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
This makes no sense to me: The solubility of a compound in water is 6.8g/100ml at 0.33g/100ml
They don't even know book self can you imagine
To calculate the amount of water required to crystallize 10g of the compound, we need to consider the solubility of the compound in water at 25 degrees Celsius.
Given that the solubility of the compound is 0.33g/100ml at 25 degrees Celsius, and we want to crystallize 10g of the compound, we can set up a proportion:
0.33g / 100ml = 10g / X ml
Cross-multiplying and solving for X, we get:
X = (10g * 100ml) / 0.33g
X ≈ 3030.30 ml
Therefore, you would need approximately 3030.30 ml of water to crystallize 10g of the compound.
Now, to determine the maximum possible amount of the compound that can be collected at 25 degrees Celsius, we need to know the volume of the solution used for crystallization. If we assume it is the same as the amount of water used, which is 3030.30 ml, we can calculate it using the solubility of the compound at this temperature.
The solubility of the compound is given as 6.8g/100ml at 25 degrees Celsius. Using the volume of the solution (3030.30 ml), we can set up another proportion:
6.8g / 100ml = X g / 3030.30 ml
Solving for X:
X = (6.8g * 3030.30 ml) / 100ml
X ≈ 206.21 g
Therefore, the maximum possible amount of the compound that can be collected at 25 degrees Celsius is approximately 206.21 g.
To calculate the amount of water required to crystallize 10g of the compound, we need to use the solubility data given.
First, let's find out the amount of water needed to dissolve 1g of the compound. We can set up a proportion:
(6.8g compound / 100ml water) = (1g compound / x ml of water)
Cross-multiplying, we get:
6.8g * x ml of water = 1g * 100ml of water
Simplifying, we find:
x ml of water = (1g * 100ml of water) / 6.8g
x ml of water ≈ 14.71 ml of water
This tells us that 1g of the compound requires approximately 14.71 ml of water to dissolve.
To find the amount of water required to dissolve 10g of the compound, we can multiply the result by 10:
10g compound * 14.71 ml of water = 147.1 ml of water
Therefore, approximately 147.1 ml of water is required to crystallize 10g of the compound.
Now, to calculate the maximum possible amount of the pure compound that can be collected at 25 degrees Celsius, we need to compare the actual amount dissolved in water to the solubility at that temperature.
The solubility is given as 0.33g/100ml at 25 degrees Celsius. This means that 100 ml of water can dissolve 0.33g of the compound at this temperature.
Using this information, we can calculate the maximum possible amount of the pure compound that can be collected. We can set up another proportion:
(0.33g compound / 100ml water) = (xg compound / 147.1ml of water)
Cross-multiplying, we get:
0.33g * 147.1ml of water = xg * 100ml of water
Simplifying, we find:
xg = (0.33g * 147.1ml of water) / 100ml of water
xg ≈ 0.485g
Therefore, the maximum possible amount of the pure compound that can be collected at 25 degrees Celsius is approximately 0.485g.