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Chemistry 12 AcidBase Equilibrium I Name: Date: Block: 1. Properties of Acids & Bases 2. Definitions of Acids and Bases 3. Conjugate AcidBase Pairs 4. Amphiprotic Substances Properties of Acids and Bases Acids Bases 1. 1. 2. 2. 3. 3. 4. 4. Definitions of Acids and Bases Arrhenius Theory of Acid and Bases • Arrhenius acids _________________ H + ions • Arrhenius bases __________________ OH ions. Typically… Acid + Base Salt + Water HCl (aq) + NaOH (aq) NaCl (aq) + H2O (l) A salt is an ionic compound that does not contain H + or OH ions. 1. Identify each of the following substances as an Arrhenius acid, an Arrhenius base, a salt or a molecular compound. a. HNO3 b. Al(OH)3 c. Al(NO3)3 d. NO2 e. H2SO4 f. XeF6 g. CH3COOH h. NaCH3COO i. KOH j. NH3

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  •    

    Chemistry  12  Acid-‐Base  Equilibrium  I  

    Name:  Date:  Block:  

     1. Properties  of  Acids  &  Bases  2. Definitions  of  Acids  and  Bases  3. Conjugate  Acid-‐Base  Pairs  4. Amphiprotic  Substances  

     Properties  of  Acids  and  Bases    

    Acids   Bases  1.   1.  

    2.   2.    

    3.   3.    

    4.   4.  

       Definitions  of  Acids  and  Bases    Arrhenius  Theory  of  Acid  and  Bases  

    • Arrhenius  acids  _________________  H+  ions  

    • Arrhenius  bases  __________________  OH-‐  ions.  

    Typically…  

    Acid   +   Base   à   Salt   +   Water  

    HCl  (aq)   +   NaOH  (aq)   à   NaCl  (aq)   +   H2O  (l)  

     

    A  salt  is  an  ionic  compound  that  does  not  contain  H+  or  OH-‐  ions.  

     

    1. Identify  each  of  the  following  substances  as  an  Arrhenius  acid,  an  Arrhenius  base,  a  salt  or  a  molecular  

    compound.  

    a.  HNO3   b.  Al(OH)3  

    c.  Al(NO3)3   d.  NO2  

    e.  H2SO4   f.  XeF6  

    g.  CH3COOH   h.  NaCH3COO  

    i.  KOH   j.  NH3  

     

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  •    

    2. Complete  the  following  neutralization  equations.  Make  sure  each  equation  is  balanced,  and  circle  and  

    name  the  salt  produced.  

     

    a. ___  CH3COOH  +  ___  LiOH  à  

    b. ___  HI  +  ___  Ca(OH)2  à  

    c. ___  Mg(OH)2  +  ___  H3PO4  à  

    3. Write  the  formula  of  the  acid  and  base  that  react  to  form  each  salt  listed.  

      Acid   Base  

    a.  KNO2      

    b.  NH4Cl      

    c.  CuC2O4      

    d.  NaCH3COO      

     

     

    Brønsted-‐Lowry  Acids  and  Bases  

    A  broader  definition    

    • Brønsted-‐Lowry  acids  _________________  H+  ion.  

    • Brønsted-‐Lowry  bases  _________________  H+  ion.  

     

    Example  1:  

    HCl  (aq)  +  H2O  (l)  à  H3O+  (aq)  +  Cl-‐  (aq)  

    ________        ________            

     

    HCl  ________________  a  proton,  H+,  to  the  water  molecule  –  HCl  is  acting  as  a  ________________________________.  

    H2O  _______________  a  proton,  H+,  from  HCl  –  water  is  acting  as  a  __________________________________.  

     

       

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  •    

    Example  2:  

    NH3  (aq)  +  H2O  (l)  ⇋  NH4+  (aq)  +  OH-‐  (aq)  

    ________        ________                    ________        ________  

           

    NH3  ____________  a  proton,  H+.  NH3  is  acting  as  a  ________________________________.  

    H2O  ____________  a  proton,  H+.  water  is  acting  as  a  __________________________________.  

     

     

     

     

    In  the  reverse  reaction….  

    NH4+  ____________  a  proton,  H+.  NH3  is  acting  as  a  ________________________________.  

    OH-‐  ____________  a  proton,  H+.  water  is  acting  as  a  __________________________________.  

                 Practice!  Complete  the  following  equations:    

    HClO4  +  H2O  à   HI  +  H2O  à  

    HBr  +  H2O  à   HCl  +  H2O  à  

    HIO3  +  H2O  ⇋   HIO3  +  H2O  ⇋  

    HIO3  +  OH-‐  ⇋   H3PO4  +OH-‐  ⇋  

    HC2O4-‐  +  H3O+  ⇋   SO32-‐  +  H3O+  ⇋  

         

       

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  •    

     Conjugate  Acid-‐Base  Pairs    Example  3  –  identify  the  Brønsted-‐Lowry  acid  and  base  in  the  following  reaction:  

     

    HF  (aq)  +  CN-‐  (aq)  ⇋  HCN  (aq)  +  F-‐  (aq)  

    ________        ________                    ________        ________  

     

    Two  substances  that  differ  by  one  H+  ion  are  called  a  conjugate  acid-‐base  pair.  

     

    In  the  example  above,  HF  and  F-‐  together  form  one  conjugate  acid-‐base  pair,  and  CN-‐  and  HCN  form  the  

    other  conjugate  acid-‐base  pair.  

    In  the  forward  reaction…  

    • HF  is  acting  as  a  BL  acid  

     

     

    • CN-‐  is  acting  as  a  BL  base  

     

                 Let’s  practice!    

       

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  •    

    Complete  the  following  table:  

    Conjugate  Acid  (donates  a  proton)  

    Conjugate  Base  (accepts  a  proton)  

    H2C2O4    

      SO32-‐  

    HCO3-‐    

    H2O2    

      H2BO3-‐  

    HCOOH    

      C6H5O72-‐  

      H2O  

    H2O    

     

    Hebden  Workbook  Pg.  117  #11,  12,  Pg.  119  #13    

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  •    

     Amphiprotic  Substances    Consider  the  two  reactions  below:    

    NH3  (aq)  +  H2O  (l)  ⇋  NH4+  (aq)  +  OH-‐  (aq)  

    HF  (aq)  +  H2O  (l)  ⇋  H3O+  (aq)  +  F-‐  (aq)  

     

    In  the  first  reaction,  water  acts  as  a  BL-‐acid.  In  the  second  reaction,  water  acts  as  a  BL-‐base.  

     

    An  amphiprotic  substance  has  the  ability  to  act  as  an  acid  or  a  base,  depending  on  what  it  is  reacting  with.  

       1.  Which  of  the  following  would  be  expected  to  exhibit  amphiprotic  behavior.  Circle  those  that  apply.    

    Se2-‐   HSe-‐   H2Se   H3PO4   HPO42-‐   HSO3-‐      2.  Of  the  species  that  were  circled  in  the  above  question,  write  two  equations:  (1)  behaving  as  an  acid  with  water  (2)  behaving  as  a  base  with  water  

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