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 need to use the solubility information provided.
At 0.33g/100ml, it means that at 25 degrees Celsius, 0.33g of the compound can dissolve in 100ml of water.
So, to find the amount of water required to dissolve 10g of the compound, we can set up a proportion:
0.33g / 100ml = 10g / x ml
Cross-multiplying the proportions:
0.33g * x ml = 10g * 100ml
Simplifying the equation:
0.33x = 1000
Dividing both sides by 0.33:
x = 1000 / 0.33
x ≈ 3030.3 ml
Therefore, approximately 3030.3 ml of water would be required to crystallize 10g of the compound at 25 degrees Celsius.
Now, to determine the maximum possible amount of the compound that can be collected when the pure compound is crystallized at 25 degrees Celsius, we will use the solubility information.
The solubility of the compound in water is 6.8g/100ml at 0 degrees Celsius. This means that at 0 degrees Celsius, 6.8g of the compound can dissolve in 100ml of water.
Since we are collecting the compound at 25 degrees Celsius, which is higher than the solubility temperature, the compound should fully crystallize out of the water.
Therefore, the maximum possible amount of the compound that can be collected when it is crystallized at 25 degrees Celsius is 10g, which is the initial amount we started with.