Without all of the question it is impossible to answer any but the first part.
25.00 mL aliquots of the solution from Part 1 are titrated with EDTA to the Eriochrome Black T end point. A blank containing a small measured amount of Mg2+ requires 2.60 mL of the EDTA to reach the end point. An aliquot to which the same amount of Mg2+ is added requires 28.55 mL of the EDTA to reach the end point.
How many milliliters of EDTA are needed to titrate the Ca+2 ion in the aliquot?
28.55-2.60 = ??
How many moles of EDTA are there in the volume obtained in the previous question?
moles EDTA in 100 mL x 10 = moles EDTA in 1 L.
What is the molarity of the EDTA solution?
25.00 mL aliquots of the solution from Part 1 are titrated with EDTA to the Eriochrome Black T end point. A blank containing a small measured amount of Mg2+ requires 2.60 mL of the EDTA to reach the end point. An aliquot to which the same amount of Mg2+ is added requires 28.55 mL of the EDTA to reach the end point.
How many milliliters of EDTA are needed to titrate the Ca+2 ion in the aliquot?
How many moles of EDTA are there in the volume obtained in the previous question?
What is the molarity of the EDTA solution?
1 answer