Lab 2. The gravimetric determination of chloride in a soluble sample Introduction: For the experiment you will get an unknown sample, containing chloride ion, and you will perform the gravimetric procedure using the analyte sample. An analyte is a chemical constituent determined by analytical techniques. The technique used in the experiment is gravimetric determination analysis which is a quantitative chemical analysis method in which the key constituent sought is converted into a substance that can be separated from the remaining sample. A common method for determining chloride ions involves isolating the silver chloride precipitate by filtration, determining its mass, and using stoichiometry to calculate the percentage of chloride in an impure sample of unknown chloride. Since the unknown chloride is soluble in water, the percentage of chloride can be analyzed by adding an aqueous solution, silver nitrate, which can form a precipitate with the aqueous chloride. Experimental: to carry out this experiment we will have to obtain the necessary materials and chemicals. The materials needed to achieve are sintered glass filter crucibles (3), desiccator (a drying chamber that holds materials in the absence of air or in the presence of a drying agent), analytical balance, hot plate, aluminum foil, 400 ml glasses (3), vacuum filter flask, the waste container and turn on the laboratory convection oven at 110°C. The required chemicals: 3 grams of unknown impure analyte sample (chloride), 6M HNO3, concentrated HNO3, 6M NH3 (minimum 10 ml), 0.2 M AgNO3 (minimum 300 ml). Results: EquationsMean/mean (¯X) = (∑▒x)/nStandard deviation s= √((∑▒〖(x_i- x ̅)〗^2 ...... half of the document ...... general situations where the only suitable analytical technique is the gravimetric method. There were several sources of error in this experiment that must be considered other precipitates, causing inaccurate mass readings for the presumed silver chloride compound. Possible points of contamination could occur during handling of the compounds; if tap water was accidentally used (substances in the water could react with the nitrate silver); or other sources of error include decomposition caused by light would also produce low results. A possible source of error could be that the crucibles were not sufficiently cooled in the desiccators, which could also have affected the masses. of the AgCl samples..