c. An Analytical laboratory at SMU has a bottle of concentrated HCI solution labelled, specific gravity of 1.2g/cm and which is 37% (w/w) HCI. M(HCI)= 36.46g/mol. From this 0.6mol,was carefully pipetted out into a 100ml standard flask and made up to the mark. Exactly 0.350g of pure sodium carbónate (Na CO3) M =105.988g/mol was dissolved into the above 100ml made up solution of HCI and the following reaction óccurred: Na2CO3 + 2HCI - 2NACI + CO2(g) + H20 i. What is the molar concentration of this HCI solution What is the resultant concentration of HCI in 100ml
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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+ P.S. Answer only the last two letters of the following questions. (Only C and D) a. Is this an example of total analysis technique or concentration technique? Explain. b. Calculate the percent (NH2)2CS ( 76.12 g/mol) in the sample. c. What is classification of the analysis based on the amount of sample and amount of analytes present? Explain. d. If the true value is 10.00%, calculate the absolute and relative error.A student was tasked to perform gravimetric analysis of a soluble sulfate. His unknown sample weighed 0.7543 g. The sample underwentprecipitation using BaCl2 and was digested for overnight. The precipitate was then filtered off to obtain white crystalline precipitate that was collected inan ash less filter paper. In performing constant weighing, he obtained a crucible mass that is 29.9442 g. After burning his samples inside the crucible,the obtained mass was 30.3375 g. Compute for the theoretical % SO3 obtained by the student and the theoretical mass (g) of SO3 that should be obtained by the student using his weighed sampleA student was tasked to perform gravimetric analysis of a soluble sulfate. His unknown sample weighed 0.7543 g. The sample underwentprecipitation using BaCl2 and was digested for overnight. The precipitate was then filtered off to obtain white crystalline precipitate that was collected inan ash less filter paper. In performing constant weighing, he obtained a crucible mass that is 29.9442 g. After burning his samples inside the crucible,the obtained mass was 30.3375 g.29. Compute for the mass (g) of BaSO4 from the experiment.A) 0.3933B) 0.3393C) 0.3133D) 0.3951E) 0.359130. Compute for the experimental mass (g) of SO3 in grams obtained by the student.A) 0.1439B) 0.1349C) 0.1943D) 0.1394E) 0.359131. Compute for the experimental % SO3 obtained by the student.A) 73.21B) 56.33C) 17.89D) 56.89E) 72.8032. Compute for the theoretical % SO3 obtained by the studentA) 0.3933B) 56.37C) 17.33D) 17.89E) 0.425233. Compute for the theoretical mass (g) of SO3 that should be obtained by the student…
- 1. A 1.2-gram sample of lanolin was treated with Wij’s solution and excess potassium iodide solution. The liberated iodine reacted with 30 ml of 0.1 N sodium thiosulfate solution. If the iodine value was determined as 12.69, what is the volume used in blank titration? 2. A fat sample with combination of acids contain standard hydrochloric acid for blank and sample with 8mL and 5mL respectively. The normality of the standard hydrochloric acid is 0.93N and the weight of the sample is 3 grams. Calculate the saponification value. 3. A 3.50-gram sample of Streptomycin powder was tested for its water content. If the water equivalence factor of the KF reagent was 4.6, what is the percentage water content of the sample if 9.2 ml of the KF reagent was used? 4. A 500mg oil sample is taken from a conical flask and is dissolved in 50mL distilled alcohol. An indicator is added and is then titrated against 0.112N KOH until a slight pink color appears. It took 17.6mL of the titrant to reach the…A 500ml solution of NaOH was made using 2g of NaOH(s) Three trials of titration were made with using KHP(s) as the acid dissolved with about 25ml of deionized water and 4 drops of phenolphthalein indicator. Slowly adding the NaOH solution until the clear solution had turned pink which would give us our end point and allow us to find the NaOH molarity by equivalence point. Trial 1: - 0.484g of KHP were used - initial volume of buret containing NaOH solution was 0.0 ml - final volume of buret was 23.60ml Trial 2: - 0.485g of KHP were used - initial volume was 0.0ml - final volume was 24.00ml Trial 3: - 0.486g of KHP - initial volume was 0.0ml - final volume was 23.80ml The molarity of NaOH was found by using the moles of KHP(as at equivalence, both solutions are balanced in moles) divided by the total volume of NaOH used to neutralize the solution. Giving us 0.100M for trial 1, 0.099M for trial 2, and 0.100M for trial 3. Make a rough sketch of a titration curve that…The standard addition method is used to analyze a sample of a river water for mercury. Solution A is made by pipetting 5.00 mL of undiluted sample in to a 10 mL volumetric flask and filling to the mark with DI water. Solution B is made by pipetting 5.00 mL of undiluted sample and 3.00 mL of 15.0 ppb of Hg standard into same 10.0 mL volumetric flask and filling to the mark with DI. Solution A and B are analyzed using atomic absorption spectroscopy and give a percent transmittance values of 56 % and 33 % respectively (not blank corrected). A blank has a transmittance of 96%. What is the corrected absorbance of both solution A and B? A. Solution A: 0.123 Solution B: 0.463 B. Solution A: 0.463 Solution B: 0.234 C. Solution A: 0.123 Solution B: 0.234 D. Solution A: 0.234 Solution B: 0.463
- A student determined the concertration of NaOCI in a commercial bleach sample using the same technique described in section "F" of the Halogens and Their Compounds lab. The student required 18 drops of 0.01M Na25203 to reach the end point. What is the concentration (reported in percentage) of NaOCI in the bleach sample?1. 1093-g sample of impure Na2CO3 was analyzed by residual precipitimetry. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back-titrated with 0.05781 M KSCN, requiring 27.36 mL to reach the endpoint. The percentage Na2CO3 (MW = 106.0 g/mole) in the tested sample is ________ % ? Note: Express final answer using least number of significant figures. 2. The alkalinity of natural waters is usually controlled by OH- (MW = 17.01 g/mole), CO3-2 (MW = 60.01 g/mole), and HCO3- (MW = 61.01 g/mole), which may be present singularly or in combination. Titrating a 10.0-mL sample to a phenolphthalein endpoint requires 38.12 mL of a 0.5812 M solution of HCl, and an additional 18.67 mL of the same titrant to reach the methyl orange endpoint. The composition of the sample is _________% CO3-2 and ___________ % OH- Note: Express final answers using least number of significant figures.The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g Volume of H2C2O4•2H2O solution = 250.0mL What is the Molarity H2C2O4 standard solution ?
- Please determine how to make a working standard Solution of about 0.010mg/mL. Caffeine will be the active. Diluent will be water.Aspirin powder = 0.8110g MW of Aspirin = 180g.mol-1 Volume of 0.5N HCl consumed in back titration = 23.50mL Volume of 0.5N HCl consumed in blank titration = 44.50mL Percent purity (USP/NF) = Aspirin tablets contain NLT 90.0% and NMT 110.0% of the labeled amount of aspirin (C9H8O4) What is the calculated weight (in grams) of pure aspirin?..Calculate the mass percent of the ascorbic acid in the same show full solution Situation: The pounded Vitamin C tablet was half into two below are the calculated data in the experiment. Each of the half are transfered in a 250ml erlen meyer flask and added 75ml of deionized water for the vitamin C to dissolve. Then it was prepared for titration where the burette was filled with 0.09794M standardize NaOH solution then a total of with 3 drops 2% phenolphthalein indicator was added to each erlen meyer flask l, swrill it and begin the titration. below are the following data gathered: Vitamins used: Nature Made vitamin C 500mg tablet Trial 1 Mass: 0.3108g of Vitamin C tablet Initial volume: 1.6mL Final volume: 15.4mL Trial 2 Mass: 0.3349g Initial volume: 15.4 mL Final volume: 30.2 mL