A saturated solution of NH4Cl was made using 500g of water at 90 degrees. the solution was cooled to 50 degrees. what mass of NH4Cl was crystallized
To determine the mass of NH4Cl that was crystallized, we need to calculate the change in solubility of NH4Cl as the temperature decreases.
The solubility of most solid solutes increases as the temperature of the solvent (in this case, water) increases. This means that as the temperature drops, the solubility of NH4Cl decreases, leading to the formation of crystals.
To start, we need to find the amount of NH4Cl that can be dissolved in 500g of water at 90 degrees. This is the maximum amount of NH4Cl that can be held in the solution before it becomes saturated.
The solubility of NH4Cl at 90 degrees is typically given in grams of NH4Cl per 100 grams of water. Let's assume that at 90 degrees, the solubility of NH4Cl is 50g/100g of water.
So, the amount of NH4Cl that can be dissolved in 500g of water at 90 degrees can be calculated as follows:
(500g water) * (50g NH4Cl / 100g water) = 250g NH4Cl
Now, we have a saturated solution of NH4Cl with 250g of NH4Cl in 500g of water at 90 degrees.
Next, we need to find the new solubility of NH4Cl at 50 degrees. Let's assume that at 50 degrees, the solubility of NH4Cl is 25g/100g of water.
To determine how much NH4Cl will crystallize out of the solution when cooled to 50 degrees, we need to find the difference between the amount dissolved at 90 degrees and the amount that can be dissolved at 50 degrees.
(250g NH4Cl) - (500g water) * (25g NH4Cl / 100g water) = 125g of NH4Cl
Therefore, 125g of NH4Cl will crystallize out of the solution when it is cooled from 90 degrees to 50 degrees.
hint:
According to
https://en.wikipedia.org/wiki/Solubility_table
The solubility of ammonium chloride is 51.4 and 71.2 at temperatures 50°C and 90°C respectively.
"Solubility" used in the above article is expressed in "grams per 100 milliliters of water (g/100 ml)"