The solubility of a compound in water is 6.8g/100ml at 0.33g/100ml at 25 degree celsius. Calculate the amount of water required to crystallise 10g of the compound. If the pure compound is collected at 25 degree celsius, what is the maximum possible
To calculate the amount of water required to crystallize 10g of the compound, we first need to find the solubility of the compound in water at 25 degrees Celsius. We are given that the solubility is 0.33g/100ml at this temperature.
The solubility of the compound is given in grams per 100ml of water. So to convert this to grams per milliliter, we divide the given solubility by 100:
0.33g/100ml = 0.0033g/ml
Next, we can calculate the amount of water required to dissolve 10g of the compound using the following formula:
Amount of water (ml) = (Mass of compound (g) / Solubility (g/ml))
Substituting the values:
Amount of water (ml) = 10g / 0.0033g/ml ≈ 3030.3 ml
Therefore, approximately 3030.3 milliliters of water are required to dissolve 10 grams of the compound at 25 degrees Celsius.
As for the maximum possible amount of the pure compound collected, it depends on how much of the compound is dissolved in the given amount of water. Since the solubility at 25 degrees Celsius is 0.33g/100ml, the maximum possible amount of the pure compound that can be collected is 0.33g for every 100ml of water. This means that for every 100ml of the solution, only 0.33g of the compound can be collected as the maximum yield.