High School

3.108 g of CaCl2 were added to 1.0 deciliter (dl) of water. Assuming the molecular weight (MW) of CaCl2 is 111 g/mol, answer the following questions:

A) What is the molarity of CaCl2 in the solution?
B) How many moles of CaCl2 were added to the water?
C) What is the volume of water in liters?
D) What is the mass of CaCl2 in the solution?

Answer :

Final answer:

The molarity of CaCl2 in the solution is 0.28 M. 0.028 moles of CaCl2 were added to the water. The mass of CaCl2 in the solution is 3.108 g.

Explanation:

To find the molarity of CaCl2 in the solution, we need to calculate the number of moles of CaCl2 and divide it by the volume of the solution in liters. The number of moles of CaCl2 can be found by dividing the mass of CaCl2 by its molar mass:

Moles of CaCl2 = (3.108 g / 111 g/mol) = 0.028 mol

Volume of water in liters = 1.0 deciliter = 0.1 liters

Therefore, the molarity of CaCl2 in the solution is:

Molarity = Moles of CaCl2 / Volume of solution = 0.028 mol / 0.1 L = 0.28 M

The moles of CaCl2 added to the water is 0.028 mol.

Mass of CaCl2 in the solution is 3.108 g.