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an experiment to find water hardness required 18.2 ml of 0.0050 M EDTA solution to titrate 40.0 mL of tap water using eriochrome black t indicator. Calculate the parts per million calcium present
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- You titrate 50.00 mL of hard water with 14.86 mL of 0.0100 M EDTA solution. How many moles of Ca²+ are present in the sample? What is the hardness in units of mg CaCO, per Liter of solution?If 10.00 mL sample of 0.01 M standard Ca2+ solution is titrated with 9.8 mL of EDTA solution, what is the molarity of EDTA? (Ca: 40 g/mol)A 10.00 mL sample of a Ca(OH)₂ solution is diluted to 250.0 mL total volume. A 25.0 mL sample of the 250.0 mL solution is titrated with 0.256 M HCl solution, and the equivalence point is found to be 34.68 mL. What is the concentration of Ca(OH)2 in the original solution (before diluting to 250.0 mL)?
- 50.00 mL of a solution containing iron (II) and iron (III) when titrated at pH2.0, 12.50 mL 0.01200 M EDTA and when titrated at pH 6.0, 28.50 mL EDTA is spent. Find the concentration of each solute in this solution in ppm. (Fe (AA) = 55,847 g / mol) A. 184 ppm Fe3+, 213 ppm Fe2+B. 167,5 ppm Fe3+, 214,4 ppm Fe2+C. 213 ppm Fe3+, 184 ppm Fe2+D. 214,4 ppm Fe3+, 167,5 ppm Fe2+In the titration of 25.00 mL of a water sample, it took 19.040 mL of 4.965x 10−3 M EDTA solution to reach the endpoint. The total hardness is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3 / Kg H2O). 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 titrated sample of water, assuming that all the Ca2+ combines with CO32−. (enter your answer with 3 significant figures)a 20 mL of EDTA titrant is required to titrate 40 mL of standard 0,25M CaCO3. A 70 mL hard water sample requires 35 mL of this EDTA titrant for total hardness determination. Calculate (a) ppm Ca, (b) ppm CaCO3 in the sample.
- Titration of Ca2+ and Mg2+ in a 50.00-mL sample of hard water required 23.65 mL of 0.01205 M EDTA. A second 50.00-mL aliquot was made strongly basic with NaOH to precipitate Mg2+ as Mg(OH)2(s). The supernatant liquid was titrated with 14.53 mL of the EDTA. Calculate the concentration in ppm of CaCO3 in the sample. Calculate the concentration in ppm of MgCO3 in the sample.Develop a titer for determining water hardness based on the following information: 6.240 mg/L Ca2+ calcium standard. It is titrated to the endpoint with 8.59, 8.34, and 8.47 mL of EDTA solution.Calculate the amount of solid in grams you would need to measure to prepare 50.0 mL of 0.100M sodium acetate buffer (MW 136.08).
- A 865.6 gram sample of bacon was pureed in a blender with 100 mL water. The suspension was filtered and the clear solution containing dissolved sodium nitrite was adjusted to pH 2. This solution was treated with 15.00 mL of KMnO 4 solution (1 mL » 212.4 mg H 2C2O4 × 2H 2O) and was back titrated with 12.73 mL of FeSO4 solution (1 mL » 87.5 mg K 2Cr2O7). Calculate the amount of nitrite (NO2–1) in ppm. H2C2O4 × 2H 2O (126) K2Cr2O7 (294.2) a. 370 b. 1480 c. 740 d. 11101. TRUE OR FALSE (a) Y-4 is the form of EDTA that effectively chelates metals in solution. True False (b) A complexometric titration is a form of volumetric titration in which the formation of a colored complex between the metal and the indicator is used to indicate the end point of a titration. True False40.00 mL of 0.1100 M HCl is diluted to 100 mL with H2O and titrated with 0.1 M NaOH. Calculate the pH after addition of the following volume (mL) of titrant. a. 0.00 b. 10.00 c. 22.00 d. 40.00 e. 43.95 f. 44.00 g. 44.05 h. 50.00 Plot the titration curve.