solution was prepared by dissolving about 3.0 g of NaH2Y2·2H2O in approximately 1 L of water and standardizing it against 50.00-mL aliquots of 0.004423 M Mg2+. An average titration of 30.27 mL was required. Calculate the molar concentration of the EDTA

What is the full equation (not the net ionic equation) for the chemical reaction of 0.001 M Fe(NO3)3 plus 0.0002 M NaSCN diluted up to 10 mL with 0.1M HNO3? Please include the acid that is the diluent.

A weighed sample of sodium nitrite was treated with 0.05 mol of ceric sulfate in solution, in air-free conditions. The resulting solution was titrated with standard Fe(II) solution and 0.01 mol of Fe(II) were required. Determine the moles of sodium nitrite present in the weighed sample.  NO2– + 2 Ce4+ + H2O → NO3– + 2 Ce3+ + 2 H+ Fe2+ + Ce4+→ Fe3+ + Ce3+

1.  A 0.9882 gram sample of iron ore is dissolved, the iron reduced to Fe2+, and the solution was titrated with 36.40 mL of 0.02065 M KMnO4 in acid solution. (a)  Write the titration reaction.  (b)  Calculate the %FeO (M.M. = 71.85) in the sample.   2.  A sample of primary standard grade K2Cr2O7 (MM = 294.20) weighing 0.2153 g is dissolved, the solution acidified and excess KI added. The liberated I2 requires 44.86 mL of the Na2S2O3 for titration. (a)  Write the titration reaction.  (b)  Calculate the molarity of the titrant solution.    Box the final answer.