listed below is the weakest base of that set?

 

      1. C2H3O2-(aq)
      2. OCl-(aq)
      3. H2C2O4(aq)

d. Cl-(aq)

      1. OCN-(aq)

 

 

  1. Given the following substances in order of increasing acid strength,

HOCl(aq) < HC2H3O2(aq) < HC2O4-(aq) < HOCN(aq) < HNO2(aq) < HCl(aq)

             

        Which species listed below is the strongest base of that set?

 

      1. Cl-(aq)
      2. HOCl(aq)   c. C2O42-(aq)    d. NO2-(aq)

                    e. OCN-(aq)

 

 

  1. Given the following substances in order of increasing acid strength,

HOCl(aq) < HC2H3O2(aq) < HC2O4-(aq) < HOCN(aq) < HNO2(aq) < HCl(aq)

             

        Which species listed below is the weakest base of that set?

 

      1. C2H3O2-(aq)
      2. OCl-(aq)
      3. HC2O4-(aq)
      4. HNO2(aq)

e. OCN-(aq)

 

  1. Which species is the weakest acid?

 

      1. HBr
      2. HCl   c. HF    d. HI

 

 

 

  1. Which species is the strongest acid?

 

      1. H2O
      2. H2
      3. H2Se

d. H2Te 

 

 

  1. NH3 can react with BF3, forming NH3?BF3.  In this reaction, 

 

      1. the NH3 acts as a Brønsted base, accepting a proton from the BF3 molecule.
      2. the NH3 acts as a Lewis base, donating a proton to the BF3 molecule.
      3. the NH3 acts as a Brønsted acid, donating a proton to the BF3 molecule.

d. the BF3 molecule acts as a Lewis acid, accepting an electron pair from the NH3 molecule to form a coordinate covalent bond.

      1. the BF3 molecule acts as a Lewis base, donating an electron pair to the NH3 molecule to form a coordinate covalent bond.

 

 

  1. SO2 can react with OH-, forming HSO3- .  In this reaction, 

 

      1. the SO2 acts as a Brønsted acid, accepting a proton from the OH- ion.
      2. the SO2 acts as a Lewis acid, accepting a proton from the OH- ion.
      3. the OH- ion acts as a Brønsted base, donating a proton to the SO2 molecule.

d. the OH- ion acts as a Lewis base, donating an electron pair to the SO2 molecule to form a coordinate covalent bond.

      1. the OH- ion acts as a Lewis acid, accepting an electron pair from the SO2 molecule to form a coordinate covalent bond.

 

 

  1. F- ion can react with BF3, forming the BF4- anion .  In this reaction, 

 

      1. the F- ion acts as a Brønsted base, accepting a proton from the BF3 molecule.
      2. the F- ion acts as a Lewis base, donating a proton to the BF3 molecule.

                                     

      1. the F- ion acts as a Brønsted acid, donating a proton to the BF3 molecule.

d. the BF3 molecule acts as a Lewis acid, accepting an electron pair from the F- ion to form a coordinate covalent bond.

      1. the BF3 molecule acts as a Lewis base, donating an electron pair to the F- ion to form a coordinate covalent bond.

 

  1. CO2 can react with OH-, forming HCO3-.  In this reaction, 

 

      1. the CO2 acts as a Brønsted acid, accepting a proton from the OH- ion.
      2. the CO2 acts as a Lewis acid, accepting a proton from the OH- ion.
      3. the OH- ion acts as a Brønsted base, donating a proton to the CO2 molecule.
      4. the OH- ion acts as a Lewis acid, accepting an electron pair from the CO2 molecule to form a coordinate covalent bond.

e. the OH- ion acts as a Lewis base, donating an electron pair to the CO2 molecule to form a coordinate covalent bond.

 

 

  1. Which pair of reactants will yield H2SO4 as one of its products?

 

      1. SO2  +  OH-
      2. SO3  +  OH-
      3. SO2  +  H2O
      4. SO42-  +  OH-

e. SO3  +  H2O

 

 

  1. Which pair of reactants will yield H2SO3 as one of its products?

 

      1. SO2  +  OH-
      2. SO3  +  OH-                        c. SO2  +  H2O
      1. SO42-  +  OH-
      2. SO3  +  H2O

 

  1. Which solution will have the lowest pH?

 

a. Al(NO3)3(aq)

      1. Ca(NO3)2(aq)
      2. KNO3(aq)
      3. Mg(NO3)2(aq)
      4. Zn(NO3)2(aq)

 

  1. Which solution will have the highest pH?

 

      1. Al(NO3)3(aq)
      2. Ga(NO3)3(aq)

c. AgNO3(aq)

      1. Cu(NO3)2(aq)
      2. Zn(NO3)2(aq)

 

  1. Which solution will have the lowest pH?

 

      1. Zn(NO3)2(aq)
      2. Cd(NO3)2(aq)  
      3. Ga(NO3)3 (aq)  
      4. Hg(NO3)2(aq)  

e. Al(NO3)3(aq)  

 

  1. Which will have the highest pH?

 

      1. Al(NO3)3(aq)
      2. Cd(NO3)2(aq)
      3. Ga(NO3)3 (aq)

d. KNO3(aq)

      1. Zn(NO3)2(aq)

 

 

  1. Five solutions were prepared by dissolving 0.00100 mole of each of the following compounds in enough water to make 1.000 liter of solution.  Which one of the solutions would you expect to be the most acidic?  The one made with

 

      1. CO2
      2. P4O6
      3. P4O10
      4. SO2   e. SO3

 

 

  1. Five solutions were prepared by dissolving 0.00100 mole of each of the following in enough water to make 1.000 liter of solution.  Which one of the solutions would you expect to be the most acidic?  The one made with

 

      1. Na2O
      2. BaO
      3. Ga2O3
      4. Al2O3

e. P4O6

 

  1. Which solution should be the most acidic?

 

a. Al(NO3)3(aq)

      1. Ca(NO3)2(aq)
      2. KNO3(aq)
      3. Mg(NO3)2(aq)
      4. Zn(NO3)2(aq)

 

  1. Which solution should be the least acidic?

 

      1. Al(NO3)3(aq)
      2. Ga(NO3)3(aq)

c. AgNO3(aq)

      1. Cu(NO3)2(aq)
      2. Zn(NO3)2(aq)

 

  1. Which solution should be the most acidic?

 

      1. Zn(NO3)2(aq)
      2. Cd(NO3)2(aq)  
      3. Ga(NO3)3 (aq)  
      4. Hg(NO3)2(aq)  

e. Al(NO3)3(aq)   

 

  1. Which solution should be the least acidic?

 

      1. Al(NO3)3(aq)
      2. Cd(NO3)2(aq)
      3. Ga(NO3)3 (aq)

d. KNO3(aq)

      1. Zn(NO3)2(aq)

 

  1. Five solutions were prepared by dissolving 0.00100 mole of each of the following in enough water to make 1.000 liter of solution.  Which one of the solutions would you expect to have the lowest pH?  The one made with

 

      1. CO2
      2. P4O6
      3. P4O10
      4. SO2   e. SO3

 

  1. Five solutions were prepared by dissolving 0.00100 mole of each of the following in enough water to make 1.000 liter of solution.  Which one of the solutions would you expect to have the lowest pH?  The one made with

 

      1. Na2O
      2. BaO
      3. Ga2O3
      4. Al2O3

e. P4O6

 

  1. An aqueous solution at 25.0 °C has an H+ concentration of 4.0 x 10-2 molar.  What is the OH- concentration in the same solution, in moles per liter?

 

      1. 4.0 x 10-2
      2. 4.0 x 10-9
      3. 4.0 x 10-12

d. 2.5 x 10-13    e. 25.0

 

  1. If the H+ ion concentration in an aqueous solution at 25.0 °C has a value of 0.100 molar, then the OH- concentration in moles per liter is 

 

      1. 0.100
      2. 1.0 x 10-7
      3. 10 x 10-12   d. 1.0 x 10-13    e. 4.0 x 1012

 

  1. If the H+ ion concentration in an aqueous solution at 25.0 °C has a value of 0.100 molar, then the pOH of the solution is 

 

      1. 1.00
      2. 7.00
      3. 12.00   d. 13.00    e. 11.40

 

  1. If the H+ ion concentration in an aqueous solution at 25.0 °C has a value of 0.100 molar, then the pH of the solution is 

 

      1. -1.00
      2. 0.100   c. 1.00    d. 6.90

                    e. 13.00

 

  1. If the OH- ion concentration in an aqueous solution at 25.0 °C is 6.6 x 10-4 M, then the H+ concentration in moles per liter in the same solution is 

 

      1. 1.5 x 10-1
      2. 1.5 x 10-4
      3. 6.6 x 10-10   d. 1.5 x 10-11    e. 6.6 x 10-11

 

  1. If the OH- ion concentration in an aqueous solution at 25.0 °C is 3.4 x 10-3 M, then the H+ concentration in moles per liter in the same solution is 

 

   a. 2.9 x 10-3   b. 2.9 x 10-12    c. 3.4 x 10-17

      1. 5.8 x 10-9
      2. 6.6 x 10-10

 

  1. If the H+ ion concentration in an aqueous solution at 25.0 °C is measured as 6.6 x 10-4 M, then the pH is

 

                    a. 3.00 

b. 3.18    c. 6.60

      1. 9.55
      2. 10.82

 

  1. If the OH- ion concentration in an aqueous solution at 25.0 °C is measured as 3.4 x 10-3 M, then the pH is

 

      1. 2.47 
      2. 7.22
      3. 8.24   d. 11.53    e. 16.47 Section 15.5
  1. Calculate the pH of a mixture made by adding 50.0 mL of 0.20 M HCl(aq) to 150.0 mL of water if the temperature of the mixture is 25.0 °C.

 

      1. 0.70
      2. 1.00
      3. 1.18   d. 1.30

                    e. 13.00

 

  1. Calculate the pH of a 0.020 M solution of Ca(OH)2 whose temperature is 25.0 °C. 

 

      1. 1.40
      2. 0.040
      3. 1.69   d. 12.60

                    e. 12.30 

 

  1. A mixture is made by adding 50.0 mL of 0.20 M NaOH(aq) to 50.0 mL of water. At 25.0 °C, what is its pH?

 

      1. 1.00
      2. 4.55
      3. 7.00   d. 13.00    e. 13.30

 

 

Fill in the Blanks

 

 

  1. What is the formula for the conjugate base of NH3(aq)?  _____

 

 

  1. What is the formula for the conjugate acid of the OH-(aq) ion?  _____

 

 

  1. The strongest base that can exist in aqueous solution is _____.

 

 

  1. The strongest acid that can exist in aqueous solution is _____.

 

 

  1. Which one of the two species, H2Se or H3As, is the stronger Brønsted acid?  _______

 

 

  1. Which one of the two species, HF(aq) or HI(aq), is the weaker Brønsted acid?  _______

 

 

  1. Which one of the two species, H2S or HBr, is the stronger Brønsted acid?  _______

 

 

  1. Three oxyacids with the formulas shown are listed in order of decreasing acid strength:

HZO3 > HYO3 > HXO3

             What is the formula for the strongest conjugate base of these acids?  ______

 

 

74. Three binary acids with the formulas shown are listed in order of decreasing acid strength:

HZ > HY > HX

           What is the formula for the strongest conjugate base of these acids?  ______

 

 

  1. The sulfide ion can react with the sulfur trioxide molecule to produce a thiosulfate ion, as shown below.

2-

    • O     

                                  ?                                ?

                        S2-  + S?O                S—S—O

                                  ?                                ?

                                   O                               O

 

            Which reagent is the Lewis base, if any?  _____

 

 

  1. Selenium atoms can react with the sulfite ion to produce a selenosulfate ion, as shown below

                                                       2-                                 2-

    • O    

                                  ?                                 ?

                       Se   +   :S—O                Se—S—O

                                  ?                                 ? 

                                  O                                 O

 

              Which reagent is the Lewis base, if any?  _______

 

 

  1. The oxide ion can react with the carbon dioxide molecule to produce a carbonate ion, as shown below.

2-

                                  O

  O     

                                  ? 

  ? 

                       O2-  + C             

O—C

                                  ? 

  ? 

                                  O

  O

 

             Which reagent, if any, is the Lewis acid?  _______

 

 

  1. Which solution is more acidic, AlCl3(aq) or InCl3(aq)?  _____

 

  1. At a temperature of 50.0 °C, the value of the ion product constant for H2O is 5.5 x 10-14.  What is the [H+] ion in pure water at this temperature?  ______ 

 

 

True and False

 

 

  1. The conjugate acid of HCl(aq) is H+(aq).  ___

 

 

  1. The conjugate base of NH3 is NH4OH(aq).  ___

 

 

  1. The conjugate acid of Cl-(aq) is HCl(aq).  ___

 

 

  1. NH4Cl(aq)  is one of the conjugate bases of Cl-(aq)  ___

 

 

  1. The H2PO4-(aq)  ion is amphiprotic in water solution.  ___

 

 

  1. O2- ion is produced by the dissociation of MgO when it is dissolved in water. The O2- ion acts as a strong acid.  ___ 

 

  1. The ion product constant for water, Kw, varies with the temperature of the water.  ___ 

 

 

Critical Thinking Questions

 

  1. At 60 °C the value of Kw is 9.5 x 10-14.  Considering this, what is the calculated value for the pOH of a 2.00 x 10-3 M HCl(aq) solution at this temperature?

 

    1. 2.70
    2. 6.51  c. 10.32    d. 11.30

                    e. 13.02

 

  1. At 60 °C the value of Kw is 9.5 x 10-14.  Considering this, what is the calculated value for the pH of a 5.00 x 10-2 M Ba(OH)2(aq) solution at this temperature?

 

    1. 1.00
    2. 1.30  c. 12.02    d. 12.70

                    e. 13.00

 

  1. At 60 °C the value of Kw is 9.5 x 10-14.  Considering this, what is the calculated value for the pOH of pure water this temperature?

 

                    a. 6.02

                  b. 6.51

    1. 7.00
    2. 7.49
    3. 9.50

 

  1. At 60 °C the value of Kw is 9.5 x 10-14.  Considering this, what is the calculated value for the pH of a solution made by dissolving 1.00 g of sodium hydroxide in enough water to make 500 ml of solution at this temperature?   _________

 

 

Short answer

 

91. Explain how NH3 can be both a Bronsted base and a Lewis base, at the same time. 

 

 

 

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