help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working Which of the following operations does notinvolve leaching?Dissolving gold from oresDissolving pharmaceutical products from bark orrootsDissolving sugar from the cells of the beetRemoving nicotine from its water solution bykerosene

Here's why: -Leaching generally refers to the process of extracting a substance from a solid…

Which of the following operations does not involve leaching? Dissolving gold from ores Dissolving pharmaceutical products from bark or roots Dissolving sugar from the cells of the beet Removing nicotine from its water solution by kerosene

Which of the following operations does not involve leaching? Dissolving gold from ores Dissolving pharmaceutical products from bark or roots Dissolving sugar from the cells of the beet Removing nicotine from its water solution by kerosene

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 35P

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When jump-starting a car with a dead battery, the ground jumper should be attached to a remote part of the engine block. Why?
The iron content of hemoglobin is determined by destroying the hemoglobin molecule and producing small water-soluble ions and molecules. The iron in the aqueous solution is reduced to iron(II) ion and then titrated against potassium permanganate. In the titration, iron(ll) is oxidized to iron(III) and permanganate is reduced to manganese(II) ion. A 5.00-g sample of hemoglobin requires 32.3 mL of a 0.002100 M solution of potassium permanganate. The reaction with permanganate ion is MnO4(aq)+8H+(aq)+5Fe2+(aq)Mn2+(aq)+5Fe3+(aq)+4H2O What is the mass percent of iron in hemoglobin?
For a 50ml beaker, 0.4532g of pure iron III oxide was weighed, to which 1 ml of a concentrated hydrochloric acid solution was added and then 20 ml of deionized water was added to the beaker. After mixing, the resulting solution was transferred to a 50.00 ml flask and the volume was made up with deionized water. Then 15ml of this solution into a second beaker to which 10ml of an iron iii chloride solution of 0.200 M concentration was added. Calculate the final concentration of the iron iii cation solution expressed in mol/L and in g/L, considering that the volumes are additive.
Identify which element is oxidized and which is reduced in the reaction: 2C1O (aq) + H2 (g) + 2e – (ag) + 2OН- (aq) Cl is oxidized; H is reduced OH is oxidized; O is reduced OH is oxidized; Cl is reduced This is not a REDOX reaction
Hydrogen peroxide solutions can easily be decomposed by dust, trace amounts of metals or light. It istherefore necessary to periodically determine the purity of the peroxide solutions.This can be done via a redox titration as follows: The density of a particular surgical grade hydrogen peroxide solution is 1.11g.cm-3. Exactly 10 mL of this solution was pipetted and quantitatively transferred, along with a sufficientamount of a dilute sulphuric acid solution, into a 250.00 mL volumetric flask and made up to the mark. A 25.00 mL portion of this diluted solution is pipetted into a conical flask, and titrated with a0.372 M KMnO4 solution. The endpoint of the titration is determined when the colourless solution in the conical flask turns apersistent bright pink due to the presence of excess permanganate ions. The average titration value is 26.20 mL of the KMnO4 solution 1.Determine the percentage of the hydrogen peroxide in the solution sample.2. Naturally occurring manganese…
(a) Write the definition of reduction and oxidation. (b) Ammonia oxidizing bacteria (AOB) play an important role in nitrogen cycle. They are also utilized in engineered systems to remove ammonia in wastewater treatment. They obtain energy by oxidizing ammonia NH3 into nitrite (NO2-) and reducing oxygen to water. Balance the reduction and oxidation reactions driven by AOB. (c) Combine the redox reactions into a single reaction. (d) Find ΔG° for the combined reaction. (e) Find ΔG for the given conditions: [NH3] = 2.7 × 10-3 M; pO2 = 0.21 atm; [NO2-] = 1.2 × 10-5 M. If necessary assumeneutral pH (i.e., pH = 7). Are the given conditions favourable for AOB growth?
For the gravimetric determination of manganese, 1.8762 g of sample containing Mn was dissolved in acid solution and made up to 100 mL in a calibrated volumetric flask. A 25.00 mL aliquot of this solution was transferred to a beaker. The solution was heated to boiling and chemical substances required were added till precipitating MnNH4PO4. After filtering, rinsing, and igniting, 0.5365 g of Mn2P2O7 was obtained. Calculate the % manganese in the sample (Mn: 55, P: 31, O: 16 g/mol).
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10
The chief chemist of the Brite-Metal Electroplating Co. isrequired to certify that the rinse solutions that are discharged from the company’s tin-plating process into the municipal sewer system contain no more than 10 ppm (parts per million) by mass of Sn2+. The chemist devises the following analytical procedure to determine the concentration. At regular intervals, a 100-mL (100-g) sample is withdrawn from the waste stream and acidified to pH = 1.0. A starch solution and 10 mL of 0.10 M potassium iodide are added, and a 25.0-mA current is passed through the solution between platinum electrodes. Iodine appears as a product of electrolysis at the anode when the oxidation of Sn2+ to Sn4+ is practically complete and signals its presence with the deep blue color of a complex formed with starch. What is the maximum duration of electrolysis to the appearance of the blue color that ensures that the concentration of Sn2+does not exceed 10 ppm?
A 5.00 mL sample of brandy was diluted to 1.00 L in a volumetricflask. The ethanol in 25.00 mL aliquot of the diluted solution wasdistilled into 50.0 mL of 0.02000 M K2Cr2O7and oxidized to aceticacid with heating.3C2H5OH + 2Cr2O72- + 16 H+ → 4 Cr3+ + 3CH3COOH + 11 H2OAfter cooling, 20.00 mL of 0.1253 M Fe3+ was pipetted into the flask. The excess Fe2+ was then titrated with 7.46 mL of standard K2Cr2O7to a diphenylamine sulfonic acid endpoint. Calculate the percent (w/v) ethanol (MW 46.07 g/mol) in the brandy.
Q1) a) What is i) a standard solution? i)a reduction-oxidation (redox) reaction? b) A standard solution of hydrated Iron (II) sulphate, FeSO4.XH2O, as prepared by dissolving 5.8g of the salt in a volumetric flask making it to 250ml (250 cm³), 25ml (25 cm³) of this solution was acidified and found to react with 22.8ml (22.8 cm³) of 0.018MPotassium permanganate solution. The half equation for the reaction are: Mn" a) + 4H20) MnO4(aq) + 8H*(ag) Fe" aq) Fe2"(aq) + e i) What is the indicator for the titration of Iron(1)sulphate and Potassium permanganate solution? ii)indicate the colour at the end point if the permanganate is in the burette. iii)Why is it necessary to acidify the Iron(II)sulphate before titration ?