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Investigation of reversible reactions at equilibrium - CuCl2 (s) was added to HCl , NaCl , H2SO4 respectively .

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Introduction

Data collection The table below shows the qualitative observations that were made when CuCl2 (s) was added to HCl , NaCl , H2SO4 respectively . Chemical Compound Observations CuCl2 (s) CuCl2 (s) was green in color . When CuCl2 (s) is added in water , the color of the solution is cyan and is transparent in nature . HCl (aq) Upon adding HCl (aq) to the aqueous solution , the drop of HCl (aq) at the point of impact in the solution forms yellow in color. Upon adding more HCl (aq) to the solution, the solution becomes green in color. When water was added to the solution, the color of the solution went back to cyan, the original color of the solution. H2SO4 (aq) When H2SO4 (aq) is added to the CuCl2 aqueous solution, upon the impact of the drop of the acid , the drop becomes yellow in color in the solution , upon stirring the color disappears . Upon adding more H2SO4 the color of the solution changes slowly from cyan to lighter cyan / blue. When water is added to the solution, the solution went to a color of bluish-green which has a slight difference of color compared to the original solution. NaCl (s) ...read more.

Middle

According to Le chatelier?s principle when a system under equilibrium is stressed , the position of the equilibrium moves such that in order to oppose the stress . Hence in this equation the position of the equilibrium shifts from left to right due to cincrease the in concentration of the Cl- ions .AS the position of the equilibrium shifts to the right the more amount of CuCl42- and H2O is produced and hence their concentration in the equilibrium increases. The increase in the CuCl42- counts for the change of the color of the solution from cyan to green . When H2O is added to water there is an increase in the concentration of water in the right hand side , hence in order to overcome the concentration of water the position of the equilibrium shifts to the left . When H2SO4 is added to the solution H2SO4 breaks into H+ ions and SO42- ions . There is an excess of H+ ions in the right hand side of the equation , these extra H+ ions react to form H2O , hence there is an excess of the concentration of water on the right side . ...read more.

Conclusion

When HCl is added to it The color of the solution turns from pink to violet to purple to blue . and then eventually becomes navy blue / dark blue . When water is added to the solution , the color of the solution goes back to the original color . CoCl2 + HCl â Co(H2O)6+2 + Cl- When HCl is added to the following equilibrium there is an excess of Cl- ions in the left side of equilibrium . Hence according to Le chatelier’s principle i.e. when a system under equilibrium is stressed the system moves in order to minimize the stress . The position of the equilibrium in the equation above shifts to the left in order to counter the increase in the concentration of the Cl- . More CuCl42- and H2O is produced and hence their concentration in the equilibrium increases. The increase in the CuCl42- counts for the change of the color of the solution from cyan to green . When H2O is added to water there is an increase in the concentration of water in the right hand side , hence in order to overcome the concentration of water the position of the equilibrium shifts to the left . This accounts for the change in the color of the solution from green back to the original color of the solution i.e. cyan ...read more.

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