given 3.650 l of a 1.75 M solution, what mass of calcium chloride is needed to prepare?
To determine the mass of calcium chloride needed to prepare the given solution, we need to use the provided information about the volume and concentration of the solution.
1. The concentration of the solution is stated as 1.75 M, which stands for 1.75 moles per liter.
2. The volume of the solution is given as 3.650 liters.
To find the number of moles of the solute (calcium chloride) present in the solution, we multiply the volume in liters by the molarity:
Number of moles = volume (liters) × molarity
Number of moles = 3.650 L × 1.75 mol/L
Now we can calculate the mass of calcium chloride using its molar mass. The molar mass of calcium chloride (CaCl2) can be obtained from the periodic table:
- The molar mass of calcium (Ca) is approximately 40.08 g/mol.
- The molar mass of chlorine (Cl) is approximately 35.45 g/mol.
Since calcium chloride (CaCl2) has one calcium atom and two chlorine atoms, its molar mass is:
Molar mass of CaCl2 = (1 × molar mass of Ca) + (2 × molar mass of Cl)
Molar mass of CaCl2 = (1 × 40.08 g/mol) + (2 × 35.45 g/mol)
Now we can calculate the mass of calcium chloride:
Mass of calcium chloride = Number of moles × Molar mass of CaCl2
Finally, substitute the values into the equation:
Mass of calcium chloride = (3.650 L × 1.75 mol/L) × [(1 × 40.08 g/mol) + (2 × 35.45 g/mol)]
Calculating this expression will give you the mass of calcium chloride needed to prepare the given solution.