100g of a saturated solution of sodium nitrate at 43°C is cooled quickly with stirring to 10°C. How many grams of the solute will crystallize?
What's the solubility of NaNO3 in water at 10 C? You must have a chart or graph.
To find out how many grams of the solute will crystallize, we need to determine the solubility of sodium nitrate at both temperatures.
1. Determine the solubility of sodium nitrate at 43°C:
At 43°C, the solubility of sodium nitrate is 150g/100g of water.
2. Determine the solubility of sodium nitrate at 10°C:
At 10°C, the solubility of sodium nitrate is 40g/100g of water.
3. Calculate the difference in solubility between the two temperatures:
Δsolubility = solubility at 43°C - solubility at 10°C
Δsolubility = 150g/100g - 40g/100g
Δsolubility = 110g/100g
4. Calculate the amount of solute that will crystallize:
The difference in solubility represents the amount of solute that will crystallize when cooled.
Mass of solute crystallized = Δsolubility * mass of saturated solution
Mass of solute crystallized = 110g/100g * 100g
Mass of solute crystallized = 110g
Therefore, 110 grams of the solute (sodium nitrate) will crystallize when the saturated solution is cooled from 43°C to 10°C.
To determine how many grams of the solute will crystallize, we need to find out the solubility of sodium nitrate at both 43°C (initial temperature) and 10°C (final temperature). The solubility of a compound generally decreases as the temperature decreases.
First, we need to find the solubility of sodium nitrate at 43°C. This information can be found in solubility tables or databases. Let's assume that the solubility of sodium nitrate at 43°C is found to be 200g/100g of water.
Next, we need to find the solubility of sodium nitrate at 10°C. Again, referring to solubility tables or databases, let's assume the solubility at 10°C is 80g/100g of water.
The difference between the initial solubility (200g) and the final solubility (80g) gives us the maximum amount of sodium nitrate that will remain dissolved after cooling, which is 200g - 80g = 120g.
Since we started with a saturated solution containing 100g of sodium nitrate, we need to subtract the amount that remains dissolved to find the amount that will crystallize. Therefore, 100g - 120g = -20g.
Based on these calculations, it seems that more sodium nitrate will crystallize out than was originally dissolved. However, this is physically impossible. The negative value for the amount of solute indicates that the solution was actually supersaturated before cooling, and the excess sodium nitrate will precipitate out as crystals.
Therefore, 20g of sodium nitrate will crystallize out from the saturated solution.