Cobalt (11) Complexes And LeChatelier's Principle. To Load The Experiment, Select "Load Homework” From The File Menu, And Select "Chemical Equilibrium”, “Cobalt Lab". [Co(H20)6]Laq) + 4Cl(Aq) = [CoCl4]{Aq) + 6H20 (1) I) Predict The Effect Of Adding Chloride Ions. Add 25 ML Of [Co(H2O).]*2 To An Empty Erlenmeyer Flask. Now Add 12 M HCl In 1 ML

 

EXERCISE. Cobalt (II) complexes and LeChatelier's Principle. To load the experiment, select "Load Homework" from the File menu, and select "Chemical Equilibrium", "Cobalt Lab". [Co(H2O)6]) + 4Cl(aq) = [COC14]aq) + 6HO (1) Predict the effect of adding chloride ions. Add 25 mL of [Co(H2O)6]2 to an empty Erlenmeyer flask. Now add 12 M HCI in 1 mL increments until the equilibrium color has changed. (Hint: Type in 1 for the volume to be transferred, and then keep clicking pour until you see a change, counting clicks to determine total volume added.) Q1) Describe what is happening with your solution. Record the change in color with the increase in Cl amount. Explain. ii) Predict the effect of removing chloride ions. Now remove some of the free chloride ions by adding some silver nitrate (Hint: add 1 mL amounts of the silver nitrate successively until the equilibrium has been shifted instead of a whole bunch at once). Ag* reacts with free chloride ions by forming a precipitate (see reaction below), and thus removes them from the solution. Q2) AgNO3(aq) + Cl(aq) AgCl(s) + NO 3(aq) Describe what is happening with your solution. Record the change in color with the increase in Ag amount. Explain.