For the titration of 50.00 mL of 0.000226 M Ba²* with 0.100 M EDTA at pH 10.00, ay = 0.30, and Kf = 7.59 x 107, calculate the initial pBa²* (i.e. before the EDTA titration begins) to the correct number of significant figures. %3D
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- 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 , filtered, and titrated with 14.53 mL of same EDTA solution. Calculate the ff: a.)The total hardness of water sample. b.)Concentration in ppm CaCO3 in the sample. c.)Concentration in ppm MgCO3 in the sample5A. Construct the titration curve for a 25.00 mL mixture solution of 0.0800 M in Br- and 0.0600M in IO3- titrated with 0.1000 M AgNO3. Calculate the pAg values of the titration solution after addition of 5.00mL, 20.00 mL, and 30.00 mL of 0.1000 M AgNO3 solution.KSP AgIO3 = 3.0 × 10-8 KSP AgBr = 5.2 × 10-13 Please answer fast i give you upvote.5. A 300.0 mg sample containing Na,CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
- You are doing a titration for a 16 mL mixture solution of 0.097 M in Cl and 0.100 M in I titrated with 0.100 M AGNO3. Calculate the pAg value of the titration solution after addition of 16 mL of 0.1000 M AGNO3 solution. Ksp AgCI = 1.77 × 10-10; KSp Agl = 8.30 x 10-17In a Complexometric Titration Experiment, the preparation of the EDTA solution is as follows: In a 250 mL beaker, weigh 0.10 g MgCl2*6H2O and 1.0 g NaOH. Add approximately 200 mL distilled water and stir to dissolve. Add about 2.0 g of EDTA and transfer the solution quantitatively to a 1-L volumetric flask. Dilute to the mark with distilled water. What is the purpose of adding MgCl2*6H2O? Please show COMPLETE solution.(b) Calculate pAg after 35.00 mL of 0.0500 MAGNO3 titrated with 50.00 mL of 0.0400 M KBr. Ksp AgBr is 5.00 x 10-13.
- 4. A 100-mL solution of the ion Mg2+ at a concentration of 0.0500 M buffered to pH 9.00 was titrated with 0.0500 M EDTA. (a) The formation constant is 1.0 x 1012 and aY(H) = 0.041 ( pH=9.00 ) . Calculate the value of the effective formation constant. (b) Calculate the concentration of Mg2+ at VEDTA = Ve . (c) What is the concentration of Mg2+ at VEDTA = 1.1 Ve ?8:A 75mL sample of water is titrated with 0.100M EDTA. exactly 16.9mL of EDTA are required to reach the EBT endpoint. calculate the total hardness in ppm CACO3 a) 2.253 ppm O 0.030 x 10^3 ppm. c) 0.02534 ppm O d) 2.253 x 10^3 ppmComplexometric titrations are generally conducted to determine divalent cations. The most important applications are the titration of calcium and magnesium with EDTA. (a) A supplement tablet containing about 300.00 mg of calcium ion was dissolved, filtered, and diluted to 100.00 ml volume. Several 2.00 ml samples of the total solution were titrated with 0.0100 M EDTA solution. The mean corrected titration volume was 13.65 mL. Calculate the calcium content of the supplement tablet in mg units. (b) A sample of Epsom Salt of mass 0.7567 g was dissolved uniformly in distilled water in a 250.00 mL volumetric flask. Portions of the magnesium ion solution of volume 10.00 mL were titrated using a 0.01000 M solution of EDTA. The mean corrected titration volume was 12.25 ml. Calculate the percentage by mass (% w / w) of the magnesium in the Epsom Salt sample. (c) A 100.00 mL sample of tap water was titrated with 0.0100 M EDTA solution. The mean corrected titration volume was 14.80 mL. Determine…
- 5. A 300.0 mg sample containing Na,CO3, NaHCO, and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 ml to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.Limestone consists mainly of the mineral calcite, The carbonate content of 0.541 3 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCl, and heating to dissolve the solid and expel Calcium carbonate FM 100.087 The excess acid required 39.96 mL of 0.100 4 M NaOH for complete titration to a phenolphthalein end point. Find the weight percent of calcite in the limestone6. Titration of Ca²+ and Mg²+ in a 50.00-mL hard water sample 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 solution. Calculate the total hardness of the water sample, expressed as ppm CaCO3.