What is the molarity of a solution made when 11 g of CaCl2 is dissolved in 100 mL of solution?

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What is the molarity of a solution made when 11 g of CaCl2 is dissolved in 100 mL of solution?

To determine the molarity of a solution, it is essential to calculate the number of moles of solute (in this case, CaCl2) and then divide by the volume of the solution in liters. First, we need to find the molar mass of CaCl2. The molar mass can be calculated by summing the atomic masses of calcium (Ca) and chlorine (Cl). Calcium has an atomic mass of approximately 40.08 g/mol, while chlorine has an atomic mass of about 35.45 g/mol. Since there are two chlorine atoms in calcium chloride, we calculate the molar mass as follows: \[ \text{Molar mass of CaCl}_2 = 40.08 \, \text{g/mol} + (2 \times 35.45 \, \text{g/mol}) = 40.08 \, \text{g/mol} + 70.90 \, \text{g/mol} = 110.98 \, \text{g/mol} \] Next, we convert the mass of CaCl2 from grams to moles using its molar mass. Given that 11 g of CaCl2 is used, the number of m

To determine the molarity of a solution, it is essential to calculate the number of moles of solute (in this case, CaCl2) and then divide by the volume of the solution in liters.

First, we need to find the molar mass of CaCl2. The molar mass can be calculated by summing the atomic masses of calcium (Ca) and chlorine (Cl). Calcium has an atomic mass of approximately 40.08 g/mol, while chlorine has an atomic mass of about 35.45 g/mol. Since there are two chlorine atoms in calcium chloride, we calculate the molar mass as follows:

[

\text{Molar mass of CaCl}_2 = 40.08 , \text{g/mol} + (2 \times 35.45 , \text{g/mol}) = 40.08 , \text{g/mol} + 70.90 , \text{g/mol} = 110.98 , \text{g/mol}

]

Next, we convert the mass of CaCl2 from grams to moles using its molar mass. Given that 11 g of CaCl2 is used, the number of m

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