Problems 1-3 are about the following reaction:

HSO₄^- (aq) <===> H⁺ (aq) + SO₄^-2 (aq) ΔH = -41.6 kJ/mol

1. The following questions require knowledge of Le Chatelier's Principle. Answer each AND give a BRIEF description of your reasoning. (In other words, what happens and why?) Be sure to answer the correct question!!

a) What direction will the equilibrium shift if the pressure is increased and why?

b) What will happen to the concentration of sulfate if the solution is heated?

c) If 6.00 M H⁺ was added to the mixture what would happen to the concentration of hydrogen sulfate (HSO₄^- ) and why?

d) If Ba⁺² was added to the mixture, what would happen to the concentration of sulfate and why? (Barium sulfate is VERY insoluble…kind of like the Fe(OH)3 in the example I did in class)

 2. If [HSO₄^- ] = 2.00 M and [H⁺ ] = 1.40 M and

[SO₄^-2 ] = 2.43 x 10^-8 M, and the mixture is at equilibrium, what is the value of K? (Include units and show work.)

3. At a different temperature the value of K is 435 (no this is NOT the value you should have gotten!). If you make up a solution that starts 1.00 M HSO₄^- , and allow it to reach equilibrium (using the new value for K), what will be the final concentration of all species present? (SHOW ALL WORK)

4. If you make up a solution that is 1.00 M H⁺ , and 1.00 M SO₄^-2, and allow it to reach equilibrium (again using the new K), what will be the final concentrations of all species present? (SHOW ALL WORK)

5. The K_sp of Cd(OH)₂ = 1.2x10^-14. What is the concentration of hydroxide in a saturated solution?

6. A solution is made of 4.6x10^-3M hydroxide and 3.8x10^-6M Cd⁺². Will a precipitate form? Use the K_sp from #5.