The end point of a titration was reached after 21.3 mL of 0.3 M disodium EDTA titrant was dispensed into a solution containing the zinc ion.
Calculate the moles of disodium EDTA used.
The end point of a titration was reached after 21.3 mL of 0.3 M disodium EDTA...
The end point of a titration was reached after 26.8 mL of 0.4 M disodium EDTA titrant was dispensed into a solution containing the zinc ion. Calculate the moles of disodium EDTA used.
The end point of the Zn2+−EDTA titration was observed after 21.50 mL of 0.0500 M EDTA solution was dispensed. Determine the number of moles of zinc ion present in the sample. number of moles of zinc ion =
A titration was performed to standardize an EDTA solution. a) A 25.00 mL aliquot of a standard solution containing 0.01500 M Ca2+ required 42.87 mL of EDTA to reach the endpoint. The molarity of the EDTA solution is: ________ M b) That same EDTA solution was then used to titrate an unknown hard water sample. A 40.00 mL aliquot of unknown hard water required 34.21 mL of EDTA solution to reach a distinct endpoint. The concentration of Ca2+ ions (assuming...
The end point in a titration of a 76 mL sample of aqueous HCI was reached by the addition of 63 mL of 0.23 M NaOH titrant. The reaction proceeds by the following equation. HCl(aq) + NaOH(aq) - NaCl(aq) + H2O(1) What is the molar concentration of HCI? Report your answer with two significant figures.
Problem 1: Consider titration of 24.0 mL of 0.0800 M Ga(NO3)3 with 0.0400 M EDTA at pH 4.00. (a) Calculate pGa+ (to the 2nd digit after the decimal point) upon addition of 10.00 mL of the EDTA solution. Log Ki= 20.30. (b) What is the pGa at the equivalence point of this titration? (C) What is the pGa upon addition of 50.00 mL of the EDTA solution?
1. What is the amount in grams of EDTA you will need to measure out to prepare a 250 mL 0.01 M EDTA solution ? The molar mass of EDTA is 374.27 g/mol. 2. Titration Data from three water samples Water Volume of 0.01 Water Drops of MEDTA Moles Ca2+ sample indicator used to of concentration volume Calmagite reach Ca2+ in water (M) end point source 50 mL4 2 ml USFISA drinking water fountain USF BSF drinking water fountain 50...
Titration of 5.00 mL of a solution labeled 0.237 6 M HCI requires addition of 40.02 mL of an NaOH solution to reach the equivalence point. 1. How many moles of HaO were used in the titration? 2. At the equivalence point, how many moles of OH had been added? 3. Calculate c in the titrant. OH in the OH 4. Another 1.00 mL of the NaOH solution is added after the equivalence point. Calculate c reaction mixture.
In a titration experiment, 9.3 mL of an aqueous H2SO4 solution was titrated with 0.3 M NaOH solution. The equivalence point in the titration was reached when 9.9 mL of the NaOH solution was added. What is the molarity of the H2SO4 solution?
A 50.0 mL sample containing Cd²+ and Mn + was treated with 43.8 mL of 0.0700 M EDTA. Titration of the excess unreacted EDTA required 14.4 mL of 0.0320 M Ca2+ The Cd2+ was displaced from EDTA by the addition of an excess of CN. Titration of the newly freed EDTA required 28.2 mL of 0.0320 M Capt. What are the concentrations of Cd- and Mn in the original solution? concentration: M Mn+ concentration: M Cd2+
Question 15 (1 point) Saved If a titration trial requires 10.86 mL of EDTA solution to reach the endpoint, how many moles of CaCO3 are in the sample if the concentration of the iodine solution is 0.003232 M? Your Answer: mol Answer units