Answer :
To answer this question, we need to interpret the solubility graph for NH4Cl (ammonium chloride). A solubility graph shows the relationship between temperature and the maximum amount of solute that can dissolve in 100 grams of water at various temperatures.
Given that we have a 100g sample of water and at 80°C it dissolves 30g of NH4Cl, we need to determine whether this amount corresponds to a point on the curve (saturated), below the curve (unsaturated), or above the curve (supersaturated) for NH4Cl on the graph.
Using the solubility graph provided (though not physically present in this interaction), follow these steps to determine the solution state:
1. Locate 80°C on the x-axis (Temperature °C) of the solubility graph.
2. From 80°C, move directly upwards until you intersect the curve for NH4Cl.
3. At the point of intersection, move horizontally to the y-axis to find the maximum grams of NH4Cl that can be dissolved in 100g of water at 80°C.
Since we don't have the actual solubility graph in front of us, we will need to rely on typical solubility behavior inferred from solubility trends. Normally:
- If the maximum grams dissolvable at 80°C is less than 30g, then 30g would exceed the solubility limit, indicating a supersaturated solution.
- If the maximum grams dissolvable at 80°C is exactly 30g, then the solution would be at its solubility limit, indicating a saturated solution.
- If the maximum grams dissolvable at 80°C is more than 30g, then 30g does not exceed the solubility limit, indicating an unsaturated solution.
In general, if a solution contains less solute than the maximum solubility at a given temperature, it is unsaturated. If it contains the maximum amount, it's saturated. And if it contains more, it is supersaturated, typically forming after a solution has been heated to a higher temperature to dissolve more solute, then carefully cooled down.
Since you've stated that a 100g sample of water dissolves 30g of NH4Cl at 80°C, you would look on the graph to see where 30g falls relative to the NH4Cl curve at 80°C. Without the actual graph, I can't give you a specific answer, but you'd follow the steps outlined above to determine the correct state of the solution: unsaturated (A), saturated (B), or supersaturated (C).
Given that we have a 100g sample of water and at 80°C it dissolves 30g of NH4Cl, we need to determine whether this amount corresponds to a point on the curve (saturated), below the curve (unsaturated), or above the curve (supersaturated) for NH4Cl on the graph.
Using the solubility graph provided (though not physically present in this interaction), follow these steps to determine the solution state:
1. Locate 80°C on the x-axis (Temperature °C) of the solubility graph.
2. From 80°C, move directly upwards until you intersect the curve for NH4Cl.
3. At the point of intersection, move horizontally to the y-axis to find the maximum grams of NH4Cl that can be dissolved in 100g of water at 80°C.
Since we don't have the actual solubility graph in front of us, we will need to rely on typical solubility behavior inferred from solubility trends. Normally:
- If the maximum grams dissolvable at 80°C is less than 30g, then 30g would exceed the solubility limit, indicating a supersaturated solution.
- If the maximum grams dissolvable at 80°C is exactly 30g, then the solution would be at its solubility limit, indicating a saturated solution.
- If the maximum grams dissolvable at 80°C is more than 30g, then 30g does not exceed the solubility limit, indicating an unsaturated solution.
In general, if a solution contains less solute than the maximum solubility at a given temperature, it is unsaturated. If it contains the maximum amount, it's saturated. And if it contains more, it is supersaturated, typically forming after a solution has been heated to a higher temperature to dissolve more solute, then carefully cooled down.
Since you've stated that a 100g sample of water dissolves 30g of NH4Cl at 80°C, you would look on the graph to see where 30g falls relative to the NH4Cl curve at 80°C. Without the actual graph, I can't give you a specific answer, but you'd follow the steps outlined above to determine the correct state of the solution: unsaturated (A), saturated (B), or supersaturated (C).
