A foot powder sample containing Zn was dissolved on 100.00 mL water and was titrated to the end point color with 22.57 mL of 0.01639 M EDTA at pH=4. (a4= 3.61x10-9, KZnY2- = 3.2 x 1016). The pzn in the sample is: Please fill in the space with a numerical value with two digits or two decimal places without units
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- A foot powder sample containing Zn was dissolved on 50.00 mL water and was titrated to the end point color with 22.57 mL of 0.01639 M EDTA at pH=4. (α= 3.61x109, KKzny2 = 3.2 x 1016). The pZn in the sample is:A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCl, evaporated to incipient dryness and quantitatively transferred to a 250 mL volumetric flask, and diluted to mark. A 10 mL of aliquot was then transferred to an Erlenmeyer flask, together with 5mL buffer and 5 drops of EBT indicator, and was used to standardize the EDTA titrant. The solution turned blue after the addition of 24.10 mL of EDTA. A blank correction was performed and was determined to be 0.4 mL. What is the concentration of EDTA obtained (MW CaCO3 = 100.0869 g/mol)?A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCl, evaporated to incipient dryness, and quantitatively transferred to a 250 mL volumetric flask and diluted to mark. A 10 mL of aliquot was then transferred to an Erlenmeyer flask, together with 5mL buffer and 5 drops of EBT indicator, and was used to standardize the EDTA titrant. The solution turned blue after the addition of 24.10 mL of EDTA. A blank correction was made and was determined to be 0.4 mL. [Analysis] A 30 mL unknown water sample was treated with 37.6 mL of EDTA. A blank correction was made and was determined to be 0.4 mL. What is the concentration of Ca2+ (40.0780 g/mol) in ppm?
- (i) You have been provided with a sample collected from a water pool beside a slag heap at the iron ore mine. 35 uL of the sample is added to 1165 uL of buffered ferrozine (excess). If the %T recorded at 562 nm in a 2 mm cuvette is found to be 25%, calculate the concentration of Fe(II) in the sample in mol L−1 and ppm. Comment on the contamination level. (ii) Comment on a possible contaminant that could interfere with the assay and suggest an approach that could be used to account for its presence.In an unprecedented initiative, the professor chose you to carry out the determination of a special sample in order to verify the inherent indication system. For that, an aliquot of 25.00 mL of a solution containing Fe(III) salts was titrated with EDTA 0.00982 mol/L, using potassium thiocyanate as indicator. In this case, you have found the volume of 31.10 mL of titrant to End Point. Based on the information given in the table, choose the option that best describes/explains the process linked to the indication system of the Final Point of the degree: (a) The indication of the system will be given by the disappearance of the reddish coloration, due to the displacement reaction: Fe(III) complex with EDTA is formed in detriment of the Fe(III) complex with thiocyanate. (b) The indication of the system will be given by the appearance of a reddish color, in function of the displacement reaction: Fe(III) complex with thiocyanate is formed in detriment of the Fe(III) complex with EDTA. (c) The…Calculate the pZn2+ for solutions prepared by adding 0.00, 5.00, 10.00, 15.00, 20.00, 25.00and 30.00 mL of 0.0100 M EDTA to 25.00 mL of 0.00250 M Zn2+. Assume that both the Zn2+and EDTA are 0.0100 M in NH3 to provide a constant pH of 9.0 Zn(NH3)n2+: pKfn, = 2.21, 2.29, 2.36, 2.03ZnY2-: Kf = 3.0 x 1016EDTA: Ka1 = 1.02 x 10-2 , Ka2 = 2.14 x 10-3 , Ka3 = 6.92 x 10-7 , Ka4 = 5.50 x 10-11
- The amount of iron in a meteorite was determined by a redox titration using KMnO4 as the titrant. A 0.4185 -g sample was dissolved in acid and the liberated Fe3+ quantitatively reduced to Fe2+, using a reductor column. Titrating with 0.0051 M KMnO4 requires 23.44 mL to reach the end point. Determine the %w/w Fe2O3 in the sample of meteorite. (Fe = 55.845 amu, Fe2O3 = 159.69 g/molA 1.509-g samle of a Pb/Cd alloy was dissolved in acid and diluted to exactly 250.0 mL in a volumetric flask. A 50.00-mL aliquot of the diluted solution was brought to a pH of 10.0 with an HCN/NaCN buffer, which also served to mask the Cd2+; 11.56mL of the EDTA solution were needed to titrate the Pb2+. Calculate the percentage of Pb and Cd in the sample.The concentration of ammonia in a cleaning product was determined by back titration.Firstly, 10.00 cm3 of the cleaning product was pipetted into a large conical flask,containing 250.00cm3 of 0.50 mol/l HCl to give Solution A.Following a period of reaction and shaking, 50.00cm3 of Solution A was removed anddiluted to 250 cm3 with water in a volumetric flask to give Solution B.20 cm3 samples of Solution B were titrated against 0.05 mol/l Na2CO3 solution, givingan average titre of 12.45 cm3. i) Write equations for the reactions that have taken place.ii) Determine the concentration of NH3 in the original cleaning product in mol/l,g/l, ppm, and % w/v.
- 50 mL of a solution of 0.0200 M Zn2+ will be titrated with 0.0100 M EDTA in 0.0100 M NH3 at pH 6.0. Ethylenediaminetetraacetic acid (EDTA) can be considered as a tetraprotic acid (H4Y). The stepwise acid dissociation constants are: K1 = 1.02 x 10-2, K2= 2.14 x 10-3, K3 = 6.92 x 10-7 and K4 = 5.50 x 10-11. The alplia value of the un-deprotonated species in a solution buffered to a certain pH is given by the following equation: a0 = [H+]4/([H+]4 + K1[H+]3 + K1K2[H+]2 + K1 K2K3[H+] + K1 K2K3K4) Calculate the alpha value of the fully deprotonated species (Y4- ) in a solution buffered to a pH of 6.0.A 5.323 g of dried eggshell is transferred to a 250-mL beaker and dissolved in 25 mL of 6 M HCl. The mixture was filtered and transferred into a 250 mL volumetric flask and diluted to the mark. A 20.00-mL aliquot is placed in a 125-mL Erlenmeyer flask and buffered to a pH of 10. The mixture was titrated with 0.04992 M EDTA and 43.25 mL was consumed to reach the end point. Determine the amount of calcium in the eggshell as %w/w calcium carbonate.Six iron tablets containing FeSO4.7H2O were dissolved in 100-ml of 0.1M HNO3 with gentle heating. All of the Fe2+ is converted to Fe3+ by the strong oxidizing conditions. After the solution had cooled to room temperature , 2.5-ml of 35wt% NH4OH was added. The precipitate Fe2O3-xH2O that was filtered weighed 0.345g. Thermogravimetric analysis of the crude product showed a 10.5% weight loss . A. How many waters of hydration were in the precipitate B. How much iron is present in each tablet