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Inorganic Chemistry                                                                                           1)   a

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Inorganic Chemistry                                                                                          

1)   a.   Using Pauling’s Rules estimate the pK₁ values for each of the following acids.  List the following acids in order of acid strength in aqueous solution:

HReO₄            H₃SbO₄           H₂SeO₃            H₂SeO₄

 

b.   Which of the following oxides are likely to be acidic, basic or amphoteric?  Write balanced equations for their reaction with water (and acid or base if amphoteric).

i) As₂O₃                 ii) TeO₂            iii) VO

2.   Choose and explain each of the following:

a.   Strongest Brønsted acid:        SnH₄                SbH₃                            TeH₂

b.   Strongest Brønsted base:        NH₃                 PH₃                              SbH₃

c.   Strongest base to BMe₃:         pyridine           2-methylpyridine         4-methylpyridine

 

3.   For each of the following reactions, identify the acid and base.  Also indicate which acid-base definition (Lewis, solvent system, Brønsted) applies.  In some cases more than one definition may apply.

a.   HF   +  HF  +  SbF5    D    [H₂F]+   +   [SbF₆^-]

b.   XeO₃   +   OH^-    D    [XeO₄H]^-

c.   PtF₅   +   ClF₃    D    [ClF₂]⁺   +   [PtF₆]^-

d.   2 CH₃HgI   +   CaCl₂    D    CaI₂   +   2 CH₃HgCl

e.   [AgCl₂]^- (aq)   +   2CN^- (aq)   ¾®   [Ag(CN)₂]^- (aq)   +   2 Cl^- (aq)

4.   Consider each of the following solvents individually: i) NH₂CH₃  ii) CF₃COOH  iii) H₂SO₄.

 a.  Give the equation for the autoionization of the pure solvent.

b.   Discuss what will happen if H₂O is dissolved in each of the solvents, i.e., what ions will form.  Give appropriate equations.  Will the solution be acidic or basic with respect to the pure solvent?  Will the solute act as a weak or a strong acid or base with respect to the solvent?

Recommended Problems

5.   Using Pauling’s Rules estimate the pK₁ values for each of the following acids.  List the following acids in order of acid strength in aqueous solution:

HClO              HClO₄             HClO₂             HClO₃

6.   Using HSAB theory, choose the better acid or base in the following pairs and explain your choice:

a.   CH₃NH₂ or NH₃ in reaction with H⁺

b.   Which end of SCN- will coordinate to Cr³⁺; Pt²⁺?

c.   Boric acid, B(OH)₃, acts as an acid in water, but does not do so via ionization of a proton.  Rather, it serves as a Lewis acid towards OH^–.  Explain with the use of a balanced equation.

7.   The hydroxoacid Si(OH)₄ is a weaker acid than H₂CO₃.  pKa[Si(OH)₄] = 10 and pKa[H₂CO₃] = 3.6.  Metal silicates M₂SiO₄ (where M = Mg²⁺, Ca²⁺, etc) form the basis of many minerals and ocean sediments.  Write balanced equations for the dissolution of M₂SiO₄ in water containing dissolved CO₂.  Given these equations, explain how silicates dissolved in ocean sediments might limit the increase in CO₂ in the atmosphere that lead to the greenhouse effect.

8.   Using Brønsted acid-base theory, identify the acids and bases in the following reactions.

a.   H₂SO₄   +   [ClO₂]^–     D   HClO₂   +   [HSO₄]^–

b.   AgNO₃   +   CH₃SH   D    HNO₃   +   CH₃SAg

c.   CdCl₂   +   H₂Te    D    2 HCl   +   CdTe

d.   2 HF   +   PF₅    D     H₂F⁺   +   PF₆^–

9.   For each of the following reactions, identify the acid and base.  Also indicate which acid-base definition (Lewis, solvent system, Brønsted) applies.  In some cases more than one definition may apply.

a.   HNO₂   +   2 HF   ¾®   [H₂NO₂]⁺   +   [HF₂]^-

b.   Li₃N   +   2 NH₃    D    3 Li⁺   +   3 NH₂^–

c.   Al₂Cl₆   +   2 NH₃    D    2 H₃N¾AlCl₃ 

10. a.   Aluminum trifluoride (AlF₃) is insoluble in HF, but dissolves when NaF is present.  When BF₃ is passed into the solution, AlF₃ is precipitated.  Account for these observations using equations.  (Is this Autoionization, Bronsted-Lowry or Lewis acid/base?)