Silver Chloride Lab Report
Purpose: The Purpose of this lab is to utilize, demonstrate and understand the various techniques and procedures used to gravimetric labs. For this particular lab we will utilize our scientific knowledge of related to gravimetric procedures to find the chloride content in an unknown soluble salt.
Theory: Using our developed knowledge of the conservation of mass, solubility and precipitation it is possible (with some degree of error) to know the content of chlorine in a particular salt by dissolving it in water, than extracting it through precipitation. This method is based on quantitative isolation of pure chlorine on both sides of the compound which we can achieve if enough data is available for calculation. We know that our dissolved unknown salt contains chlorine, a halide, which can be precipitated effectively using silver nitrate. The positive Silver ions in the Silver nitrate ions react with the chlorine in in this net ionic reaction:
Ag+(aq) + Cl-(aq) = AgCl(aq)
Silver Chloride is an extremely insoluble compound, as it has a Ksp constant of 1.6 * 10-10 which means the reverse reaction of the Silver Chloride dissolving …show more content…
In hindsight there were phases of the lab where we forgot to put our precipitate in the drawer enabling the precipitate to decompose and ultimately loose mass. We also could have been a tad more cautious when handing the precipitate as the solid separated into smaller sup unit which increased the surface area enabling the photodecomposition of the precipitate to occur more dramatically. We also added our precipitating agent to the supernatant solution too quickly, making all the chlorine unable to bond with the Ag+ as other, smaller ions co-precipitate instead. The precipitate may not have undergone a complete reaction as our test for more precipitate was not as thorough as it could have
Theory: Using our developed knowledge of the conservation of mass, solubility and precipitation it is possible (with some degree of error) to know the content of chlorine in a particular salt by dissolving it in water, than extracting it through precipitation. This method is based on quantitative isolation of pure chlorine on both sides of the compound which we can achieve if enough data is available for calculation. We know that our dissolved unknown salt contains chlorine, a halide, which can be precipitated effectively using silver nitrate. The positive Silver ions in the Silver nitrate ions react with the chlorine in in this net ionic reaction:
Ag+(aq) + Cl-(aq) = AgCl(aq)
Silver Chloride is an extremely insoluble compound, as it has a Ksp constant of 1.6 * 10-10 which means the reverse reaction of the Silver Chloride dissolving …show more content…
In hindsight there were phases of the lab where we forgot to put our precipitate in the drawer enabling the precipitate to decompose and ultimately loose mass. We also could have been a tad more cautious when handing the precipitate as the solid separated into smaller sup unit which increased the surface area enabling the photodecomposition of the precipitate to occur more dramatically. We also added our precipitating agent to the supernatant solution too quickly, making all the chlorine unable to bond with the Ag+ as other, smaller ions co-precipitate instead. The precipitate may not have undergone a complete reaction as our test for more precipitate was not as thorough as it could have