Chemical Equilibrium

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RESULTS AND DISCUSSION

In the Iron (II) - Silver Ions System the reaction had a balance chemical equation of Fe2+ + Ag+  Fe3+ + Ag(S). The process if centrifugation is used in this part of the experiment to be able to separate the supernatant and the precipitate. And the supernatant will be used to test for the presence of Fe2+, Ag+ and Fe3+ in the solution. Results showed that there is a positive presence for FE 2+, Fe3+ and Ag+ because of the visible change of color of Prussian blue precipitate, blood red solution and white precipitate. The balance chemical equation for the reactions were Fe2+ + K3Fe(CN)6 - Fe(CN)36 +K2 +Fe , Fe3+ + KCSN  Fe(SCN)3+K and Ag+ + HCI  AgCl + H+. The bonding between the ions in the solution is weak because it can be separated easily and they are very reactive to the solution used as the test reagents since the range of the Keq for this reaction is greater than 102 , a forward reaction that is highly favored with the formation of product. In addition HCl the solution formed white precipitate. Because HCl is responsible for the precipitate being dissolve and it also decolorizes the solution because in the chemical equilibrium it shifts forward to the product’s side of Ag+ + HCI  AgCl + H+ producing more product.

In the copper-ammonia system the balance chemical equation is [Cu(H2O)6]2+(aq) + 4NH3(aq) ⇌ [Cu(NH3)4(H2O)2)]2+(aq) + 4H2O(l) and the initial color was pale blue and when 8 drops of NH3 was added to the solution the color changed to dark blue having the chemical equilibrium have a forward reaction while for the addition of 9 drops of HCl the color went back to pale blue and the equilibrium shifted back to the reactant side.

In the chromate-dichromate system results showed that chromate solution have yellow color while for dichromate have orange color and when base is added chromate remained yellow but the dichromate from orange to yellow. And when an acid was added chromate turned orange while...
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