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- It is required to know the concentration of an aqueous solution of H2SO4 that appeared in the laboratoryChemistry III and it's unlabeled. To this end, a student of analytical chemistry carried out the followingProcedure: He took 5.00 mL of a fresh and standardized solution of 0.525M NaOH and brought them to a250.0 mL balloon to be completed with distilled water. Subsequently, he poured 15.00 mL of the solutionH2SO4 of unknown concentration in an Erlenmeyer flask and added 2 drops of phenolphthalein.Using a burette filled with the last NaOH solution, he noticed that when adding 39.40 mL of the hydroxidethe Erlenmeyer solution reached a faint but permanent pink. With the above dataDetermine the concentration and pH of the H2SO4 solution.If 50.0 mL of Thiosulfate solution are required to titrate the I2 liberated from an excess ofKI by 0.3000 grams of potassium Iodate, calculate (a) normality of the thiosulfate solution(b) value of each milliliter of Thiosulfate solution in terms of grams of I2.As solution was prepared by dissolving 5.76g of KCl.MgCl2.6H2O (277.85g/mol) in sufficient water to give 2.000L. calculate a. pMg for the solution b. pCl for the solution
- Calculate the volume of solution required to dissolve 65.1 g of C12H22O11(molar mass 342.34g/mol) to producers a solution with a molar it's of 1.12MA 600.0 mg sample consisting of only CaC2O4and Mg C2O4is heated at 500oC converting the two salts to CaCO3and MgCO3. The sample weighs 465.0 mg. If the sample had been heated at 900oC where the products are CaO and MgO, what would the mixture of oxides weigh? Show the clear and complete solutionWhile working in a metal processing facility, Letlen had accidentally mixed two metal vatstogether creating an alloy. One vat was labeled for cadmium, while the other was not. It canbe assumed that these are of pure metal composition. To identify this metal, Letlen took 1.000 g of the homogenous alloy sample composed ofcadmium and the unknown metal, dissolved, and diluted it to exactly 100.0 mL in avolumetric flask. A 20.00-mL aliquot was taken and titrated this using 22.82 mL of 0.05000M EDTA. In a second 20.00-mL aliquot, the Cd was masked through the addition of HCN/NaCN buffer.The titration of the unknown metal in the aliquot required 15.13 mL of EDTA.MW: Cd (112.411 g/mol) a. Calculate the moles of Cd and the moles of unknown metal in the 20.00-mL aliquot.b. Calculate the moles of Cd and the moles of unknown metal in the sample.
- The volume of water needed to dissolve 0.0724 grams of calcium chromate is ________ L.Assume no volume change upon addition of the solid.How many grams of Ag2CO3 will be soluble in 250 ml of 0.180 M AgNO3? (Ksp of Ag2CO3 = 5.95 x 10-10)Five drops of dichlorofluorescein have been added to a solution containing 0.800 g sample which required 25.30 mL of 0.100 M AgNO3. (c) Calculate the weight percent NaCl in the original sample.
- You are given an 18% solution of sodium imidazole. What mass of imidazole (in g) would be in 20 mL of this solution? a. You need to use the sodium imidazole stock solution from Q11 to make a dilute imidazole solution (final volume 180 mL) at a final concentration of 0.2 M. The molecular weight of imidazole is 90 g/mole. What volume of imidazole stock would you use (mL)? b. You need to use the sodium imidazole stock solution from Q11 to make a dilute imidazole solution (final volume 180 mL) at a final concentration of 0.2 M. The molecular weight of imidazole is 90 g/mole. What volume of water would you add (mL)?One gram of sodium hydroxide (NaOH) is used to adjust the pH of an aqueous solution (200 gallons) thatcontains 10 lbs of finely ground rhodochrosite (MnCO3) ore. Does the NaOH raise or lower the solutionpH? What is the amount of NaOH added in lbs/ton? What is the molarity (mol/l) of the system? Assumingthe NaOH is completely soluble and the system is at room temperature, what is the solid-to-liquid ratio(wt%) of the system?slove Part BFor the same procedure described in the chemical equilibrium lab handout for determining K, 27.0 mL of organic solution was added to 65.0 mL of KI aqueous solution at 317.1 K. Both the aqueous and organic solutions were prepared at 298.15 K with the apparent concentration of 0.0796 M for the I-(aq) and 0.0065 for the I2(org) solutions, respectively. After mixing these immiscible solutions, the final concentration of I2 in the organic layer was determined to be 0.0006 M through UV-Vis spectroscopy. In a separate experiment, the partition coefficient was found to be k = 0.01 at 317.1 K. a) Determine the approximate equilibrium constant, K, without making any temperature correction, for the reaction: I2(aq) + I-(aq) ⇌ I3-(aq) at 317.1 K. K = 5294.4 b) Now, make the temperature correction for volume expansion in the calculation of K assuming the solvent is Cyclohexane. What is the percentage error for using the non-corrected K rather than the corrected K?