Calcium Chloride (CaCl2) is the chemical compound formed when calcium and chloride ions bond together, and it is a common style of de-icing salt. It is produced commercially in large quantities, and is a key component in many water treatment processes. It can also be used to make an aqueous solution with a specific concentration of CaCl2. In this article we will be examining how much water must be added to 40.0g of CaCl2 to produce a solution that is 35.0 wt% CaCl2.
To begin, it is important to understand the structure of the CaCl2 molecule. CaCl2 is an ionic compound, meaning it is composed of two separate ions. The CaCl2 molecule is formed when calcium and chloride ions bond together, forming one molecule with the formula of CaCl2. The mass of one molecule of CaCl2 is 111.0 g/mol, which is composed of 40.0 g of calcium and 71.0 g of chloride per mole.
Now that we understand the structure and mass of the CaCl2 molecule, we can use it to calculate how much water must be added to 40.0 g of CaCl2 to produce a solution that is 35.0 wt% CaCl2. To solve this equation, we must first convert the 35.0 wt% to a mass concentration. The mass concentration can be calculated by multiplying the mass of CaCl2 (40.0 g) by 0.35, which gives us 14.0 g of CaCl2.
Next, we can calculate the mass of water that needs to be added to the 40.0 g of CaCl2 to produce a solution with a mass concentration of 14.0 g of CaCl2. To do this, we can subtract the mass of CaCl2 from the mass of the original solution (40.0g – 14.0g = 26.0g). Thus, we can conclude that 26.0 g of water must be added to 40.0 g of CaCl2 to produce a solution that is 35.0 wt% CaCl2.
In conclusion, to produce a solution of 35.0 wt% CaCl2, we must add 26.0 g of water to 40.0 g of CaCl2. This equation can be used to calculate the amount of water needed to make any solution with any desired wt% of CaCl2.