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10.6 10.00 mL of a sample of a solution containing Feand Co are added to 100...
10.7 10.00 mL of a solution of Hg2+ and 25.00 mL of 0.04516 M EDTA are...
10.7 10.00 mL of a solution of Hg2+ and 25.00 mL of 0.04516 M EDTA are added to 100 mL of pH 10 buffer. The resulting solution is titrated with 21.77 mL of 0.02385 M Mg2+ solution. What was the molarity of the Hg2+ solution? Report the answer with the correct number of significant figures.
A 24.34 mL aliquot of a Pb2 solution, containing excess Pb2+, was added to 11.50 mL...
A 24.34 mL aliquot of a Pb2 solution, containing excess Pb2+, was added to 11.50 mL of a 2,3-dimercapto-1-propanol (BAL) solution of unknown concentration, forming the 1:1 Pb2+-BAL complex. The excess Pb2+ was titrated with 0.0157 M EDTA, requiring 9.88 mL to reach the equivalence point. Separately, 39.89 mL of the EDTA solution was required to titrate 32.75 mL of the Pb2+ solution. Calculate the BAL concentration, in molarity, of the original 11.50 mL solution concentration:
6. (8) A 50.0 mL sample of hard water containing Ca2 was titrated with 0.0500 M...
6. (8) A 50.0 mL sample of hard water containing Ca2 was titrated with 0.0500 M EDTA standard solution at pH 10 and with Eriochrome Black T indicator. The endpoint was reached when 11.35 mL of EDTA was added a) (6) Calculate the concentration of Ca* in the unknown sample in moles per liter (M). b) (2) What is the pCa of the solution?
4. 50.0 mL of 0.00200 M Ca2 solution buffer at pH 10.0 is titrated with 0.00200 M EDTA. At equivalence point (i.e. 50.0 mL EDTA has been added), what is the equilibrium concentration of Ca2, [Ca2...
4. 50.0 mL of 0.00200 M Ca2 solution buffer at pH 10.0 is titrated with 0.00200 M EDTA. At equivalence point (i.e. 50.0 mL EDTA has been added), what is the equilibrium concentration of Ca2, [Ca2], and what is the pCa? The formation constant of CaY, Kaa 5.0 x 1010, and α4 of EDTA at pH 10.0 is 0.35
4. 50.0 mL of 0.00200 M Ca2 solution buffer at pH 10.0 is titrated with 0.00200 M EDTA. At equivalence point...
Answer units Save Question 7 (10 points) A 100.00 mL sample of hard water is to...
Answer units Save Question 7 (10 points) A 100.00 mL sample of hard water is to be titrated with 0.03505 M EDTA solution. A small amount of Mg2+ (that required 1.63 mL of EDTA to titrate as a blank solution) is added to the hard water sample. This sample requires 13.47 mL of EDTA to reach the endpoint. What volume of EDTA is used in titrating the Ca2+ in the hard water? Your Answer units Answer Save
Mass of antacid in sample: 1.5558 g Antacid tablet: 1.6010 g Composition of antacid: Aluminum hydroxide:...
Mass of antacid in sample: 1.5558 g Antacid tablet: 1.6010 g Composition of antacid: Aluminum hydroxide: 160 mg Magnesium carbonate: 105 mg Protocol A: Pipet a 10.00 mL aliquot of the antacid sample solution into a 125 mL Erlenmeyer flask followed by adding about 10 mL of the bicarbonate-carbonate buffer solution (pH 10.0 ± 0.1). Transfer quantitatively a 34.96 mL aliquot of standard EDTA solutioN, 0.01000 M, to the flask using a buret. Boil gently the mixture for 5 min....
A 25.0 mL aliquot of 0.0440 M EDTA was added to a 49.0 mL solution containing...
A 25.0 mL aliquot of 0.0440 M EDTA was added to a 49.0 mL solution containing an unknown concentration of V3+. All of the V3+ present in the solution formed a complex with EDTA, leaving an excess of EDTA in solution. This solution was back-titrated with a 0.0340 M Ga3+ solution until all of the EDTA reacted, requiring 11.0 mL of the Ga3+ solution. What was the original concentration of the V3+ solution?
To determine the Ca^2+ concentration in water sample, a standard EDTA solution of 0.01988 M was...
To determine the Ca^2+ concentration in water sample, a standard EDTA solution of 0.01988 M was used to titrate 25 ml. of the sample solution with the presence of an ammonium buffer (pH 10). If 15.80 ml. of the standard EDTA was used to reach the end point, calculate the molar concentration and the ppm concentration of the unknown Ca^2+ (atomic weight of Ca = 40.08g/mole) solution The amount of 0.2915g of benzoic acid was dissolved in 100 ml. of...
EBTA TItration Q3. A 1. volumetric flask. A 50.00-ml aliquot of the diluted solution was brought...
EBTA TItration Q3. A 1. volumetric flask. A 50.00-ml aliquot of the diluted solution was brought to a pH of 10.0 with a NH NH buffer; the subsequent titration involved both cations and required 28.89 ml of 0.06950 M EDTA. A secand 50.00-mL aliquot was brought to a pH of 10.0 with an HCN/NaCN buffer, which also served to mask the Cd? 11.56 mL of the EDTA solution were needed to titrate the Pb*, Calculate the percent Pb and Cd...
Please help! Will rate. A 50.0 mL sample containing Cd2+ and Mn2+ was treated with 56.5...
Please help! Will rate.
A 50.0 mL sample containing Cd2+ and Mn2+ was treated with 56.5 mL of 0.0600 M EDTA. Titration of the excess unreacted EDTA required 13.3 mL of 0.0100 M Ca. The Cd2t was displaced from EDTA by the addition of an excess of CN. Titration of the newly freed EDTA required 11.2 mL of 0.0100 M Ca2+. What are the concentrations of Cd2+ and Mn2+ in the original solution? M Mn2+ concentration: M Cd2 concentration: A...
10.7 10.00 mL of a solution of Hg2+ and 25.00 mL of 0.04516 M EDTA are added to 100 mL of pH 10 buffer. The resulting solution is titrated with 21.77 mL of 0.02385 M Mg2+ solution. What was the molarity of the Hg2+ solution? Report the answer with the correct number of significant figures.
A 24.34 mL aliquot of a Pb2 solution, containing excess Pb2+, was added to 11.50 mL of a 2,3-dimercapto-1-propanol (BAL) solution of unknown concentration, forming the 1:1 Pb2+-BAL complex. The excess Pb2+ was titrated with 0.0157 M EDTA, requiring 9.88 mL to reach the equivalence point. Separately, 39.89 mL of the EDTA solution was required to titrate 32.75 mL of the Pb2+ solution. Calculate the BAL concentration, in molarity, of the original 11.50 mL solution concentration:
6. (8) A 50.0 mL sample of hard water containing Ca2 was titrated with 0.0500 M EDTA standard solution at pH 10 and with Eriochrome Black T indicator. The endpoint was reached when 11.35 mL of EDTA was added a) (6) Calculate the concentration of Ca* in the unknown sample in moles per liter (M). b) (2) What is the pCa of the solution?
4. 50.0 mL of 0.00200 M Ca2 solution buffer at pH 10.0 is titrated with 0.00200 M EDTA. At equivalence point (i.e. 50.0 mL EDTA has been added), what is the equilibrium concentration of Ca2, [Ca2], and what is the pCa? The formation constant of CaY, Kaa 5.0 x 1010, and α4 of EDTA at pH 10.0 is 0.35
4. 50.0 mL of 0.00200 M Ca2 solution buffer at pH 10.0 is titrated with 0.00200 M EDTA. At equivalence point...
Answer units Save Question 7 (10 points) A 100.00 mL sample of hard water is to be titrated with 0.03505 M EDTA solution. A small amount of Mg2+ (that required 1.63 mL of EDTA to titrate as a blank solution) is added to the hard water sample. This sample requires 13.47 mL of EDTA to reach the endpoint. What volume of EDTA is used in titrating the Ca2+ in the hard water? Your Answer units Answer Save
To determine the Ca^2+ concentration in water sample, a standard EDTA solution of 0.01988 M was used to titrate 25 ml. of the sample solution with the presence of an ammonium buffer (pH 10). If 15.80 ml. of the standard EDTA was used to reach the end point, calculate the molar concentration and the ppm concentration of the unknown Ca^2+ (atomic weight of Ca = 40.08g/mole) solution The amount of 0.2915g of benzoic acid was dissolved in 100 ml. of...
EBTA TItration Q3. A 1. volumetric flask. A 50.00-ml aliquot of the diluted solution was brought to a pH of 10.0 with a NH NH buffer; the subsequent titration involved both cations and required 28.89 ml of 0.06950 M EDTA. A secand 50.00-mL aliquot was brought to a pH of 10.0 with an HCN/NaCN buffer, which also served to mask the Cd? 11.56 mL of the EDTA solution were needed to titrate the Pb*, Calculate the percent Pb and Cd...
Please help! Will rate.
A 50.0 mL sample containing Cd2+ and Mn2+ was treated with 56.5 mL of 0.0600 M EDTA. Titration of the excess unreacted EDTA required 13.3 mL of 0.0100 M Ca. The Cd2t was displaced from EDTA by the addition of an excess of CN. Titration of the newly freed EDTA required 11.2 mL of 0.0100 M Ca2+. What are the concentrations of Cd2+ and Mn2+ in the original solution? M Mn2+ concentration: M Cd2 concentration: A...
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