Use the molarity of the EDTA solution and the average volume of EDTA added to calculate the average number of moles of EDTA required for the titration. Molarity EDTA = 0.01 & Volume EDTA = 0.01755 L. Find moles?
Added by Angela H.
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We are given the molarity of the EDTA solution, which is 0.01 M, and the average volume of EDTA added during the titration, which is 0.01755 L. Show more…
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You are standardizing an EDTA solution. 0.2500 grams of CaCO3 (Mwt. 100.0892 g/mol) are dissolved into 250.0 mL of water. 25.00 mL of this calcium carbonate solution was titrated with the EDTA solution. The titration volume was 24.88 mL. The blank titration is 1.23 ml. Calculate the concentration of the EDTA solution in moles per liter.
Derrick D.
An average of 35.35 mL of EDTA solution was required to titrate 50.0 mL aliquots of a standard that contained 0.9682 g of MgCO3 (84.314 g/mol) per liter. What is the molarity of the EDTA solution. Write your answer up to four decimal places and do not write the unit.
Dr. Satish I.
The total concentration of $\mathrm{Ca}^{2+}$ and $\mathrm{Mg}^{2+}$ in a sample of hard water was determined by titrating a $0.100-\mathrm{L}$ sample of the water with a solution of EDTA $^{4-}$. The EDTA $^{4-}$ chelates the two cations: $$ \begin{array}{r} \mathrm{Mg}^{2+}+[\mathrm{EDTA}]^{4-}--\rightarrow[\mathrm{Mg}(\mathrm{EDTA})]^{2-} \\ \mathrm{Ca}^{2+}+[\mathrm{EDTA}]^{--}--\rightarrow[\mathrm{Ca}(\mathrm{EDTA})]^{2-} \end{array} $$ It requires $31.5 \mathrm{~mL}$ of $0.0104 M[\mathrm{EDTA}]^{4-}$ solution to reach the end point in the titration. A second $0.100-\mathrm{L}$ sample was then treated with sulfate ion to precipitate $\mathrm{Ca}^{2+}$ as calcium sulfate. The $\mathrm{Mg}^{2+}$ was then titrated with $18.7 \mathrm{~mL}$ of $0.0104 \mathrm{M}[\mathrm{EDTA}]^{4-}$. Calculate the concentrations of $\mathrm{Mg}^{2+}$ and $\mathrm{Ca}^{2+}$ in the hard water in $\mathrm{mg} / \mathrm{L}$.
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