The thiourea in a 1.455 g sample of organic material was extracted into a dilute sulfuric acid solution and titrated with 37.31 mL of 0.009372 M Hg2+ via reaction: 4(NH2)2CS + Hg2+ →[(NH2)2CS]4 Hg2+
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The thiourea in a 1.455 g sample of organic material was extracted into a dilute sulfuric acid solution and titrated with 37.31 mL of 0.009372 M Hg2+ via reaction: 4(NH2)2CS + Hg2+ →[(NH2)2CS]4 Hg2+
- Is this an example of total analysis technique or concentration technique? Explain.
- Calculate the percent (NH2)2CS ( 76.12 g/mol) in the sample.
- What is classification of the analysis based on the amount of sample and amount of analytes present? Explain.
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- A student performed three KHP titrations in Part 1 in order to standardize their NaOH solution. They reported the following measurements: Mass of KHP + Vial Mass of 'Empty' Vial Final Burette Reading Initial Burette Reading Determination #1 16.7538 g 16.2649 g 21.67 mL 0.40 mL Determination #2 14.1709 g 13.5560 g 26.98 mL 0.31 mL Determination #3 15.6625 g 15.0833 g 26.04 mL 0.93 mL How many moles of KHC8H4O4 did they use in their second titration? Report your answer to the correct number of significant figures and only report the numerical value (no units).Silver nitrate can be standardized using primary standard KCl. A dried sample of analytical grade KCl of mass 0.918 g was dissolved and diluted to 250.0 mL. Repeat 10.00-mL aliquots of the potassium chloride solution were titrated with the silver nitrated solution. The mean corrected titration volume was 8.98 mL Calculate the molarity (M) of the silver nitrate solution.In order to form Ba(IO3)2, 500 mL of 0.5000 M Ba(NO3)2 was mixed with 500 mL of 0.0500 M NaIO3. Ksp= 1.57x10^-9 How many millimoles of Ba(NO3)2 are needed to completely react with NaIO3? 500 mmol 250 mmol 25 mmol 12.5 mmol What is the concentration of the excess reagent? 0.1125 M 0.3219 M 0.1195 M 0.2375 M What is the molar solubility of Ba(IO3)2 in this solution? 04x10^-5 M 07x10^-5 M 15x10^-5 M 30x10^-5 M
- In order to form Ba(IO3)2, 500 mL of 0.5000 M Ba(NO3)2 was mixed with 500 mL of 0.0500 M NaIO3. Ksp= 1.57x10^-9How many millimoles of Ba(NO3)2 are needed to completely react with NaIO3?What is the limiting reagent?What is the excess reagent?A set of five solutions are prepared by delivering 10 mL of unknown sample and increasing volumes of standard (0, 5, 10, 15, and 20 mL) into 50-mL volumetric flasks. Analytical reagents are then added and the flasks are diluted to volume. The x-intercept of the best-fit line is -5.63 mM. What is the concentration of the unknown? w 22+ as (6) A sample of an ore was analyzed for Cu* follows. A 1.25 g sample of the ore was dissolved in acid and diluted to volume in a 250 mL volumetric flask. A 20 mL portion of the resulting solution was transferred by pipet to a 50 ml volumetric flask and diluted to volume. An analysis showed that the concentration of 2+ Cu* in the final solution was 4.62 ppm. What is the weight percent of Cu in the original ore?
- The thiourea (NH2)2CS in a 1.600 g sample of an unknown organic material was extracted into a dilute acid solution and was titrated with 42.50 mL of 0.0010 M Hg2+. Equation: 4 (NH2)2CS + Hg2+ → [(NH2)2CS]4Hg2+ Find the percentage thiourea present in the sample.You were assigned to assay a product sample of milk of magnesia. A 0.600-g sample was reacted with 25.00 mL 0.10590 N H2SO4 . The excess unreacted acid in the solution required 13.00 mL of 0.09500 N NaOH when titrated to reach the methyl red end point. Determine the dosage strength of the product in terms of % Mg(OH)2 content. Type your answer in 2 decimal places, numbers only.5 The amount of ascorbic acid, C6HSO6, in orange juice was determined by oxidizing the ascorbic acid to dehydroascorbic acid, C6H6O6, with a known excess of I3, and back titrating the excess Is with Na2S2O3. A 5.00-mL sample of filtered orange juice was treated with 50.00 mL of excess 0.01023 M I3. After the oxidation was complete, 13.82 mL of 0.07203 M NazS2O3 was needed to reach the starch indicator end point. Report the concentration of ascorbic acid in milligrams per 100 mL.
- CHARACTERIZATION OF A WEAK ACID In this experiment, we shall perform a titration of an unknown weak acid (HX(aq)) with NaOH (aq) a strong base. The net ionic equation of the titration reaction is: HX(aq) + OH(aq) à H,O(I) + X(aq) The identity of the unknown can be determined by comparing its experimental molecular weight and pKa to the molecular weights and pKa of the weak acids shown in the table I. EXPERIMENT Determination of Molecular weight: Approximately 0.3 grams of unknown acid is dissolved in 70.0 mL deionized water. The unknown acid solution is then titrated with 0.123 M NaOH (aq). 50 • Initial volume of NaOH in the burette = mL 32 • Final volume of NaOH in the burette = mL • Volume of NaOH used to complete the titration = Number of moles of NaOH added = 13 135.50 g/mol • Number of moles of unknown acid present MOLECULAR WEIGHT OF UNKNOWN ACID = Determination of pKa of the weak acid: 9,93A 5.0 g sample containing a pesticide with molecular formula [C14H9Cl5], was decomposed with metallic sodium in alcohol, and the liberated chloride ion was precipitated as AgCl. (i) Express the results of this analysis in terms of percent based on the recovery of 0.1606 g of AgCl. (ii) Convert your answer (g/g) to ppm.A researcher reconstituted a vial of 750 mg Cefuroxime Sodium Powder for Injection with 6mL of sterile water for injection. The reconstituted solution was dark amber-colored solution. The package insert states that solution colors range from clear to yellow depending on concentration, diluent, and storage conditions. The researcher was then hesitant to give the patient the solution due to its unusual dark color. Five portions were taken from a batch of cefuroxime sodium. Prior to testing in the instrument, each part was subjected to one of the following conditions: Conditions Specifications Temperature Portion 1: 8°C ± 2°C Portion 2: 30°C ± 2°C Portion 3: 40°C ± 2°C Light Portion 4: Kept in the dark Portion 5: Exposed to direct sunlight 1. Of the several solutions prepared, which absorbance value results should be compared with each other to answer the questions of the pharmacist? Explain your answer.