47.6 mL aliquot from a 0.5 L solution that contains 0.45g of MnSO4 (MW is 151 g/mol) required 41.9 mL of an EDTA solution to reach the titration endpoint. What mass of CaCO3 (MW is 100.09 g/mol) will react with 1.58 mL of the EDTA solution?
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A 47.6 mL aliquot from a 0.5 L solution that contains 0.45g of MnSO4 (MW is 151 g/mol) required 41.9 mL of an EDTA solution to reach the titration endpoint. What mass of CaCO3 (MW is 100.09 g/mol) will react with 1.58 mL of the EDTA solution?
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- A 49.10 mL aliquot from a 0.500 L solution that contains 0.530 g of MnSO4 (MW=151.00 g/mol) required 41.6 mL of an EDTA solution to reach the end point in a titration. What mass, in milligrams, of CaCO3 ( MW=100.09 g/mol) will react with 1.53 mL of the EDTA solution?A sample of pure CaCO3 weighing 0.3677g is dissolved in hydrochloric acid and the solution diluted to 250.0ml in a volumetric flask. A 25.00ml aliquot requires 30.26ml of an EDTA solution for titration. Calculate a) the molarity of the EDTA solution; b) the number of grams Na2H2Y•2H2O (FW = 372.2) required to prepare 500.0ml of the solution.25.00 mL aliquots of the solution in problem 1 are titrated with EDTA to the calmagite end point. A blank containing a small measured amount of Mg^2+ requires 2.12 mL of the EDTA to reach the end point. An aliquot to which the same amount of Mg^2+ is added requires 25.88 mL of the EDTA to reach the end point.
- A 5.00 mL tap water sample was measured out with a volumetric pipette, and added to a 25 mL Erlenmeyer flask. It was then titrated with a 0.0100 M Na2EDTA.2H2O solution, and found to take 0.635 mL of the EDTA solution to reach the blue endpoint.Given that the titration of Ca2+ and Mg2+ in a 50.00-mL sample of hard water required 22.35 mL of 0.01115 M EDTA. A second 50.00-mL aliquot was made strongly basic with NaOH to precipitate the Mg2+ as Mg(OH)2(s) . The supernatant liquid was titrated with 15.19 mL of the EDTA solution. Calculate the concentration in ppm of CaCO3 in the sample.Is this for Average Molarity of EDTA Standard Solution? Then, would it be always the same with average Molarity of EDTA? How about the Ca Titer (mg Ca/mL of EDTA Solution? Show step by step solution.
- 0.8153 g of a sample containing Pb(NO3)2 was taken, dissolved in water, and 40.20 mL of 0.06 M EDTA was added. What is the percentage of Pb(NO3)2 since the excess EDTA is back-titrated with 23.10 mL of 0.02 M EDTA? (Pb(NO3)2: 331 g/mol, Pb: 207 g/mol)A chemist is given a piece of limestone and told that 50.00% of the sample exists as calcium oxide (CaO). To analyze the sample, the chemist wants to dissolve a portion of the sample in 100 mL and then titrate an aliquot (10 mL) using 0.005300 M EDTA. How much sample (in grams) is needed if a titration volume of 25.00 mL EDTA is desired?A solution was prepared by dissolving about 30.00m g of EDTA in approximately 1 L of water and standardizing against 50.00-mL aliquots of 0.004356 M Mg2+. An average titration of 32.65 mL was required. Calculate the molar concentration of the EDTA.
- A sample of pure CaCO3 weighing 0.2428g is dissolved in HCl and the solution diluted to 250ml in a volumetric flask. A 50.00ml aliquot requires 42.74ml of an EDTA solution for titration. A 200ml sample of water containing Ca+2 is titrated with 16.38ml of the EDTA solution. Calculate the degree of hardness of water in ppm CaCO3.Calamine, which is used for relief of skin irritations, is a mixture of zinc and iron oxides. A 1.022-g sample of dried calamine was dissolved in acid and diluted to 250.0 mL. A 50.00 mL aliquot was suitably buffered and titrated with 2.40 mL of 0.002727 M ZnY-2 (Zn-EDTA) solution to allow the following reaction: Fe+3 + ZnY-2 → FeY- + Zn+2. Molecular mass: Fe2O3 = 165.74 a. The weight of sample in the aliquot portion is _________g ? b. the percentage composition of Fe2O3 in the sample is ______ % ?A 5.00 mL tap water sample was measured out with a volumetric pipette, and added to a 25 mL Erlenmeyer flask. It was then titrated with a 0.0100 M Na2EDTA.2H2O solution, and found to take 0.635 mL of the EDTA solution to reach the blue endpoint. a.) How many moles of the 0.0100 M Na2EDTA.2H2O were added in the titration reaction? Show calculation. b.) How many moles of calcium ions were reacted?
