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 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)

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