Solve the following problems using the systematic approach to
equilibrium problems.
Determine the concentration of Ag+, CN-, and HCN in a saturated solution
of AgCN where the pH is fixed at 5.90.
Determine the concentration of NH4+, NH3, CH3COOH (acetic acid), and
CH3COO- (acetate ion) if 0.0050 moles of ammonium acetate (NH4+ -OOCCH3)
is dissolved in 1.00 L of water and the pH is fixed at 5.90.
Please show all work!
3. Calculate the pH of 5.0 x 10-8 M HCl. You will need to use the
systematic treatment of equilibrium, and there are no simplifying
assumptions you can make. Approximately what fraction of the total H+
in this solution is due to the autoprotolysis of water?
4. Write chemical reactions for the following:
a. Ka for 3-nitrobenzoic acid
b. Kb for 3-nitrobenzoate
c. Kb for benzylamine
d. Ka for benzylammonium ion
5. Calculate the pH and fraction of dissociation for a 0.10 M solution
of formic acid.
6. Calculate the pH and fraction of association for a 0.10 M solution
of sodium formate.
7. Calculate the pH and fraction of dissociation for a 0.050 M solution
of ethanolamine (2-amino ethanol).
Chemistry Homework Solutions
#36934
Systematic Treatment of Equilibrium
The attached problems in MS Word involve the systematic treatment of problem solving in chemical equilibria. The college course is Quantitative Analysis. Excellent knowledge of some inorganic and organic acids and the systematic approach in solving chemical equilibria are required.
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