1. How would using 0.42 g CH3CO2Na * 3H2O instead of the amount called for in the procedure change the theoretical yield of Fe(C5H7O2)3 = 3.53g.
2. When a student sees crystals form after she added a few drops of water to the filtrate. Need chemical formula of the crystals.
3. Why the addition of water to the filtrate causes the crystals to precipitate from the solution.
4. Why is it more efficient to examine a small portion of the filtrate rather than the entire solution, when checking to see if crystalization is complete.
5. Why is it better to wash the collected crystals with distilled water instead of water--methanol mixture.
Please help on these questions. Have no clue at all.
Can you explain how to calculate Q1?
1. To determine the change in theoretical yield of Fe(C5H7O2)3, we need to calculate the molar ratio between CH3CO2Na * 3H2O and Fe(C5H7O2)3, as well as the molar mass of CH3CO2Na * 3H2O and its actual mass used.
First, let's calculate the moles of CH3CO2Na * 3H2O by dividing the given mass by its molar mass:
moles = mass / molar mass
moles = 0.42 g / (molar mass of CH3CO2Na * 3H2O)
Next, we need to determine the moles of Fe(C5H7O2)3 using the given theoretical yield of 3.53 g and its molar mass:
moles = mass / molar mass
moles = 3.53 g / (molar mass of Fe(C5H7O2)3)
Then, we find the molar ratio between the two compounds by dividing the moles of Fe(C5H7O2)3 by the moles of CH3CO2Na * 3H2O.
Finally, we can calculate the new theoretical yield by multiplying the molar ratio by the moles of CH3CO2Na * 3H2O and the molar mass of Fe(C5H7O2)3.
2. To determine the chemical formula of the crystals formed when water is added to the filtrate, we would need more information about the substances involved. Without this information, it is not possible to provide a specific formula. However, you can use techniques like spectroscopy or chemical tests to identify the compounds in the filtrate and analyze the crystal structure to determine their chemical formula.
3. The addition of water to the filtrate causes the crystals to precipitate from the solution due to a change in solubility. When water is added, it increases the solvent's ability to dissolve the solute, reducing its solubility. As a result, the solute becomes less soluble and forms solid crystals, which can be observed in the solution.
4. It is more efficient to examine a small portion of the filtrate rather than the entire solution when checking for completion of crystallization because a small portion represents the overall composition of the solution. By examining a small sample, you can determine if crystals have formed and if the process of crystallization is complete without needing to analyze the entire solution, which could be time-consuming.
5. Washing the collected crystals with distilled water instead of a water-methanol mixture is preferable because distilled water is less likely to contain impurities that may interfere with the purity of the crystals. Methanol, on the other hand, may introduce additional compounds or contaminants that could affect the quality or composition of the crystals. By using distilled water, you can ensure a cleaner and more reliable wash, resulting in purer crystals.