Calculate the molar concentration (and uncertainty) of an EDTA solution of which 5.40(±0.05) mL was used to titrate 100.00(±0.03) mL sample containing 0.786(±0.005) mg primary standard CaCO₃. Consider the molecular weight [100.09 g/mol] of CaCO₃ to have a negligible uncertainty
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Calculate the molar concentration (and uncertainty) of an EDTA solution of which 5.40(±0.05) mL was used to titrate 100.00(±0.03) mL sample containing 0.786(±0.005) mg primary standard CaCO₃. Consider the molecular weight [100.09 g/mol] of CaCO₃ to have a negligible uncertainty
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- SCE students measured the concentration of HCl in a solution by titrating with different indicators to find the end point.Indicator Mean HCl concentration (M)(± standard deviation)Number of measurementsBromothymol blue 0.09565 ± 0.00225 28Methyl red 0.08686 ± 0.00098 18Bromocresol green 0.08641 ± 0.00113 29Is the difference between indicators 1 and 2 significant at the 95% confidence level? Answer the same question for indicators 2 and 3Spectrophotometric Determination of a Metal A 100.00 mL of exactly 250.0 mg/L Cu2+ stock solution was prepared using a 99.95% pure Cu(NO3)2-3H20 (241.60 g/mol). From this stock, a series of standard solutions were prepared by pipetting certain volumes into 100-mL volumetric flasks, followed by adding 2.00 mL of concentrated NH3, and finally diluting to mark with deionized water. Additionally, a blank solution was prepared by using only NH3 and distilled water. Question: Why was NH3 added to each standard solution before diluting with distilled water? What will be the resulting color of the solution and why is this the color that is observed?A 20-mL solution of 0.0659 M AgNO3 was titrated with 20 mL of 0.0509 M NaCl (Ksp = 1.8x10-10). Calculate the pAg of the analyte solution. Express your answer with 3 decimal places.
- 25 ml of pickled brine was taken from an apple pickled with vinegar and diluted to 500 ml, 25 ml of this was taken and acidity was determined with 0.2 N (Factor: 1.05) NaOH. In the main trials, 6.3 ml - 6.5 ml - 6.9 ml, respectively, 0.1 ml base was used in the analysis without using the sample.For example, how many ppm is its acidity?2+ 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?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 = 16.00
- The mass percent of Fe in an unknown salt sample was determined using both volumetric and gra vimetric titration. Ten determinations using both methods were performed. Volumetric(% of Fe): 24.22, 23.86, 24.07, 24.49, 24.69, 23.71, 24.28, 24.11, 24.26, 24.10 Gravimetric (% of Fe): 24.35, 24.26, 24.10,24.19, 24.18, 24.32, 24.11, 24.33, 24.17, 24.12 a. Do the two methods give similar standard deviations? b. Do the two methods give similar results for the mass percent of Fe at the 95% confidence level?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.In the acetic acid determination in vinegar experiment; NaOH was standardized with 0.35 g KHP (molar mass = 204.22 g/mol). The KHP was dissolved in 75.0 mL distilled water in a 250 mL Erlenmeyer flask and titrated to the endpoint colour by dispensing 11.40 mL of NaOH from the burette. Calculate the molarity of NaOH. a. 0.10 М b. 0.15 M с. 0.20 М d. 0.35 M e. 0.25 М
- 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 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