Calculate the mole fraction(x) of acetic acid in a mixture consisting of 150 gm acetic acid , and 138 gm ethyl alcohol ? Note ( M.wt (acetic acid) = 60 g/mole & M.wt (ethyl alcohol) = 46 g/mole ) * %3D O 0.45 m O 45 m O 10 m 0.1 m
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- A Fajans titration of a 0.7908-g sample required 45.32 mL of 0.1046 M AgNO3 . Express the results of this analysis in terms of the percentage of BaCl2 * H2O. (Use a MW value in 4 decimal places)The Kjedahl procedure was used to analyze 256 µL of a solution containing 37.9 mg protein/mL. The liberated NH3 was collected in 5.00 mL of 0.033 6 M HCl, and the remaining acid required 6.34 mL of 0.010 M NaOH for complete titration. What is the weight percent of nitrogen in the protein? wt%1. What is the molar solubility of PbCl2 in a solution of 0.23 M CaCl2? Ksp = 1.6 ✕ 10-5 for PbCl2. 2. What is the Qsp when 32.0 mL of 6.50 ✕ 10-7 M Na3PO4 are mixed with 41.4 mL of 5.50 ✕ 10-5 M CaCl2? Assume the volumes are additive. Ksp = 2.0 ✕ 10-29. 3. What is the Qsp when 61.0 mL of 1.50 ✕ 10-4 M AgNO3 are mixed with 80.0 mL of 5.20 ✕ 10-3 M CaCl2? Assume the volumes are additive. Ksp = 1.6 ✕ 10-10. 4. What [I-1] is needed to start the precipitation of AgI from a saturated solution of AgCl? Ksp = 2.9 ✕ 10-16 for AgI and Ksp = 1.2 ✕ 10-10 for AgCl.
- PART 2: A solution is prepared by mixing 150.0 mL of 0.0010 M magnesium nitrate and 250.0 mL of 0.100 M sodium fluoride (Ksp = 7.4x10-11). Is Ksp greater than , equal to, or lower than Qsp? Will a precipitate form, Y/N? What is the fluoride ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3). What is the magnesium ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3).A suitable target for the titration is 30.0 cm3 of 0.025 moldm-3 Br2(aq) Justify why a much smaller target titre would not be appropriate Calculate the amount in moles of bromine in the target titer Justification? calculate a suitable massof alive oil to transfer to the volumetric flask using your answer to of above question and the structure of Y Assume that the olive oil contains 85/- of Y by mass (If you were unable to calculate the amount of bromine in the target titer,you should assume it is 6.25×10^-8 mol .this in not the correct amount)The molar solubility of MgCO3 (Ksp = 3.50 x 10-8) in distilled water at room temperature is ______ M. Titration of a 50.00-mL aliquot of the saturated solution will require ______mL of 0.005000 M HCl to reach the phenolphthalein endpoint.
- 1 ) The density of a 5.26MNaHCO 3 (84.0 g/mol) is 1.19g / m * l . Its molality is 2) Calculate the pAg^ + at the equivalence point in the titration of 25.0ml of 0.0823 M Kl with 0.051M AgNO 3 . Ksp Agl=8.3*10^ -16 3) Commercial concentrated aqueous nitric acid is 70.4% HNO3(63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is 4) Consider the titration of 25ml of 0.0823M KI with 0.051M AGNO3, Kspagi =8.3x10-16 Calculate pAg* after adding 39.0 ml I03 Ag* + 103 ====AglO3 5) Commercial concentrated aqueous nitric acid is 70.4 1\%HNO 3 (63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is: 6) What mass in g of Na 2 CO 3 [106 g/mol] is required to prepare 250 ml of 0.3M aqueous solution in Na^ + [23.g/mol] ? 7) Calculate pAg^ + after adding 42.30ml AgNO 3 In the titration of of 0.0823M Kl with 0.051M AgNO 3 . KspAgl = 8.3 * 10 ^ - 16 8) The milliliters of concentrated HClO 4 (100.5 g/mol),6 60% by mass,…In how much volume of diluted sulfuric acid should you dissolve a multivitamin tablet of approximately 1700 mg of Vitamin C to back analyze 10.00 mL of that solution, with 25.00 mL of 0.01 M KIO3 and 0.04 M thiosulfate to use approximately 8-10 mL of titrant ? You have 25, 50, 150, 250 and 500 mL flasks.pls complete table given the data Determination of Ksp and Molar Solubility1. Add Ca(OH)2 to 250.0 mL distilled water with stirring until equilibrium is achieved. 2. Filter the undissolved precipitate. Measure out 50.0 mL of the supernate into a 250-mL Erlenmeyer flask using a pipette.3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved.4. Record the volume the HCl solution used. Perform two more trials.
- What is the solubility of calcite (CaCO3) in grams per milliliter at a temperature at which its Ksp is 9.93×10-9?How many grams of potassium napthenate (KC11H7O2; MW=210.27 g/mole; Kb=85x10-10) must be added to 50.0 ml of 0.4 M Naphthenic acid (HC11H7O2; Ka=5.4x10-5) to obtain a buffer with pH 5.0?The next 11 questions are related to the titration of 30.00 mL of a 0.1000 M acetic acid solution with 0.0800 M KOH. Assume that the temperature is 25 oC.What is the initial pH of the analyte solution? What volume of KOH is required to reach the equivalence point of the titration? How many mmol of acetate are present at the equivalence point? Report the analytical amount, not the equilibrium amount of acetate at the equivalence point. What is the total volume of the solution at the equivalence point?