PROCEDURE $1.$ Add a stock solution of $1$M CoCl$2$ and a $250$mL Erlenmeyer flask to the workbench from the stockroom. $2.$ Transfer $50\mathrm{.}00$mL of the stock solution to the empty flask by dragging the stock solution onto the flask and typing in the transfer amount. $3.$ Record the temperature and your observations and ion concentrations in a data table. $4.$ Add a stock solution of $12$M HCl from the stockroom to the workbench. Transfer $10\mathrm{.}00$mL of $12$M HCl to your cobalt solution. $5.$ Record the temperature and your observations and ion concentrations in a data table. $**$Hint: Record the temperature as soon as the solutions are mixed. Record the ion concentrations once they have become consistent $($and the temperature has returned to $25\backslash$deg C$).6.$ Add a stock solution of $6$M AgNO$3$ from the stockroom to the workbench. Transfer $10\mathrm{.}00$mL of the $6$M AgNO$3$ to your cobalt solution. $7.$ Record the temperature and your observations and ion concentrations in a data table. $8.$ Right$-$click on your cobalt solution, and then click on $$Thermal Properties$.$ Insulate the flask from the surroundings, and change the temperature to $0\backslash$deg C$.9.$ Record the temperature and your observations and ion concentrations in a data table. $10.$ Right$-$click on your cobalt solution, and then click on $$Thermal Properties$.$ Insulate the flask from the surroundings, and change the temperature to $100\backslash$deg C$.11.$ Record the temperature and your observations and ion concentrations in a data table. $12.$ Try to shift the reaction so that the products are heavily favoured and a bright blue solution appears $($there are a couple of different way that you can do this$).13.$ Place an empty $500$mL Erlenmeyer flask on the workbench. Right click on your blue cobalt solution and chose $$Remove Solid$.14.$ Transfer $50\mathrm{.}00$mL of your blue cobalt solution to the $500$mL Erlenmyer flask. $15.$ Transfer $100$mL of H$2$O from the stockroom to your workbench. $16.$ Transfer the H$2$O to your $50$mL cobalt solution. $17.$ Record the temperature and your observations and ion concentrations in a data table. RESULTS Table $1$: The Effect of Concentration and Temperature Stressors on a Cobalt Equilibrium Observations $($Colour$)$ Temperature $(\backslash$deg C$)[$Co$($H$2$O$)62+][$Cl$-][$CoCl$42-]$ Keq Cobalt Eq$.$ Add $12$M HCl Add $6$M AgNO$3$ Temp: $0\backslash$deg C Temp: $100\backslash$deg C Add H$2$O ANALYSIS For your analysis section, complete the following: $1.$ Write the equilibrium constant expression for the cobalt equilibrium. $2.$ Calculate the Keq of the cobalt equilibrium before and after each stressor was added. Record your answer in the data table. Include a sample calculation in this section. $3.$ What direction did the equilibrium shift when you added HCl$?$ What evidence do you have to support this? Explain the shift using Le Chatelier$$s principle. $4.$ What direction did the equilibrium shift when you added AgNO$3?$ What evidence do you have to support this? What evidence do you have to support this? Explain the shift using Le Chatelier$$s principle. $5.$ How did the equilibrium shift when the system was diluted? What evidence do you have to support this? Explain the shift using Le Chatelier$$s principle. $6.$ Was this reversible reaction exothermic or endothermic? How do you know? Explain using Le Chatelier$$s principle. $7.$ Did the Keq value for the equilibrium system exhibit any reasonable change as a result of the stresses you applied? If so$,$ which stresses caused a change in the Keq value? DISCUSSION For the discussion section, please include: $$ A summary of your experiment. $$ Were you able to meet the objectives using this procedure? Why or why not? $$ How did your results compare with your hypotheses? Were there any discrepancies? Explain. $$ If you were conducting this experiment under real laboratory conditions, what would be $2$ likely sources of error? How would you improve on this experiment?