Can 2.38g of Magnesium Hydroxide be used to make up 100mL of solution

A student uses 2.38g of magnesium hydroxide to make up 100mL of solution. What is the molar concentration of the solution? Is this possible, why or why not?

There's no way you can dissolve 2.38 g of Mg(OH)2 in 100 mL of water. You'd be lucky to dissolve 1 mg! If you COULD do it,

2.38 g Mg(OH)2 x (1 mole Mg(OH)2 / 58.3 g Mg(OH)2) = 0.0408 moles Mg(OH)2

Molarity Mg(OH)2 = 0.0408 moles / 0.100 L = 0.408 M