A saturated solution at 25 C contains 10g of kclo3 in 50 ml of water. At what temperature does the solution become unsaturated?
You must have a graph or tabular data that gives you the solubility of KClO3 at various temperatures. I don't have all of the soubilities for all of the salts memorized.
To determine the temperature at which the solution becomes unsaturated, we need to consider the solubility of potassium chlorate (KClO3) in water at different temperatures. The solubility of a substance usually increases with temperature, meaning higher temperatures can dissolve more solute.
To find the solubility of KClO3 at different temperatures, we can refer to a solubility graph, a table, or other sources. However, I'll provide the known solubility data for KClO3 so you can calculate it yourself.
Solubility of KClO3 at 25°C is 40 g/100 mL (or 0.4 g/mL).
To find the temperature at which the solution becomes unsaturated, we can use the solubility data. First, we need to calculate how much KClO3 can dissolve in 50 mL of water at 25°C.
Since the solubility of KClO3 at 25°C is 0.4 g/mL, the maximum amount that can dissolve in 50 mL is:
0.4 g/mL * 50 mL = 20 g.
Given that the solution at 25°C contains only 10 g of KClO3, which is less than the maximum amount that can dissolve at that temperature, the solution is still saturated at 25°C.
To determine the temperature at which the solution becomes unsaturated, we need to find the temperature at which the solubility of KClO3 is equal to 10 g in 50 mL.
Let's assume the solubility of KClO3 at the unsaturation temperature is x g/mL.
We can set up a proportion to find x:
0.4 g/mL / 25°C = x g/mL / T°C,
where T represents the temperature at which the solution becomes unsaturated.
Cross-multiplying:
0.4 g/mL * T°C = x g/mL * 25°C.
To solve for T, let's substitute the given values:
0.4 g/mL * T°C = 10 g * 25°C.
Now, we can solve for T:
T°C = (10 g * 25°C) / 0.4 g/mL.
T°C = 250°C / 0.4 g/mL.
T°C = 625°C.
Therefore, the solution becomes unsaturated at a temperature of 625°C.