A chemist prepares a solution of iron(III) bromide (FeBr,) by weighing out 152.1 g of iron(III) bromide into a 250. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in g/dL of the chemist's iron(III) bromide solution. Be sure your answer has the correct number of significant digits. dL

A chemist must dilute 42.4 mL of 483. mM aqueous potassium dichromate (K,Cr,O,) solution until the concentration falls to 380. mM . He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Round your answer to 3 significant digits. mL ala

A solution is made by mixing 5.40 g of toluene, CH8(1), with 954. mL of chloroform, CHCI3(1). Calculate the concentration of the solute in the solution using the units given below. (Density of = 0.867 g/mL. Density of chloroform = 1.49 g/mL. Assume volumes mix additively.) toluene Enter your answers in decimal form to 3 significant figures. Do not enter units since they are already provided. Molar: molal: m mole fraction: mass percent: %(m/m) percent volume: %(v/v)

A chemist prepares a solution of iron(II) bromide (FeBr,) by measuring out 63. g of iron(II) bromide into a 150. 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.