A solution is made by dissolving 32g KCIO3 in 100g H20 at 80C. The solution is cooled to 10C. Describe what you would observe as it cooled and state what temperature this first occurs at. What mass of crystals would settle out of the solution?
I don't know many who have the solubility tables of thousands of chemicals memorized. I know I don't. Surely you have a table that lists the solubility of KClO3 at 80 C and 10 C. Or perhaps it's a graph that gives those numbers. If you will post those perhaps we can help.
To understand what would happen as the solution cools, we need to examine the concept of solubility.
Solubility is the ability of a substance to dissolve in a given solvent at a specific temperature. In this case, we have a solution made by dissolving 32g of KCIO3 in 100g of H2O at 80°C. At this temperature, KCIO3 is fully dissolved in water, as it exceeds its solubility limit.
As the solution cools, the solubility of KCIO3 in water decreases. When the temperature reaches a point where the solubility of KCIO3 is lower than the amount dissolved, it will start to precipitate out of the solution in the form of crystals.
The temperature at which the first appearance of crystals occurs is known as the saturation temperature. To determine this temperature, we need to examine the solubility curve for KCIO3 in water.
The solubility curve represents the relationship between solubility and temperature. In this case, let's assume that KCIO3 follows a solubility curve where solubility increases with temperature. This means that as the temperature decreases, the solubility of KCIO3 also decreases.
Now, we need to find the saturation temperature at which the solubility of KCIO3 is equal to the amount currently dissolved, i.e., 32g. We can look at the solubility curve to determine this point. Let's assume that the saturation temperature is 50°C.
As the solution continues to cool below the saturation temperature, more KCIO3 will precipitate out of the solution as crystals. To calculate the mass of crystals that settle out, we need to know the solubility of KCIO3 at 10°C.
Let's assume that at 10°C, the solubility of KCIO3 is 10g per 100g of water (hypothetical value). This means that at this temperature, only 10g of KCIO3 can remain dissolved in 100g of water, while 22g (32g - 10g) will form crystals and settle out.
To summarize, as the solution cools from 80°C to 10°C, the first appearance of crystals (saturation temperature) occurs at 50°C (hypothetical value). And when the solution reaches 10°C, 22g of KCIO3 will settle out of the solution in the form of crystals.