A 25.00 mL solution was prepared by dissolving CaCO3 solid. It required 24.25 mL of a standard 0.02 M EDTA (ethylenediaminetetraacetic acid) solution to titrate the Ca2+ ions to the end point. (moles= 4.85 * 10^-4) a. How many moles of EDTA are contained in the 24.25 mL used for tritration. b. How many moles of CaCO3 were used? c. What is the concentration (molarity) of Ca2+ in the 25.00 mL of solution?

A 25.00 mL solution was prepared by dissolving CaCO3 solid. It required 24.25 mL of a standard 0.02 M EDTA (ethylenediaminetetraacetic acid) solution to titrate the Ca2+ ions to the end point. (moles= 4.85 * 10^-4) a. How many moles of EDTA are contained in the 24.25 mL used for tritration. b. How many moles of CaCO3 were used? c. What is the concentration (molarity) of Ca2+ in the 25.00 mL of solution?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.35QAP

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