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Show your complete solution and round-off your answers to four decimal places.
A 0.1093-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of 0.06911 N AgNO3, the sample was back titrated with 0.05781 N KSCN, requiring 27.36 mL to reach the end point. Calculate the % purity of the Na2CO3 sample.
Answer = _% Na2CO3
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- The grid has six lettered boxes, each of which contains an item that may be used to answer the questions that follow. Items may be used more than once and there may be more than one correct item in response to a question. Place the letter(s) of the correct selection(s) on the appropriate line. Could dissolve Zn(OH)2 _____________ Could be used to prepare a buffer from __________ Halfway to the equivalence point in the titration of a weak, monoprotic acid with strong base ________ SO2-related atmospheric phenomenon __________ Species formed by a Lewis acid-base reaction ________ General condition required for precipitation to occur ________ [conj. base] = [conj. acid] in a buffer ___________1. A sample of pure sodium oxalate, Na2C2O4 , weighing 0.2856 g is dissolved in water, sulfuric acid is added, and the solution titrated at 70°C , requiring 45.12 mL of a KMNO4 solution. The end point is overrun and back-titration is carried out with 1.74 mL of a 0.1032 N solution of oxalic acid. Calculate the normality of the KMNO4 solution. Hint: A redox reaction is involed between oxalate and permanganate. Look at the changes in oxidation state by determining the balanced redox reaction: 5C20,2 + + 2MN2+ 2 Mn04 + 10H* → 10CO2 + 8H20A 15.00 g sample containing mixed alkali and other inert components was dissolved and diluted to 300 mL with water. A 20 mL aliquot was titrated with 5.02 mL of 0.5352 M HCl to reach PHP endpoint. Another 20 mL aliquot was titrated to the BCG endpoint, using up 18.87 mL of titrant in the process. Note: Answer in two decimal places only. If there is no answer, type in 0.00. Use the molar masses 105.989 ?/??l ??2cO3 and 84.007 g/mol NaHCO3 indicated. The volume of titrant needed to neutralize NaOH is _________ mL.The volume of titrant needed to neutralize Na2CO3 is _____________ mL.The volume of titrant needed to neutralize NaHCO3 is _____________ mL. The mass of NaOH is ___________ g.The mass of Na2CO3 is __________ g.The mass of NaHCO3 is __________ g. The percent weight of NaOH is __________ %.The percent weight of Na2CO3 is __________ %.The percent weight of NaHCO3 is __________ %.
- Six 50.0 ml volumetric flask 1 through 6 are labeled. 10.00 ml of 2.00 x 10-1 M Fe(NO3)3 solution was then pipet into each volumetric flask. A 1.00,2.00,3.00,4.00 and 5.00ml of 2.00 x 10-3M NaSCN solution was then pipetted to flask 2 through 6 respectively. A sufficient amount of 0.10 M nitric acid was then added to each flask to make each a total volume of 50.00ml. Hint M1V1=M2V2 a)what would be the concentration of Fe(NO3)3 in 0.10M HNO3? b)what would be the concentration of NaSCN in 0.10M HNO3?You want to determine the concentration of NaCl in a water. In preliminary analysis, it appears to be saline water with a NaCl content of approximately 4%. Should you dilute the sample if your titrant has a concentration of 0.1 M and you want to spend 25 mL of sample?A sample with a density of 0.502 kg/L was tested in the laboratory. Upon the arrival, a 3 uL of the sample was diluted until the volume was 250 uL. The laboratory assistant who used a different analysis method, computed the molarity of the sample solution was 0.159 M. Determine the concentration of the original sample in percent by volume in a solution (% v/v).
- Bay Water Titration The concentration of Cl- in ocean water is about 500-600 mM. The baywater is diluted by a factor of 12.5 using a 20.00 mL volumetric pipet and a 250 mL volumetric flask. Using a 15.00 mL volumetric pipet, 15.00 mL is transferred into three clean Erlenmeyer flasks. 10 mL of 1% dextrin solution, 20 mL of de-ionized water, and 3-4 drops of indicator are added and titrated each with the AgNO3 solution. From the procedure, find: Dilution factor Volume of diluted bay water Then calculate: The [Cl-] of diluted bay water The [Cl-] of bay water Consider this information: [AgNO3] = 0.04043177 trial # Veq 1 13.91 2 13.73 3 13.9 4 13.86 5 13.87 6 13.84 average 13.85167 [Cl-]Bay = ([AgNO3](Veq(ave))/Vdil bay water pipeted) (Vflask/Vbay water)An impure sample of 250 mg of adipic acid was recrystallized from 2.0 mL of boiling water. The solution was cooled to room temperature slowly and further cooled in an ice bath. What is the maximum amount of recoverable adipic acid at 0 oC? Solubility of adipic acid at 0 oC is 0.3 g/ 100 mL Group of answer choices 6 mg 249 mg 244 mg 250 mgA 5.00 mL wine vinegar was diluted to 25 mL and was titrated with 0.1198 M NaOH to determine its acidity. The endpoint was reached after addition of 31.45 mL of the NaOH solution. Calculate the % acidity of sample expressed as % acetic acid (w/w) if the density of the wine vinegar is 1.105 g/mL.
- A 0.1 g amine-containing compound is dissolved in water then diluted to 100 mL. You subject it to spectroscopic analysis, in order to get the concentration of amine in this compound. Next, you get 1 mL of the previously diluted sample then dilute it again to 250 mL for measurement. Then, you fill 3/4 of a 1-cm cuvette with this diluted sample, and you run an analysis using an AAS. The recorded absorbance is 0.545 at 410 nm. What is the molecular weight of the compound? (The molar absorptivity is 1.23 x 104 cm-1 mol-1 L.)Maganite is the leading brand for antacid to alleviate heartburn. Its active ingredient is a saturated solution of magnesium hydroxide (milk of magnesia) which neutralizes the sudden increase of H+ during heartburn. Its manufacturing company performed microtitration to simulate how the drug works upon intake. A 50.0 mL saturated solution was prepared. After filtering each solution, a 5.0 mL aliquot was transferred to a 25.0 mL Erlenmeyer flask and was titrated using pre-standardized 0.0320 M HCl which resembled the gastric acid. The endpoint was reached after the addition of 52.2 μL titrant. What is the concentration of hydroxide ions in the solution? Determine solubility s.Maganite is the leading brand for antacid to alleviate heartburn. Its active ingredient is a saturated solution of magnesium hydroxide (milk of magnesia) which neutralizes the sudden increase of H+ during heartburn. Its manufacturing company performed microtitration to simulate how the drug works upon intake.A 50.0 mL saturated solution was prepared. After filtering each solution, a 5.0 mL aliquot was transferred to a 25.0 mL Erlenmeyer flask and was titrated using pre-standardized 0.0320 M HCl which resembled the gastric acid. The endpoint was reached after the addition of 52.2 μL titrant.1. What is the concentration of hydroxide ions in the solution? Note: Use the scientific notation of 0.00012 = 1.2e-4 2. Determine s and Ksp of Mg(OH)2.Note: Use the scientific notation of 0.00012 = 1.2e-4