The following reaction has a Keq = 6.3 × 10–38. 3Fe(OH)3 (s) ⇌ Fe3+(aq) + 3OH3–(aq) Use this information to explain your observations of the position of the equilibrium in the presence of OH–(Part 1b). (HINT: Think about what happens to Fe3+(aq) when there is OH– (aq) present.)
3. The following reaction has a Keq = 6.3 × 10–38.
3Fe(OH)3 (s) ⇌ Fe3+(aq) + 3OH3–(aq)
Use this information to explain your observations of the position of the equilibrium in the presence of OH–(Part 1b). (HINT: Think about what happens to Fe3+(aq) when there is OH– (aq) present.)
4. As part of the discussion, explain your results from Part 2 within the context of Le Châtelier’s Principle. Look at the cobalt equilibrium and decide which is pink (I or II) and which is blue?
Co(H2O)62+ + 2Cl– ⇌ CoCl2(H2O)2 + 4H2O
I II
As part of the discussion, explain the effect of changing the temperature based upon your observations. Is the cobalt equilibrium exothermic or endothermic, as it is written? Explain your observations with respect to the addition of saturated aqueous sodium chloride solution and the addition of water. (HINT: what is the major component of aqueous sodium chloride?)
Step by step
Solved in 3 steps with 7 images
