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Homework answers / question archive / Inorganic Chemistry                                                                                           Acids & Bases                                                                                                      1)   a

Inorganic Chemistry                                                                                           Acids & Bases                                                                                                      1)   a

Chemistry

Inorganic Chemistry                                                                                          

Acids & Bases                                                                                                     

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?

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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?)

 

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