**Educational Content on Gravimetric Analysis****Discussion Questions**1. **Gravimetric Analysis in Routine Monitoring:** - **(a)** Gravimetric analysis is highly effective for monitoring ions at relatively high concentrations. However, it is not suitable for determining trace amounts of ions. This limitation arises because gravimetric methods require sufficient quantities of the analyte to form a measurable precipitate. In trace scenarios, the amount of analyte may be too small to form a detectable precipitate, thus affecting accuracy and precision. - **(b)** Sources of error in gravimetric analysis can include incomplete precipitation, impurities in the precipitate, loss of precipitate during handling, or issues with the drying process. Each of these factors can lead to discrepancies between the observed and actual values.2. **Analysis of Unknown Chloride Sample:** - From a sample weighing 0.323 g of an unknown chloride (represented as \( M_xCl_y \)), 0.523 g of silver chloride (\( \text{AgCl(s)} \)) solid is obtained through gravimetric analysis. The task is to determine the percentage of chlorine in the unknown sample and infer the theoretical molar weight of the metal in the chlorite salt sample \( M_xCl_y \) based on the conditions: - **a.** \( x = 1, y = 1 \) - **b.** \( x = 1, y = 2 \) - **c.** \( x = 2, y = 4 \) **Note:** This problem requires a detailed numerical analysis using the molecular weights of the elements involved and the stoichiometry dictated by the chemical formulas provided.

Since you have asked multiple questions, we will answer the first one for you. To get the remaining question solved please repost stating the question you want us to solve.Gravimetric analysis is used to quantitatively analyze the constituent analyte present in a sample by converting it into a substance that can be easily separated rom the sample. a) Trace amount of ions are present in very small amount in the sample. Since gravimetric analysis is based upon weighing to obtain the mass, the amount of precipitate formed by trace amount of ions is very small which is difficult to be accurately weighed and separated and thus, is not very well determined using gravimetric analysis. b) Sources of error: 1) Decomposition of precipitate under light which can affect the amount of precipitate weighed. 2) Directly weighing the precipitate from the hot crucible. If the precipitate is not weighed before properly cooling down, it would provide a smaller than actual yield. 3) Weighing the precipitate before being completely dried. It would give more than actual yield of the precipitate due to excess water.