What would be the resulting molarity of a solution made by dissolving 31.3 grams of Ca (OH) 2 in enough water to make a 1050-milliliter solution? Show all of the work needed to solve this problem.

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Chemistry

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30 December, 21:16

What would be the resulting molarity of a solution made by dissolving 31.3 grams of Ca (OH) 2 in enough water to make a 1050-milliliter solution? Show all of the work needed to solve this problem.

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Willow Williamson · Answer 1

1) Calculate number of moles of Ca (OH) 2

1 mole = 40.1 + 2 (16.0) + 2 (1.0) = 74.1 g

31.3 g x 1 mol / 74.1 g = 0.422 mol

2) Calculate molarity

0.422 mol / 1.05 L = 0.402 M

P. S. This isn't a very practical problem, because 31.3 g of Ca (OH) 2 wont actually dissolve in 1050 mL of solution. Its solubility is low.