Question
In: Chemistry
A solution is prepared by dissolving 12.36 g of CaCl2 ( an electrolyte, molar mass= 111g)...
A solution is prepared by dissolving 12.36 g of CaCl2 ( an electrolyte, molar mass= 111g) in 135g of H2O ( molar mass =18.0g). The resulting solution has a density of 1.10 g/ml. Calculate the molarity of CaCl2 in the solution.
Solutions
Expert Solution
Total mass = 12.36 g + 135 g = 147.36 g
density = mass / volume
1.10 g/ml = 147.36 / volume
volume = 134 mL
= 0.134 L
mass of CaCl2 = 12.36 g
Molar mass of CaCl2 = 111 g
number of moles of CaCl2 = mass / molar mass
= 12.36/111
= 0.114 mol
V = 0.134 L
M = number of moles / volume
= 0.114 / 0.134
= 0.83 M
Answer: 0.83 M
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