Question

A 0.680 M Ca(OH)2 solution was prepared by dissolving 55.0 grams of Ca(OH)2 in enough water. What is the total volume of the solution formed?

Answer 1

Explanation:

Molarity is the number of moles divided by volume in liter. Whereas number of moles is equal to mass given divided by molar mass.

Mathematically,   $Molarity = \frac{mass}{molar mass \times volume}$

Since, it is given that molarity is 0.680 M, mass is 55.0 g and molar mass of $Ca(OH)_{2}$ is 74.093 g/mol.

Therefore, $Volume = \frac{mass}{molar mass \times Molarity}$

                                       = $\frac{55.0 g}{74.093 g/mol \times 0.680 mol L^{-1}}$

                                       = 1.091 L

Thus, we can conclude that total volume of the solution formed is 1.091 L.

Answer 2

Convert 55.0g Ca(OH)2 to mols.

55.0g Ca(OH)2 = 0.742 mols Ca(OH)2

0.742mol Ca(OH)2/ 0.680M Ca(OH)2 = 1.09L Ca(OH)2

Neglecting the volume of the Ca(OH)2 itself, since it is minimal and its density wasn't provided, 1.09L would be the total volume of a 0.680M solution produced by dissolving 55.0g of Ca(OH)2 in enough water.