A spectrophotometric method for the quantitative determination of the concentration of Pb2+ in blood yields an Ssamp of 0.133 for a 1 mL sample of blood that has been diluted to 6 mL. A second sample is spiked with 1 µL of a 1467 ppb Pb2+ standard and diluted to 6 mL, yielding an Sspike of 0.491. Determine the concentration of Pb2+ in the original sample of blood.
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A spectrophotometric method for the quantitative determination of the concentration of
Pb2+ in blood yields an Ssamp of 0.133 for a 1 mL sample of blood that has been diluted to 6
mL. A second sample is spiked with 1 µL of a 1467 ppb Pb2+ standard and diluted to 6 mL,
yielding an Sspike of 0.491. Determine the concentration of Pb2+ in the original sample of
blood.
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- A spectrophotometric method for the quantitative analysis of Pb2+ in blood has a normal calibration curve for which Sstd=(0.296 ppb−1)×Cstd+0.003. What is the concentration of Pb2+ in a sample of blood if Ssamp is 0.397?A second spectrophotometric method for the quantitative analysis of Pb2+ in blood yields an Ssamp of 0.712 for a 5.00 mL sample of blood. After spiking the blood sample with 5.00 μL of a 1560 ppb Pb2+ external standard, an Sspike of 1.546 is measured. What is the concentration of Pb2+ in the original sample of blood?A 10.00 mL of natural water sample containing Ni2+ was pipetted into a volumetric flask and diluted to 50.00 mL with pure water. In the second 10.00 mL of natural water sample transferred into a volumetric flask, exactly 4.00 mL of a Ni2+ solution with a concentration of 5.99 mg/L was added and then diluted to 50.00 mL with pure water. The measured absorbance is A1= 0.436 and A2 = 0.663. What is the Ni2+ concentration in unit of mg/L in the natural water sample?
- 4- A sample containing H2C204 had a purity equal to 90.50% (w/w). An unknown mass of this sample was dissolved in water and transferred to a 50.00 mL flask. An aliquot of 25.00 mL was transferred to an erlenmeyer flask and 50.00 mL of a 0.2000 mol L^-1 NaOH solution were added. %3 Excess NaOH was titrated with 0.09000 mol L^-1 HCI solution using 2.000 mL. Calculate the mass (g) of the sample used. Data: H = 1.008 C= 12.01 O = 16.00The nitrite in a series of standard solutions (mg/L, n = 5) are converted to azo dye and the slope of the calibration curve is 2.0 ppm1. A 10.00-mL mineral water sample is treated in the same way as standards and diluted to a final volume of 100.00-mL. It gives an absorbance of 0.80. The absorbance of blank solution under the same conditions is 0.10. Calculate ppm (mg/L) of NO2 (46 g/mol) and the molarity of NANO2 (69 g/mol) in the original sample2+ as (6) A sample of an ore was analyzed for Cu* follows. A 1.25 g sample of the ore was dissolved in acid and diluted to volume in a 250 mL volumetric flask. A 20 mL portion of the resulting solution was transferred by pipet to a 50 ml volumetric flask and diluted to volume. An analysis showed that the concentration of 2+ Cu* in the final solution was 4.62 ppm. What is the weight percent of Cu in the original ore?
- (Standard addition) Tooth enamel consists mainly of the mineral calcium hydroxyapatite, Ca10(PO4)6(OH)2. Trace elements in teeth of archeological specimen provide anthropologists with clues about diet and diseases of ancient people. Student at Dankook University measured the trace element strontium (Sr) in enamel from extracted wisdom teeth by atomic absorption spectroscopy. Solutions were prepared with a constant total volume of 10 mL containing 0.750 mg dissolved tooth enamel plus variable concentrations of added standard Sr. Added Standard Sr (ng/mL=ppb) 0 2.50 5.00 7.50 10.00 Emission Signal 28.0 34.3 42.8 51.5 58.6 (a) Make a graph showing the experimental data and the calculated straight line. (b) Find the concentration of Sr in the tooth ennamel in parts per million = μg/mL.A freshwater sample containing Ca2+ and Mg2+ will be analyzed using EDTA titration. The EDTA titrant was standardized by dissolving 0.5005g of CaCO3 (99.00% purity) in 100.0mL. A 10.00-mL aliquot was then titrated using 24.93 mL of EDTA titrant to the Eriochrome Black T endpoint. A sample with a volume of 250.00 mL is titrated with 20.32 mL of the EDTA titrant in an ammonia buffer at pH 10.00. Another 250.00 mL sample was then treated with NaOH to precipitate Mg(OH)2 and was then titrated at pH 13.00 with 10.43 mL using the same EDTA solution. FW: CaCO3 (100.09 g/mol) & MgCO3 (84.314 g/mol) Questions: Find concentration of EDTA titrant in M. Calculate the Amount of CaCO3 and MgCO3 in the sample. Express your answers in moles and ppm of each compound.A freshwater sample containing Ca2+ and Mg2+ will be analyzed using EDTA titration. The EDTA titrant was standardized by dissolving 0.5005g of CaCO3 (99.00% purity) in 100.0mL. A 10.00-mL aliquot was then titrated using 24.93 mL of EDTA titrant to the Eriochrome Black T endpoint. A sample with a volume of 250.00 mL is titrated with 20.32 mL of the EDTA titrant in an ammonia buffer at pH 10.00. Another 250.00 mL sample was then treated with NaOH to precipitate Mg(OH)2 and was then titrated at pH 13.00 with 10.43 mL using the same EDTA solution. FW: CaCO3 (100.09 g/mol) & MgCO3 (84.314 g/mol) c. What is the total hardness of the water sample expressed as ppm CaCO3. Total hardness = ____ ppm CaCO3
- A freshwater sample containing Ca2+ and Mg2+ will be analyzed using EDTA titration. The EDTA titrant was standardized by dissolving 0.5005g of CaCO3 (99.00% purity) in 100.0mL. A 10.00-mL aliquot was then titrated using 24.93 mL of EDTA titrant to the Eriochrome Black T endpoint. A sample with a volume of 250.00 mL is titrated with 20.32 mL of the EDTA titrant in an ammonia buffer at pH 10.00. Another 250.00 mL sample was then treated with NaOH to precipitate Mg(OH)2 and was then titrated at pH 13.00 with 10.43 mL using the same EDTA solution. FW: CaCO3 (100.09 g/mol) & MgCO3 (84.314 g/mol) a. What is the concentration of the EDTA titrant? b. Calculate the Amount of CaCO3 and MgCO3 in the sample. Express your answers in ppm of each compound. mol Ca2+ = _____ mol mol Mg2+ = _____ mol [Ca2+] = ______ ppm CaCO3 [Mg2+] = ______ ppm CaCO3A freshwater sample containing Ca2+ and Mg2+ will be analyzed using EDTA titration. The EDTA titrant was standardized by dissolving 0.5005g of CaCO3 (99.00% purity) in 100.0mL. A 10.00-mL aliquot was then titrated using 24.93 mL of EDTA titrant to the Eriochrome Black T endpoint. A sample with a volume of 250.00 mL is titrated with 20.32 mL of the EDTA titrant in an ammonia buffer at pH 10.00. Another 250.00 mL sample was then treated with NaOH to precipitate Mg(OH)2 and was then titrated at pH 13.00 with 10.43 mL using the same EDTA solution. FW: CaCO3 (100.09 g/mol) & MgCO3 (84.314 g/mol) Question: What is the concentration of EDTA titrant in M?A spectrophotometric method for the quantitative determination of Pb2+ levels in blood uses Cu²+ as an internal standard.A standard containing 1.75 ppb Pb2+ and 2.25 ppb Cu2* yields a ratio of SA/Sis of 2.37.A sample of blood is spiked with the same concentration of Cu2* giving a signal ratio of I.80. Determine the concentration of Pb2+ in the sample of blood.