To prevent inclusion from occurring during precipitation, the technique to follow isI. filter precipitate with less porous paperII. crystal growth be made to occur more slowlyII. use of dilute analyte with concentrated precipitantIV. addition of soluble electrolyteO I & IIIO I l onlyO Iv onlyO II & IVO I only

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Answered: To prevent inclusion from occurring…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter28: Atomic Spectroscopy

Section: Chapter Questions

Problem 28.13QAP

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A sample of iron ore weighing 800 mg was treated with HNO3 , boiled to dryness and redissolved in dilute HCl. After filtration and removal of undissolved silica, the liquid was passed through a Walden reductor. The collected sample was titrated with 0.0210 M KMnO4 , requiring 12.0 mL to reach the end point. Calc %Fe (55.845) in the ore.
What are the steps to yield Only typed solution
Sources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided. TOPIC: Measured mass of the precipitate 1. Overignition which causes the conversion of BaSO4 precipitate to BaO. EX _____ ET2. Precipitate was not washed thoroughly. Ex _____ ET TOPIC: Standardization of Titrant 3.Distilled water was not equilibrated to room temperature before the preparation of NaOH titrant. EX _______ ET
It is required to prepare 300.0 ml of 0.3375 Ma calcium acetate solution for which two bottles with 0.4250 Ma and 0.1250 Ma solutions of this reagent are available. Describe clearly how to prepare the required solution. (Answer /mix 212.5 mL of solution 0.4250 Ma with 87.5 ml of 0.1250 Ma solution in this reagent)
In gravimetric analysis, co-precipitation occurs alongside with analyte precipitation,resulting in the introduction of impurity and excess mass. Occlusion and inclusion areamong the sources of impurities. Distinguish the difference between occlusion andinclusion and compare them using diagrams
A mixture consisting of 15 mole % Phenol in water is to batch distilled at 260 torr, what fraction of the original batch is remains in the still when the total distillate contain 98mole % w water? What is the residues concentration?
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)
Using the term u of KSP experimental procedure the 6 p.m. As you add 5 ml of .004M AgNo to 5ml of .0025M K2CrO4. Is either of these reagents in excess? If so which one?
. 100 ml boiled cooled and filtered water sample takes 9.6 ml of M/50 EDTA in titration. The Permanent hardness of the water sample in terms of ppm of CaCO3 equivalent is
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…
00 mL of a diprotic acid primary standard solution was accurately prepared to a concentration of 0.1431 M. Three samples of this primary standard solution were used as samples in a titration to standardize an aqueous solution of sodium hydroxide, NaOH, which would be used as a titrant. Using the following table of data for the titration of the primary standard acid with NaOH, calculate the average concentration of NaOH. Trial # Volume of primary standard Initial titrant volume Final titrant volume 1 10.00 mL 8.21 mL 27.22 mL 2 10.00 mL 27.22 mL 46.23 mL 3 10.00 mL 30.28 mL 49.29 mL 0.1506 M 0.0753 M 0.0376 M 0.1431 M 0.0526 M

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