1. Lecture 102/7/07

2. Write the chemical equation for the formation of the complex ion, and write its formation constant expression. a) [Ag(CN) 2 ] -

3. Compare the molar solubility of AgCl in pure water, in 1M NaCl, and in 1.0 M NH 3 solution. K sp (AgCl) = 1.8 x 10 -10 K f (Ag(NH 3 ) 2 + ) = 1.6 x 10 7

4. Mix 0.1 L of 0.3 M Ca(NO 3 ) 2 and 0.2 L of 0.06 M NaF. Does a precipitate form? K sp (CaF 2 ) = 3.9 x 10 -11

5. How would the given changes affect the equilibrium for following reaction? SiH 4 (g) + 2 O 2 (g) ⇄ SiO 2 (s) + 2 H 2 O (g)  H = -1100 KJ/mol Adding more SiO 2 Shift toward reactants Shift toward products No change Raising the temp. Shift toward reactants Shift toward products No change Removing H 2 O Shift toward reactants Shift toward products No change Reducing the volume of the reaction flask Shift toward reactants Shift toward products No change Adding a catalyst Shift toward reactants Shift toward products No change

6. Hemoglobin, Hb, has four Fe atoms per molecule that, on the average, pick up roughly three molecules of O 2. Hb (aq) + 3O 2 (g) ⇆ Hb(O 2 ) 3 (aq) Discuss mountain (high altitude) or space sickness in terms of this equilibrium.

7. Using the solubility rules, suggest a method to separate the following ions. Pb 2+, Ca 2+, Sr 2+, Li +, and Mn 2+