Assignment

Complete the ChemCollective lab.

• View the orientation video to learn how to use the ChemCollective website.

• After watching the video, go to the Cobalt Chloride and LeChatelier’s Principle lab (Links to an external site.) http://chemcollective.org/vlab/85 on ChemCollective.
• Follow the instructions in the PDF that is provided below.
• Complete the Excel Spreadsheet download.
• Write a short discussion (instructions are in the PDF)

This file is downloadable: cobalt_BYH.pdf download

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For help with ChemCollective and with the Excel sheet, you can view the video below. You need to conduct the experiment on the ChemCollective simulator, so I have blurred out some sections in the video.

Solution Equilibria: Cobalt(II) complex ions

In this section, you will examine an equilibrium reaction that occurs in solution. The reaction examined will use something called a complex ion. Many transition metal ions can form bonds with electron rich compounds or ions. These complexes often exhibit different colors, depending on what is bound. In this simulation, we will examine the reaction between hexaaquacobalt(II) ion in equilibrium with tetrachlorocobaltate(II) ion. The cobalt(II) ion bound to water is a pink color where as the cobalt(II) ion bound to chloride ions is blue.

Co(H2O)2+6(aq)+4Cl−(aq)⇀↽CoCl2−4(aq)+6H2O(l)$Co{\left(H_{2}O\right)}_6^{2+}\left(aq\right)+4C{l}^{-}{\left(aq\right)}_{\leftharpoondown }^{\rightharpoonup }CoC{l}_4^{2-}\left(aq\right)+6H_{2}O\left(l\right)$

Image Credit: http://www.docbrown.info/page07/transition07Co.htm

Watch the following video for see what the equilibrium looks like in a real lab setting.