You need to make an aqueous solution of 0.187 M nickel(II) iodide for an experiment in lab, using a 300 mL volumetric flask. How much solid nickel(II) iodide should you add?

17.53 g

Explanation:

The chemical formula of nickel (II) iodide is NiI₂. Its molar mass (MM) can be calculated from the molar mass of its chemical elements:

MM(NiI₂) = 58.7 g/mol + (2 x 126.9 g/mol)= 312.5 g/mol

Given the following data:

M = 0.187 M = 0.187 mol/L

V= 300 mL = 0.3 L

We calculate the mass of NiI₂ as the product of the molarity of the solution (M), the molar mass (MM) and the volume:

mass = M x MM x V = (312.5 g/mol) x (0.187 mol/L) x 0.3 L = 17.53 g

Therefore, we have to add 17.53 grams of solid nickel(II) iodideto prepare the solution.

i believe the answer is three water molecules