Solve the following problems using the systematic approach to equilibrium problems.
1. Determine the concentration of Ag+, CN-, and HCN in a saturated solution of AgCN where the pH is fixed at 5.90.
2. 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.
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).
With this solution, you will have to do some of the calulations yourself. Web links are provided for the acids and bases. Problem 1 and 2 are set up in a lot of depth, merely do not include final calculations (a calculator will be needed). Included is a detailed explanation of solubility product constant calculations and acid dissociation calculations. Steps for each of the problems are identified. 695 words.