Calculate the concentration of an EDTA solution of which 24.22 mL were needed to titrate the Ca2+ ions present in a 50.00 mL solution containing 246.7 mg CaCO3. Express your answer in terms of (a) molar concentration of EDTA (b) Ca Titer (mg Ca per mL of EDTA) MM Ca= 40.078
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Calculate the concentration of an EDTA solution of which 24.22 mL were needed to titrate the Ca2+ ions present in a 50.00 mL solution containing 246.7 mg CaCO3.
Express your answer in terms of
(a) molar concentration of EDTA
(b) Ca Titer (mg Ca per mL of EDTA)
MM Ca= 40.078
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- Titration of 25.0 mL of a 0.0500 M Zn2+ solution with 0.0550 M EDTA in a solution buffered at pH 8. Assume that the temperature is 25 oC and that the formation constant for Zn2+ is 3.13 x 1016 at this temperature. What is the pZn of the solution after 30 mL of titrant have been added?Calcium in powdered milk is determined by dry ashing a 1.46g sample and then titrating the calcium with EDTA solution, 12.1mL being required. The EDTA was standardized by titrating 10.4mL of a Zn solution prepared by dissolving 0.634g Zn metal in acid and diluting to 1L (10.83mL EDTA required for titration). What is the concentration (ppm) of calcium in the powdered milk?Calculate the concentration of an EDTA solution of which 24.22 mL were needed to titrate the Ca2+ions present in a 50.00 mL solution containing 246.7 mg CaCO3. Express your answer in terms of (a) molar concentration of EDTA (b) Ca Titer (mg Ca per mL of EDTA) MM Ca= 40.078
- 50 mL of a sample known to contain Mg+2 was taken and titrated with 0.075 M EDTA standard solution by adding pH 10 buffer and EBT indicator. Since the EDTA consumption is 10.5 mL, which of the following is the amount of magnesium in the sample in ppm? (Mg:24 g/mol) A. 378 B. 302 C. 214 D. 251Calcium in powdered milk is determined by dry ashing a 3.00g sample then titrating the calcium with 12.10mL EDTA solution. The EDTA was standardized by titrating 10.00mL of a Zn solution by dissolving 0.632g Zn metal in acid and dilution to 1.00L (10.80 mL EDTA required for titration). What is the concentration of Ca in the powdered milk in ppm?The hardness of a water sample may be determined by titrating a 100-mL sample of water with 0.010 M EDTA. If the Eriochrome Black T (EBT) end point occurs after 12.3 mL of the EDTA solution is added, calculate the water hardness in terms of (1) ppm CaCO3 and (2) mM Ca2+.
- 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.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. If the excess EDTA was back-titrated with 23.10 mL of 0.02 M EDTA, which of the following is the percentage of Pb(NO3)2? (Pb(NO3)2: 331 g/mol, Pb: 207 g/mol) A. 85,23B. 38.25C. 35.63D. 79.17To determine the concentration of an EDTA solution, the following magnesium(II) solution is prepared: metallic magnesium (m(Mg) = 0.5915 g) is dissolved in dilute sulfuric acid, the resulting solution is poured into a volumetric flask with a volume of 0.250 L and is filled to the graduation mark with water. The titration of an aliquot of magnesium(II) solution with a volume of 25.00 ml consumes (11.11 ml; 11.32 ml; 11.24 ml; 11.29 ml) of EDTA. Calculate the concentration of EDTA solution with accuracy corresponding to the starting data, give confidence interval.
- Five white, 500-mg uncoated ascorbic acid (AA) tablets with an average weight of 0.6100-g were pulverized in a mortar. A sample of the powdered ascorbic acid weighing 0.4610-g was placed in an iodine flask and was dissolved in 50-mL H2SO4 then 5-g of KBr was added to the resulting solution. The solution was titrated with 46.73-mL of 0.0152 M STD. KBrO3 to reach a faint yellow endpoint then 3-g KI and 5-mL Starch TS. The blue color solution is then titrated with 2.78-mL of 0.1047 M STD. Na2S2O3 to reach the disappearance of the blue iodostarch complex. MW: KBrO3 = 167.0 ; KIO3 = 214.0 ; Na2S2O3 = 158.11 ; C6H8O6 = 176.12 Compute the milligrams of pure AA per tablet from the assay. None of the choices 349.7 mg 264.3 mg 462.7 mgCalculate the PCa vs. EDTA titration curve for 50.0 mL of 0.0060 M Ca2+ being titrated with 0.0150 M EDTA in a solution buffered to a constant pH of 10.00. After the addition of 0.00 mL After the addition of 26.0 mLCalculate the PCa vs. EDTA titration curve for 50.0 mL of 0.0060 M Ca2+ being titrated with 0.0150 M EDTA in a solution buffered to a constant pH of 10.00. After the addition of 0.00 mL After the addition of 5.00 mL After the addition of 26.00 mL