Question

In a group assignment, students are required to fill 10 beakers with 0. 720 M CaCl2. If the molar mass of CaCl2 is 110. 98 g/mol and each beaker must have 250. ML of solution, what mass of CaCl2 would be used? Use Molarity equals StartFraction moles of solute over liters of solution EndFraction. 3. 13 g 38. 5 g 200 g 617 g.

Answer 1

The mass of calcium chloride required in the solution has been 200 g. Thus, option C is correct.

Molarity has been defined as the mole of solute in a liter of solution. Molarity has been expressed as:

$\rm Molarity=\dfrac{Mass}{Molar\;mass}\;\times\;\dfrac{1}{Volume\;L}$

Computation for the mass of Calcium chloride

The given number of beakers has been 10.

The volume of a beaker has been 250 mL. The total volume of the solution in 10 beakers has been 2500 mL.

The given molarity of the solution has been 0. 72 M.

The mass of calcium chloride has been given by substituting the values as:

$\rm 0. 72=\dfrac{Mass}{110. 98} \;\times\;\dfrac{1}{2.5}\\ Mass=200 \;g$

The mass of calcium chloride required in the solution has been 200 g. Thus, option C is correct.

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