A 50.00-mL aliquot of solution containing 0.310 of MgSO4 (FM 120.37) in 0.500 L required 37.77 mL of EDTA solution for titration. How many milligrams of CaCO3 (FM 100.09) will react with 1.00 mL of this EDTA solution? Answer in 3 significant figures. Do not include the unit. need asap
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A 50.00-mL aliquot of solution containing 0.310 of MgSO4 (FM 120.37) in 0.500 L required 37.77 mL of EDTA solution for titration. How many milligrams of CaCO3 (FM 100.09) will react with 1.00 mL of this EDTA solution?
Answer in 3 significant figures. Do not include the unit.
need asap
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- A 50.00-mL aliquot of solution containing 0.358 of MgSO4 (FM 120.37) in 0.500 L required 38.08 mL of EDTA solution for titration. How many milligrams of CaCO3 (FM 100.09) will react with 1.00 mL of this EDTA solution?A50.0 mL aliquot of solution contairing 0.450 g of MgSO4 [FM 120.27) in 0.500 L required 376 mL of EDTA solution for titration. How many miligrams of CaCO3 (FM 106.09) will react with 100 mL of this EDTA solution?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 5.00 mL sample that contains the borate ion {B4O5(OH)42-} at 35oCwas transferred to an Erlenmeyer flask and diluted with water to ~25 mL. This solution was titrated with 20.9 mL of 0.21 M HCl to the bromocresol green endpoint. What is the Ksp for the borax? Report your Ksp value to 3 decimal places.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?a. A deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 10 ( with Mg-EDTA pH 10 buffer reagent) and consumed 31 mL. Calculate the Total Hardness of the water sample as mg CaCO3. b. A deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 12 and consumed 31 mL. Calculate the Calcium content of the water sample in mg/L.
- A 30-mL portion of a solution containing Ca2+ and Mg2+ was titrated with 28.19 mL of 0.213 M EDTA at pH 10. Another 30-mL aliquot of the same Ca-Mg mixture was treated with NaOH to make the solution strongly alkaline and precipitate Mg(OH)2. This solution was then titrated with the same EDTA solution. What would be the required EDTA volume (in mL) to reach the endpoint of the second aliquot if it was found that there was 0.061 M of Mg2+ in the sample?Please answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE. A 50.00-mL sample of water containing Ca2+ and Mg2+ is titrated with 10.28 mL of 0.01001 M EDTA in an ammonia buffer at pH 10.00. Another 50.00-mL sample is titrated with NaOH to precipitate Mg(OH)2 and then titrated at pH 13.00 with 6.75 mL of the same EDTA solution. Calculate the concentration of CaCO3 and MgCO3 in the sample in ppm.1. How much volume (mL) is needed to standardize 0.05M of EDTA using 180mg of magnesium ribbon? MW: 24g/mol2. How many grams of EDTA is required to prepare 250mL of a 0.05M solution? MW: 292g/mol3. What is the Molarity of the EDTA solution if 35mL of the titrant was added to 0.2g of calcium carbonate? Round off to four decimal places
- 10) 1.0 gram of CaCO3 was dissolved in HCl and the solution was made up to 1000 ml with distilled water. 50 ml of the solution required 45 ml of EDTA solution for titration, 50 ml of hard water sample required 28 ml of EDTA and after boiling and filtering required 15 ml of EDTA solution. Calculate Temporary Hardness. A. 288.6 ppmB. 166.6 ppmC. 88.6ppm 11) Calculate the Permanent Hardness for No. 10 A. 111 ppmB. 222 ppmC. 333 ppm 12) Calculate the Total Hardness for No. 10 A. 421.6 ppmB. 621.6 ppmC. 521.6 ppmAn automatic titration was performed with the following results: Standardized NaOH Solution Concentration: 0.1191 M Volume of HA- product examined in each trial: 25.00 mL Volume of Standardized NaOH Titrant used to achieve the first equivalence point: Trial #1: 1.300 mL Trial #2: 1.137 mL Trial #3: 1.140 mL Calculate the %(w/v) for each trial, Average Concetration (%), Deviation (%), Standard Deviation (%), and RSD (%)Concentration EDTA (M): 1.94e-3 Trial #1 Trial #2 Trial #3 Volume of Water Sample titrated (mL): 25.00 25.00 25.00 Volume EDTA used (mL): 36.23 39.00 37.77 Calculate the average of the volume of EDTA used. Calculate the number of moles of EDTA solution required to titrate the water sample. The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample. The total hardness and the information on Table 1 is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3/KgH2O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO3 per liter of water. Determine the number of moles of CaCO3 present in the bottled water, assuming all the Ca2+ combine with CO32−. Calculate the number of grams of CaCO3 present and convert to mg.…