Acids & Bases – Review 

1)    For each reaction listed, identify the proton donor (acid), the proton acceptor (base), the conjugate acid and the conjugate base:

a.    H₂PO₄^-_(aq)  +  OH^-_(aq)  ?  HPO₄^2-_(aq)  +  H₂O_(l) 

b.    H₃O⁺_(aq)  +  Cl^-_(aq)  ?  H₂O_(l)  +  HCl_(aq)

c.    NH₄⁺_(aq)  +  H₂PO₄^-_(aq)  ?  NH_3(aq)  +  H₃PO_4(aq) 

2)    For each of the following salts, predict whether an aqueous solution would be acidic, basic, or neutral.

a.  CaI₂                             b.  K₂CO₃                               c.  Au(NO₃⁾₂ 

d.  Ca(C₂H₃O₂)₂              e.  CuSO₄                              f.  LiCl

3)    A solution of Ca(OH)₂ is found to have a [OH^-] of 2.73 x 10^-5 M.  What is the [H₃O⁺] of this solution?  What is the pH of this solution?  What is the pOH of this solution?  Is this solution acidic or basic?

4)    You have made a solution of 4.50 x 10^-3 M HNO₃.  What is the [H₃O⁺] of this solution?  What is the [OH^-] of this solution?  What is the pH of this solution?  Is this solution acidic or basic?

5)    You have made a solution of 9.12 x 10^-4 M NaOH.  What is the [H₃O⁺] of this solution?  What is the [OH^-] of this solution?  What is the pH of this solution?  Is this solution acidic or basic?

6)    In lab, you discover the pH of your solution to be 5.43.  What is the [H₃O⁺] of this solution?  What is the [OH^-]?  Is this solution acidic or basic?  What is its pOH?

7)    In lab, you discover the pH of your solution to be 7.21.  What is the [H₃O⁺] of this solution?  What is the [OH^-]?  Is this solution acidic or basic?  What is its pOH?

8)    In the titration of 45.0 mL of an NH₃ solution, the end point was reached when 18.9 mL of 0.250 M HCl was added.  What is the concentration of the ammonia solution?

9)    25.0 mL of an unknown solution of H₂SO₄ was titrated to the end point with 38.4 mL of 0.512 M KOH.  What is the concentration of the sulfuric acid?