A pharmacist is conducting an analysis of 2.7 g sodium bicarbonate and titrated with 26.05 mL of 0.9987 N HCl. What is the potency or percent assay of sodium bicarbonate? Did it pass the USP requirement? ROUND-OFF TO 2 DECIMAL PLACES. Answer = _% Disposition (Passed or Failed) = _
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- A commercial vinegar was analyzed by titration to determine the percent acetic acid. Briefly, 10.00 mL of vinegar sample was diluted to 100. mL solution in a volumetric flask. A 25.00 mL aliquot from the diluted vinegar required 25.55 mL of 0.1005 M sodium hydroxide to reach the phenolphthalein endpoint From this experiment which is the standard solution used in titration? CH3COOH NaOH NaCH3COO C20H14O4A 50.0 mL of 0.100 M Cu(NO3) solution and a 50.0 mL of 0.100 M NaBr solution are mixed. If the Ksp of CuBr is 5.30 x 10-9, which of the following is correct? a. CuBr will precipitate out of solution. b. CuBr will not precipitate out of solution. c. Cu(NO3) will precipitate out of solution. d. Cu(NO3) and NaBr will precipitate out of solution.A local company sent you their green alternative for window cleaner to be tested for percent (w/v) acetic acid content. For your experiment, you first standardized your NaOH titrant with 0.8053 g of (99.80 % purity) KHP. You used 40.60 mL of NaOH for your standardization. After that you then analyzed a 10.00 mL sample and found that you needed 43.20 mL NaOH to reach the end point. Summary of results: Standardization Sample analysis KHP Weight (g) 0.8053 g Volume of sample 50.00 mL Purity 99.80% NaOH (mL) used 33.20 mL NaOH (mL) used 40.60 mL Determine the following: Molarity of NaOH % (w/v) acetic acid
- Calculate the percent difference in the two values for the molarity of the NaOH solution by: %Difference =[M1-M2]\Mavg x100% Given: 1st value for the molarity of NaOH = 0.0647 M 2nd value for the molarity of NaOH= 0.2627 M NaOH vs H2SO4 Burette solution is NaOH and the pipette solution is 10.0 mL of 0.205 M H2SO4 Titration Initial burette reading Final burette reading Volume of NaOH consumed Average volume of NaOH Approximate 0.0 mL 31.8 mL 31.8 mL 31.7 mL Titration 1 0.0 mL 31.5 mL 31.5 mL Titration 2 0.0 mL 31.7 mL 31.7 mL To find the average volume Average volume = 31.8 mL + 31.5 mL + 31.7 mL331.8 mL + 31.5 mL + 31.7 mL3 = 31.7 mL NaOH vs CH3COOH Burette solution is NaOH and the pipette solution is 5.0 mL of Vinegar Titration Initial burette reading Final burette reading Volume of NaOH consumed Average volume of NaOH Approximate 0.0 mL 20.1 mL 20.1 mL 20.3 mL Titration 1 0.0 mL 20.9 mL 20.9 mL Titration 2 0.0 mL 20.0 mL…A pharmacist is identifying the saponification value of corn oil in the lab. She weighs 1.8 g of corn oil and saponified with 25 mL of 0.4 N KOH which require 9 mL of 0.5N HCl to titrate the excess KOH. She performs blank determination, 20 mL of 0.5 N HCl was required to titrate the corn oil. What is the saponification value of the corn oil? Does the sample comply with the USP requirement? Use this formula to work your result Saponification Value = (Vblank - Vsample)N of HCl56.11/Sample weight (g)1. If Mg(OH)2 has a Ksp of 7.0 × 10–6, then what is the solubility of Mg(OH)2 in pure water? Give your answer in units of g/L. Express the answer to 4 significant digits and do not use scientific notation. *Use the Ksp given here. Do not look up your own value. 2. 200.0 mL of 0.005 M Na2CO3 are added to 200.0 mL of 0.002 M MgCl2. Does a precipitate form? [Ksp(MgCO3) = 6.82 × 10–6] Question 2 options: No, because Q = Ksp. Yes, because Q > Ksp. No, because Q < Ksp. No, because Q > Ksp. Yes, because Q < Ksp. 3.In order for a precipitate of PbBr2 to form, what is the minimum concentration of Br- that must be present in a solution of 0.00050 M Pb(NO3)2. The Ksp of PbBr2 is 2.20 × 10–6.
- Assume that the molarity of the standardized KMnO4 solution is 0.025 M and it takes 23.00 mL to reach the endpoint when titrating a dilute sample of H2O2. How many moles of H2O2 are in the diluted sample initially? Group of answer choicesDr. Donwonree tried to determine the vitamin C content in apple juice which he bought at CheMarket. He measured out 50.0 mL of the juice and added the HCl, KI, and starch. Then he started the titration by adding KIO3 solution into the juice. The concentration of the KIO3 solution was 0.200 M and it took only 1.50 mL of KIO3 to reach the endpoint. How much vitamin C (mg) is contained in 1.00 L of this apple juice?If you are making 500 ml of a stock solution of 10X PBS pH7.4 please tell me how much of each component you would need to add if the appropriate concentrations of 1x PBS are: 1x PBS Solution Concentrations: NaCl: 137 mM KCl: 2.7 mM Na2HPO4: 10 mM KH2PO4: 1.8 mM MW NaCL= 58.44 g/mol MW KCl = 74.55 g/mol MW Na2HPO4= 141.96 g/mol MW KH2PO4= 136.09 g/mol You should also describe the step by step process of making the solution.
- 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,…From a 1000 ppm stock solution of Pb2+, 10 mL are pipetted into a 1000 mL volumetric flask, which is then filled with water. From this new solution, 25 mL are pipetted into a 100 mL flask, which is then filled with water. What is the concentration of the final solution?Zhongli is a speleologist tasked to analyze the CaCO₃ content of a limestone stalactite. A 5.0000-g sample was dissolved in 25.00 mL of 1.350 M HCl, it was then heated to expel any CO₂ formed. The excess HCl was titrated to a phenolphthalein end point, it used 37.50 mL of 0.1200 M NaOH. How many moles of HCl was added initially to digest the limestone sample? How many moles of CaCO₃ is present in the limestone sample? What is the purity of the limestone in terms of %w/w CaCO₃?
