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 sol

Question

bekas

3 months ago

9

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 sol

ution formed?

Chemistry

2 answers:

Anarel [2.9K] · Answer 1 · 2026-02-27T19:08:54+03:00

Explanation:

Molarity is calculated by dividing the number of moles by the volume in liters. The number of moles can be derived from the given mass divided by the molar mass.

In this case, we have a molarity of 0.680 M, a mass of 55.0 g, and the molar mass for $Ca(OH)_{2}$ listed as 74.093 g/mol.

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

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

= 1.091 L

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

castortr0y [3K] · Answer 2 · 2026-02-27T19:10:47+03:00

Convert 55.0g Ca(OH)2 to moles.

The calculation shows that 55.0g of Ca(OH)2 corresponds to 0.742 moles.

To find the volume, divide 0.742 mol of Ca(OH)2 by its molarity of 0.680M, yielding approximately 1.09L of Ca(OH)2.

If you disregard the negligible volume of the Ca(OH)2 itself, the resulting total volume of a 0.680M solution created by dissolving 55.0g of Ca(OH)2 in an appropriate amount of water would be 1.09L.