Question

Section: Name: Laboratory Questions: Solution Stoichiometry A solution is prepared by dissolving 3.7500 grams iron(III) oxalate in enough water to make 125.00 mL of solution. 1. What is the molar concentration of iron(III) oxalate in this solution? a. b. What is the molar concentration of oxalate ions in this solution? . Describe how prepare 250.00 mL of 0.150 M ammonium ion solution beginning with would you solid ammonium phosphate, (NH), PO

Answer 1

u Malarity = moles of solute litres of solution = mass of solute molar mais solule x Volume osobelion (L) = 3.75 g 375.747g/mol X 0.125L = 0.0798 M Fee (Ou); → 2 Fe3+ + 36207 has the abogadost from the reaction, molar.concentration of Fe3t = 2 [Fez (204)3 7 = 230.0 798M = 0.1596M molar concentration of 50 = 3 [Fe (204)] = 3x 0.0798M =0.2394M I Ans (a) 0.0798M (6) 0.2394M | 2 (NH4), PO 3 NH4 + POS- NH] = 3 [WHG) Pou] [(NH4), ply] = [NHH 1 - 0-150m . 3 3 = 0.05M (NH4), Роу mass of (NM, 1,80,- Molasiuly - x molar mass & Volume -0.05 MX 149.09g/mol X 0-250L = 1.8649

Dissolving 1.864 g (NH 4 ) Poy salt in a * 250 ml volumetric flask and making up the volume to 250 ml with water will give 0.05 m (NH 4 ) Poy solution land o. is om ammonium con solution