A 0.530 M Ca (OH) 2 solution was prepared by dissolving 36.0 grams of Ca (OH) 2 in enough water. What is the total volume of the solution thus formed?

0.720 liters

0.917 liters

1.03 liters

1.21 liters

The concentration of a solution is the number of moles of solute per fixed volume of solution.

Concentration (C) = number of moles of solute (n) / volume of the solution (v)

we have to find the volume of the solution when 36.0 g of Ca (OH) ₂ is added to water to make a solution of concentration 0.530 M

mass of Ca (OH) ₂ added - 36.0 g

number of moles of Ca (OH) ₂ - 36.0 g / 74.1 g/mol = 0.486 mol

we know the concentration of the solution prepared and the number of moles of Ca (OH) ₂ added, substituting these values in the above equation, we can find the volume of the solution

C = n/v

0.530 mol/L = 0.486 mol / V

V = 0.917 L

answer is 0.917 L

The total volume of the solution is 0.917 liters (option 2)

Explanation:

Step 1: Data given

Molarity of Ca (OH) 2 = 0.530 M

Mass of Ca (OH) 2 = 36.0 grams

Molar mass of Ca (OH) 2 = 74.09 g/mol

Step 2: Calculate moles Ca (OH) 2

Moles Ca (OH) 2 = mass Ca (OH) 2 / molar mass Ca (OH) 2

Moles Ca (OH) 2 = 36.0 grams / 74.09 g/mol

Moles Ca (OH) 2 = 0.486 moles

Step 3: Calculate volume

Molarity = moles / volume

Volume = moles / molarity

Volume = 0.486 moles / 0.530 M

Volume = 0.917 L

The total volume of the solution is 0.917 liters (option 2)