A chemist prepares a solution of iron(II) bromide (FeBr2) by measuring out 46. g of iron(II) bromide into a 400. mL volumetric flask and filling the flask to the mark with water.
Calculate the concentration in mol/L of the chemist's iron(II) bromide solution. Round your answer to 2 significant digits.

Solution

Given mass of FeBr2 = 85.5 g

Molar mass of FeBr2 = 215.65

No. of Moles of FeBr2 = Given Mass / Molar mass = 85.5 / 215.65

No. of Moles = 0.3964

Given Volume is 450 mL i.e. 0.450 L

Now Concentration = 0.3964/0.450

Hence Concentration = 0.881 mol/L

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

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