Antimony Trichloride Reaction Lab Report

Le Châtelier's principle was observed through different reactions during which different elements of the reaction were changed. The investigation began by observing the reaction of antimony trichloride solution and distilled water. Then, the reaction was observed as more distilled water was added in increments of 4.00 mL until of total volume of 16.02 mL was added to the initial 5.00 mL of SbCl3 solution. Additionally, the hydrolysis of antimony trichloride was completed by adding 12.72 mL of water until a white cloud persisted throughout the solution. Another reaction was observed which was between iron (III) nitrate and sodium thiocyanate to form the iron (III) thiocyanate ion. The resulting solution was then split into four test tubes which either had Fe(NO3)3, NaSCN, and NaH2PO4 added to them. Finally, the enthalpy of the reaction was evaluated by

Also, the boiling water test tube and ice bath test tube were switched to see if any additional shifts would take place.
As water was added to the SbCl3 solution, a white cloud formed and as more water was added a white precipitate formed when the white cloud persisted. When HCl was added, the SbCl3 became clear again indicating, the reaction had reversed. Earlier, prior to reaching equilibrium, the solution would become cloudy and revert to its original state. Therefore, as HCl was added, a shift occurred. Additionally, the equilibrium for the reaction was determined to be 92. After iron (III) thiocyanate was formed and separated into four separate test tubes, one control and three with additional components, shifts had occurred in each of the three experimental test tubes. When 0.02 M Fe(NO3)3 was added, the solution changed from a reddish-orange color to a deep, dark red indicating a shift to the right or to the products, while 0.02 M NaSCN was added to another test tube, it simply became about one shade lighter but should have