1.   

a.      Base (Strong) -> Li⁺+OH^-

b.      Base (weak) -> Mg²⁺+2OH^- (these ions will be found in solution but to a lesser extent than if this was a strong base)

c.       Acid (weak) -> H⁺ + ClO^- (these ions will be found in solution but to a lesser extent than if this was a strong acid)

d.      Acid (strong) -> H⁺ + Br^-

e.      Base (Strong) -> K⁺ + OH^-

f.        Acid (weak) -> HSO₃^- + H⁺ (these ions will be found in solution but to a lesser extent than if this was a strong acid)

2.   It has a proton that can be transferred3.   Left. The concentration of hydroxide and hydronium ions in pure water is very, very small. Although it is rarely something you need to worry about when looking at acids and bases in solution,it does help account for certain properties of water such as electrical conductivity.

4.   HCO₃^- + HCl -> H₂CO₃ (acting as a base)HCO₃^- + NaOH -> NaCO₃ + H₂O (acting as an acid)

5.   SO₄^2- + H₃O⁺

6.   Parent acid, Parent base, conj acid, conj base

1. 
   
   1. HF+H₂O?F^?+H₃O⁺
   2. HSO₄^-+NH₃?SO₄^?2+NH⁺⁴
   3. C₂H₃O₂^?+HCl?HC₂H₃O₂+Cl^?
   4. HNO₂+H₂O? H₃O⁺+NO₂^?
   5. HCN+H₂O?H₃O⁺+CN^?

7.   HCl is a stronger acid than H₂S. Acids become stronger as the X-H bond becomes more polar.  The larger the difference in the electronegativity between X and H atoms, the easier it is to form H ⁺ and X ^- ions.

8.   H₃PO₄ > NaH₂PO₄ > Na₂HPO₄ > Na₃PO₄.  According to the Bronsted definition of acids and bases, acids donate protons and bases accept them.  Proton donation becomes much more difficult as the resulting anions become more electronegative.  H₃PO₄ can form H₂PO₄^- more easily than H₂PO₄^- can form HPO₄^2-, etc.

9.   Remember, a Lewis acid has an unfilled octet and thus is able to accept a pair of electrons.  A Lewis base has a lone pair of electrons to "donate"a.      Lewis base.  Nitrogen has a lone pair

b.      Lewis acid.  Ag⁺ is a cation.

c.       Lewis acid.  Ni²⁺ is a cation.

d.      Lewis acid.  Pt⁴⁺ is a cation.

e.      Lewis base.  Oxygen has lone pairs

f.        Lewis acid.  Sulfur can accept the lone pair electrons from another atom

10.                SiF₄ has a central Silicon Atom which can expand its octet to 12 (compared to the typical 8) so that it forms [SiF₆]^2-.
18. K_auto = [H₃O⁺][OH^?]/[H₂O]²
K_w = [H₃O⁺][OH^?] = K_auto[H₂O]²
19. H₂O(l) + HNO₃(g) ? H₃O⁺(aq) + NO₃^?(aq); water is the base H₂O(l) + NH₃(g) ? OH^?(aq) + NH₄^?(aq); water is the acid
20. KH2SO4=[H3SO4+][HSO4?]=K[H2SO4]2;[H₃SO₄⁺] = 0.3 M; the fraction ionized is 0.02.