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- Explain the need of adding MgCl2 ° 6H2O to EDTA solution before standardization
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- Required: Normality of IodineA conductivity cell filled with a 0.01 M KCl solution was found to have a resistance of 189 ohms at 25oC. When filled with 0.01 M HCl solution, the cell gave a resistance of 64.8 ohms at the same temperature. At 25oC, the conductivity of 0.01 M KCl solution was 1.4088 x 10-3 S cm-1. Calculate (a) the cell constant and (b) the conductivity of the HCl solution. answer is [0.266; 4.105 x 10-3] please explain. thank you!To 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 mg10aFive white, 500-mg uncoated ascorbic acid (AA) tablets with an average weight of 0.6152-g were pulverized in a mortar. A sample of the powdered ascorbic acid weighing 0.4700-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 47.81-mL of 0.09640 N 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 2.73-mL of 0.09123 N 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. 293.3 mg 502.5 mg None of the choices 383.9 mg
- An impure sample of calcium carbonate with a mass of 7.95 g was reacted with 50.00 cm3 of 1.00 mol dm hydrochloric acid (an excess). The resulling solution was transferred to a volumetric flask and titrated with 11.10cm3 of 0.300 mol dm-3 sodium hydroxide solution. Determine the percentage purity by mass of the calcium carbonate sample.CaCO3 + HCl -> CaCl2 + H2O + CO2 HCl + NaOH -> NaCl +H2O a. Determine how many moles of hydrochloric acid were used.b. Determine how many moles of excess HCI was titratedc. Determine how much in moles calcium carbonate present in the sample.d. Calculate the mass of calcium carbonate presente. Determine the percentwge calcium carbonate is in the sample.In a beaker 20mL of 0.5M Ca(OH)2 and 80mL of 0.5M CH3COOH are mixed and then this mixture is added on 2g of active coal. After waiting for about 20 minutes the solution is filtered and the filter is titrated by 1M NaOH solution in the presence of an indicator. 10mL of the NaOH solution has been used. Calculate the amount of acetic acid adsorbed per gram of the coal in moles. Explain all the steps and reactions of the experimental process by your own comments.4. The %Mn in steel can also be determined spectrophotometrically by oxidizing the manganese to the intensely colored permanganate, MnO4-. Standard solutions of permanganate gave the following absorbances (in a 1 cm cell): ABSORBANCE CONC. OF MnO4 (g/mL) 0.210 1.05 x 10-5 0.315 1.61 x 10-5 0.429 2.21 x 10-5 0.599 2.98 x 10-5 0.801 4.04 x 10-5 The following samples of steel were thoroughly reacted to convert the manganese into permanganate and then diluted to 500.00 mL. WT. OF STEEL (g) ABSORBANCE 0.5886 0.611 0.3498 0.359 0.4555 0.482 Again using Excel, plot the calibration data and calculate the %Mn in the steel.
- A domestic water pipe is suspected to be contaminating drinking water with lead. In order to test this hypothesis, a section of the pipe is leached for 24 hours using 120.0 mL of 4% acetic acid. A 40.00-mL aliquot of the leachate is transferred to an electrochemical cell and 10.00 mL of a 0.200 mM standard solution of Cďd²+ is bo added (as an internal standard). A stripping analysis of the solution yields peak currents of 1.81 µA for lead and 2.18 µA for cadmium. Analysis of a standard solution that is 0.0600 mM in Pb2t and 0.0500 mM in Cd2+ gives peak currents of 2.39 µA and 2.71 µA, respectively, under the same conditions. What is the concentration of Pb²+ in the original leachate? 13.Determining Chemical Oxygen Demand You are given a 200-mL sample of surface water from Lake Ontario, and asked to determine the chemical oxygen demand (COD) of the sample. To do so, you reflux the sample with 15 mL of a 0.2M K,Cr,O, standard solution for 2 hours, then titrate the excess dichromate using 20.0 mL of a 0.3M Fe2 solution. What was the COD of the sample (reported in mol/L of O2)? Reminder: Cr30,2 consumes 6e", Fe2* offers le. A. The COD of the sample is 0.010 mol/L O2 B. The COD of the sample is 0.o08 mol/L O2 C. The COD of the sample is 0.015 mol/L O2 O D. The COD of the sample is 0.005 mol/L O2.1. (a) Calculate Eo’ for the process:AgI03(s) + e- ⇔ Ag(s) + I0 3-(b) Use the shorthand notation to describe a cell consisting of a saturated calomel reference electrodeand a silver indicator electrode that could be used to measure pIO3.(c) Develop an equation that relates the potential of the cell in (b) to pIO3.(d) Calculate plO3 if the cell in (b) has a potential of 0.294 V.