SUPER CONFUSED please hppp
How many grams of solid Calcium Chloride (CaCl2) need to be added to 0.247 liters of a 0.5 M Calcium Chloride solution to raise the Molarity to 1.2?

The answer to your question is 19.19 g of CaCl₂

Explanation:

Data

mass of CaCl₂ = ?

volume = 0.247 l

[CaCl₂] 1 = 0.5 M

[CaCl₂] 2 = 1.2 M

Process

1.- Calculate the moles of CaCl₂ in the solution 1.2 M

Molarity = moles / volume

-Solve for moles

moles = Molarity x volume

-Substitution

moles = 1.2 x 0.247

moles = 0.2964

2.- Calculate the molar mass of CaCl₂

CaCl₂ = 40 + (35.5 x 2)

          = 40 + 71

          = 111 g

3.- Convert the moles to grams

                           111 g       1 mol

                              x       0.2964 mol

                     x = (0.2964 x 111)/1

                     x = 32.9 g

4.- Calculate the moles of the 0.5 M solution

moles = Molarity x volume

          = 0.5 x 0.247

          = 0.1235

-Convert to grams

                           111 g       1 mol

                             x         0.1235 moles

                             x = (0.1235 x 111) / 1

                             x = 13.7085

5.- Subtract the grams to find the mass needed.

     Mass = 32.9 - 13.7085

               = 19.19 g of CaCl₂

6.- Conclusion

We need to add 19.19 g of CaCl₂ to raise the concentration to 1.2.

hey there!

boiling point is the temperature at which the vapor pressure of the liquid equals atmospheric pressure. the vapor pressure of solvent molecules is decreased when a solute is added, so a higher temperature is required to increase the number of solvent molecules in the gas phase above the liquid.

at the freezing point, the vapor pressures of the solid and liquid are equal; a lower temperature is needed to reduce the number of solvent particles above the liquid.

hope this you

tobey