A 20.8 mL of EDTA solution ( 2.0M) was used in a titration to determine the hardness of the water. If 25.0 mL was used for this experiment calculate the hardness of water. (Molar mass of CaCO3 = 100.09 g) 10 ppm 20 ppm 12300 ppm 166549 ppm E) 256789 ppm
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- A sample of water from a river was analyzed by titrating a 125 mL aliquot with 0.0210 M EDTA, consuming 22.52 mL. Express the hardness of the water in ppm of CaCO3.In order to adjust the Potassium Permanganate solution, 0.0544g Na2C2O4 was taken and necessary experimental procedures were performed on it and the titrant consumption was found to be 7.9 mL. What is the KMnO4 concentration? A. 0.040B. 0.044C. 0.021D. 0.027C1. A carefully weighed 280mg Calcium carbonate was used in the standardization of an EDTA solution. Initially, 25mL of the titrant was consumed but only after the addition of another 10mL of the titrant did an endpoint was visible. What is the MW of calcium carbonate? (use C1 as reference)* 102 g/mol 98 g/mL 100 g/mL 100 g/mol What is the molar concentration of the standardized EDTA solution? (use C1 as reference)* 0.08m 0.8M 0.08N 0.08M How many grams of EDTA (MW: 292 g/mole) is required to prepare 250mL of a 0.025M solution?* 0.1825 0.1852 1.825 1.1852
- Titration of a 0.824 g of 99.99% KHP (204.23 g/mol) with phenolphthalein required 18.3 mL of NaOH (40.00 g/mol) solution to reach the end point. The same titrant was used to analyze an impure acetic acid (CH3COOH, 60.06 g/mol) solution. A 10.0 mL aliquot of the sample required 12.9 mL of the titrant. What substance served as the primary standard?Which served as the indicator in the titration?What is the color at the end point?What is the concentration of the titrant?What is the molar concentration of the acetic acid solution?1) 100 mL tap water is titrated with 20 mL of 0.02 M EDTA solution to determine the hardness of the water. The second 100 mL tap water is precipitated as CaC2O4 and removed by filtration and the filtrate is titrated with 8.0 mL of the same EDTA solution. What are the concentrations (as ppm) of Ca2+ (40.078 g/mol) and Mg2+ (24.305 g/mol) ions in the water? 2) 10 g of a solution, containing one or more of NaOH, Na3PO4, Na2HPO4, NaH2PO4, H3PO4 and HCl substances, is titrated with 1.0 M NaOH using the phenolphthalein indicator and 34.5 mL NaOH is used. Another 10 g mixture was titrated to reach the bromocresol green end point and 20.50 mL NaOH is used. What is the composition of the solution? What are the percentages of the species(H:1.0078, O:15.99, Na: 22.98, P:30.974, Cl:35.453)?Determine the total hardness of water (ppm CaCO3; MM: 100.09 g/mole) if 100.0mL sample of drinking water required 38.41mL of 4.65 x 10-3 M EDTA for titration. 179 ppm CaCO3 357 ppm CaCO3 452 ppm CaCO3 733 ppm CaCO3
- Standardization of EDTA was done using MgSO4 standard wherein a 50-mL aliquot of solution obtained from 0.480 g MgSO4 in 500 mL needed 39.4 mL of the EDTA solution to reach the endpoint. Determine how many milligrams of CaCO3 will react per mL of this EDTA solution.What is the mass of pure dry CaCO3 (MW: 100.0869 g/mol) standard used in the standardization of EDTA solution? Assume that 1.758 M EDTA solution was computed based on the titration of CaCO3 standard. The volume of titrant needed to reach the endpoint was 35.00 mL. Ca2+ + Y4- → CaY2- 0.1500 g 5.630 g 6.158 g 0.6158 gIn how much volume of diluted sulfuric acid should you dissolve a multivitamin tablet of approximately 1700 mg of Vitamin C to back analyze 10.00 mL of that solution, with 25.00 mL of 0.01 M KIO3 and 0.04 M thiosulfate to use approximately 8-10 mL of titrant ? You have 25, 50, 150, 250 and 500 mL flasks.
- An unknown sample of Cu2+gave an absorbance of 0.262. Then 1.00 mL of solution containing 100 ppm (ug/mL)Cu2+was mixed with 95.0 mL of the unknown and the mixture was diluted to 100 mL in a volumetric flask with deionized water. The absorbanceof the new solution was 0.500. a.Denoting the initial unknown concentrationas [Cu2+]i,write an expression for the final concentrationafter dilution [Cu2+] b.Find [Cu2+]in the unknown.Calculate the pCa for the titration of 50 ml of 0.02 M Ca2+ at pH = 8 with 0.4 M EDTA at the equivalence point Ca2+ + Y4- ⇄ CaY2- Kf = 5x1010 Select one: a. 7 b. 12 c. 10 d. 5 e. 910. The color change of a chemical indicator requires an over titration of 0.03 mL. Calculate the percent relative error if the total volume of titrant is(a) 50.00 mL. (b) 10.0 mL. (c) 25.0 mL.(d) 30.0 mL.