of the crucible because of oils on skin. During this experiment, the crucible was massed after the reaction had taken place and was cleaned improperly so there were still small remnants of AgCl precipitate. This would also affect the mass measurement the same as the oils from a hand. This would be classified as a humane error as it was a mistake that could have easily been avoided. When taking this measurement, the massing tool was not calibrated; therefore, it could have given incorrect readings. The second time that the crucible was to be weighed, it was not fully cooled; therefore, its mass measurement may have been affected because the metal parts in the analytical balance could expand and cause an incorrect reading. Lastly, there are the limitations of the measuring equipment that cannot be controlled by the chemists.
Araba 4 | 0.8345 − 0.925 | 0.925 x 100 = 8.81% DISCUSSION QUESTIONS Calculate the following: 1a. The amount of NaCl needed to precipitate all the silver in the sample. Assume the sample is 100% silver. Please refer to Calculations section. 1b. Calculate the percent silver in silver chloride. Record this value in the Data Table. 107.87 g Ag 143.32 g AgCl = 0.75265 (See Data Table) 1c. From the mass of filtered silver chloride and the mass of the silver alloy sample, calculate the mass of silver in the alloy. Record this value in the Data Table. 107.87 g Ag 143.32 g AgCl x 0.2836 g AgCl 1 = 0.2135 g Ag (See Data Table)
- Fall '16
- Sodium chloride, g Ag, AgCl