[CHM 115] Some Solutions....

[Andrew J. Pounds]

So as I mentioned when I posted the last quiz solution, I have been 
having some problems with my scanner.  I therefore went through and 
pulled out some of the solutions to the even numbered recommended 
problems from the solutions manual.

Hope these help.   Remember though -- you have a BUNCH of worked 
solutions for the odd numbered problems and you also have the examples 
that I worked in class.


Chapter 15:

15.16 For H3O+ ion, the range is 4.5 ×10−8 M to 3.5 ×10−8. For OH– ion 
the range is 2.2 ×10−7 to 2.8 ×10−7 M.

15.22   Kb = 6.7 x 10^-10

15.30 a)   pH = 2.664   <-- note, 3 sig figs

15.46 a)  pH = 3.04     b)  pH = 2.8

15.58 The tablet contains 0.5243 g of CaCO3

15.100  The pH is 3.98

15.106  a)  pH = 10.6     b) pH = 5.4


Chapter 16:

16.12   Solubility is 2.0x10^-6 mol/L

16.32   a)  Ksp = 1.2 × 10−11 = S (2S)2 from which S = 1.4 × 10−4 mol L−1

             b)   the solubility is 0.12 mol L−1

16.34 a) Solubility will increase as CO3 − reacts with H3O+ to give HCO3 .
           b) Solubility will show little change because HBr is a strong 
acid.
           c) Solubility will increase as HS− (from the dissolution of 
the MnS) reacts with H3O+ to give H2S.



-- 
Andrew J. Pounds, Ph.D.  (pounds_aj at mercer.edu)
Professor of Chemistry and Computer Science
Mercer University,  Macon, GA 31207   (478) 301-5627
http://faculty.mercer.edu/pounds_aj

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