Question

How many grams of Ca(OH)2 are needed to produce 600 ml of 1.22 M Ca(OH)2 solution?

Answer 1

Answer: 54.2 g Ca(OH)2

Explanation: Molarity is moles of solute / L solution

First convert mL to L

600 mL x 1L / 1000 mL = 0.6 L

Find moles of Ca(OH)2

n= M x L

= 1.22 M x 0.6 L

= 0.732 moles Ca(OH)2

Convert moles to mass using its molar mass of Ca( OH)2 = 74 g

0.732 moles Ca(OH)2 X 74 g Ca(OH)2 / 1 mole Ca(OH)2

= 54.2 g Ca(OH)2

Answer 2

54.2 g of Ca(OH)₂

Step-by-step explanation:

Let's determine the moles of solute, we should need

Molarity . volume (L) = moles

Let's convert 600 mL to L

600 mL/ 1000 = 0.6L

1.22 mol/L . 0.6L = 0.732 moles

Finally we must convert the moles to mass ( moles . molar mass)

0.732 mol . 74.08 g/mol = 54.2 g