Preparation and Standardization of KMnO4 solutionExperimental dataComplete the table below.Trial 10.2001 gTrial 20.2065 gTrial 3Weight of sodium oxalate(Na2C2O4, MM= 134 g/mol)Titration data0.2050 gFinal readingInitial reading29.86 mL0.00 mL30.66 mL30.52 mL0.00 mL0.00 mLTotal vol. of KMNO4 usedComputed Molarity of KMNO4solutionMean MolarityComputed Normality of KMNO4Mean Normality of KMNO4solutionReaction Involved:Calculations:

Answered: Image /qna-images/answer/6e19ae5f-00d3-499e-9562-3f4a1d0d6231.jpg

Preparation and Standardization of KMNO4 solution Experimental data Complete the table below. Trial 1 0.2001 g Trial 2 0.2065 g Trial 3 0.2050 g Weight of sodium oxalate (NazC204, MM= 134 g/mol) Titration data Final reading Initial reading Total vol. of KMNO4 used 29.86 mL 0.00 mL 30.66 mL 0.00 mL 30.52 mL 0.00 mL Computed Molarity of KMNO4 solution Mean Molarity Computed Normality of KMNO4 Mean Normality of KMNO4 solution Reaction Involved: Calculations:

Preparation and Standardization of KMNO4 solution Experimental data Complete the table below. Trial 1 0.2001 g Trial 2 0.2065 g Trial 3 0.2050 g Weight of sodium oxalate (NazC204, MM= 134 g/mol) Titration data Final reading Initial reading Total vol. of KMNO4 used 29.86 mL 0.00 mL 30.66 mL 0.00 mL 30.52 mL 0.00 mL Computed Molarity of KMNO4 solution Mean Molarity Computed Normality of KMNO4 Mean Normality of KMNO4 solution Reaction Involved: Calculations:

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.40QAP

See similar textbooks

Similar questions

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?..
When standardizing two liters of a potassium permanganate solution with a primary standard solution of sodium oxalate, approximately 0.0100 M, it was planned to use between 30.00 mL and 45.00 mL of the titrated reagent. In which mass range (in grams) the primary standard should be weighed? Data: MM KMnO4 = 158.00 g/mol; MM Na2C2O4 = 134.00 g/mol 2CO2 + 2e- ↔ C2O4 2- Eo = -0,432 V MnO4 - + 8 H+ + 5e- ↔ Mn2+ + 4 H2O Eo = 1,52 V
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 buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of solubility and Ksp of calcium hydroxide: Trial 1: Final Buret reading (ml)-19.80; Initial Buret reading (ml)- 13.00; Temperature (Celcius)- 25 Trial 2: Final Buret reading (ml)-26.10; Initial Buret reading (ml)- 19.80; Temperature (Celcius)- 25 Voume of HCl used: Trial 1- 6.80ml; Trial 2- 6.30mL 1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction.3. Calculate the molar solubility (in mol/L) of OH- and Ca2+.4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5.…
The buret was filled with 0.100 M HCl solution. Then was transferred in a 25.0 mL of saturated calcium hydroxide solution (2g of calcium hydroxide per 100 ml of water) in two separate E-flasks. Then 2 drops of phenolphthalein was added to each flask Titration data for the determination of solubility and Ksp of calcium hydroxide: Trial 2: Final Buret reading (ml)-26.10; Initial Buret reading (ml)- 19.80; Temperature (Celcius)- 25 Voume of HCl used: Trial 2- 6.30mL 1. Compute for the moles of H+ used and the moles of OH- present. moles of H+ used = (concentration of HCl) × (volume of HCl used)moles of OH- = moles of H+ used 2. Construct an ICE table for the reaction.3. Calculate the molar solubility (in mol/L) of OH- and Ca2+.4. Determine the solubility of Ca(OH)2 in g/L. (MM of Ca(OH)2 = 74.096 g/mol). 5. Calculate the Ksp of Ca(OH)26. Compute for the percent error of the experimental value for Ksp of Ca(OH)2 with the literature…
A sample is analyzed for chloride by the Volhard method. From the following data, calculate the percentage of chloride present:Weight of sample = 6.0000 g dissolved and diluted to 200 mLAliquot used = 25.00 mL AgNO3 added = 40.00ml of 0.1234MKSCN for back titration = 13.20ml of 0.0930M
A 320.00 mL solution of 0.00290 M AB2 is added to a 260.00 mL solution of 0.00235 M C3D2. What is pQsp for A3D2?
Back titration. Impure K2S2O8 (FM 270.32, 0.507 3 g) was analyzed by treatment with excess standard Na2C2O4 in H2SO4. After reaction with 50.00 mL of 0.050 06 M Na2C2O4, the excess oxalate required 16.52 mL of 0.020 13 M KMnO4. Find the weight percent of K2S2O8 in the impure reagent.
The SO2 present in air is mainly responsible for the phenomenon of acid rain. The concentration of SO2 can be determined by titrating against a standard permanganate solution as follows: 5SO2 + 2MnO4- + 2H2O ---> 5SO42- + 2Ms2 + 4H+ Calculate the number of grams of SO2 in a sample of air if 4.90mL of 0.00700M KMnO4 solution are required for the titration. Be sure your answer has the correct number of significant digits.
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 sample
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.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…
1.065g of MgO (Analyte) of 84.74% were treated w/ 50ml of 1.02N H2SO4 (Acidic Titrant), and 48.28 mL of NaOH (Base Titrant) 1.103N concentration MW of analyte: 40Meq of analyte: 0.02NaOH vol: 48.28 Compute for the meq weight consumed by the acidic titrant (g-meq)