Question 21 To analyze the amount of dissolved oxygen in a water sample, the oxygen is reacted with iodine and a starch indicator is added. Thiosulfate is added until the indicator turns blue, and the amount of thiosulfate added can be used to calculate the amount of dissolved oxygen in the water. This is an example of titration analysis non-combustion gravimetric analysis combustion analysis dimensional analysis

Question 21 To analyze the amount of dissolved oxygen in a water sample, the oxygen is reacted with iodine and a starch indicator is added. Thiosulfate is added until the indicator turns blue, and the amount of thiosulfate added can be used to calculate the amount of dissolved oxygen in the water. This is an example of titration analysis non-combustion gravimetric analysis combustion analysis dimensional analysis

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter12: Gravimetric Methods Of Analysis

Section: Chapter Questions

Problem 12.25QAP

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A mixture of xenon and ?uorine was heated. A sample of the white solid that formed reacted with hydrogen to yield 81 ml of xenon (at STP) and hydrogen ?uoride, which was collected in waiter, giving a solution of hydro?uoric acid. The hydro?uoric acid solution was titrated, and 68.43 mL of 0.3172 M sodium hydroxide was required to reach the equivalence point. Determine the empirical formula for the white solid and write balanced Chemical equations for the reactions involving xenon.
Sodium bicarbonate (baking soda), NaHCO3, can be purified by dissolving it in hot water (60 C), filtering to remove insoluble impurities, cooling to 0 C to precipitate solid NaHCO3, and then filtering to remove the solid, leaving soluble impurities in solution. Any NaHCO3 that remains in solution is not recovered. The solubility of NaHCO3 in hot water of 60 C is 164 g/L. Its solubility in cold water of 0 C is 69 g/L. What is the percent yield of NaHCO3 when ills purified by this method?
Nitrous acid (HNO2) disproportionates in acidic solutionto nitrate ion (NO3- ) and nitrogen oxide (NO). Write abalanced equation for this reaction.
A newly-discovered iron ore was examined to determine percent iron in the ore gravimetrically. 5.408 grams of the ore samples was subjected to gravimetric analysis and precipitated as iron (III) oxide and dried at 105 degrees Celsius. What is the percent iron contentn of the ore if the mass of the precipitate is 0.3785 grams?
How many grams of silver carbonate will precipitate when 12.75 g of silver nitrate are added to excess potassium chromate?
Phosphate in a solution is titrated with 0.08141 M solution of silver nitrate (AgNO3) as follows:PO 43- + 3Ag+ ---> Ag3PO4How many g of PO43- (94.971 g/mol) are present in the sample if the titration required 30.55 mL of the Standardized Silver Nitrate titrant?Answer to 3 decimal places.
A sample containing NaCl, NaBr, & inert material weighs 1.000 g. Excess of AgNO3 gave a whiteprecipitate consisting of only AgCl and AgBr which weighs 0.5260 g. By heating the precipitate in a currentof Cl2 gas, the AgBr (187.78 g/mol) is converted to AgCl (143.32 g/mol) and the precipitate weighs 0.4260g. Find the % NaCl (58.44 g/mol) and % NaBr (102.909 mol) in the original sample.
A mixture of xenon and fluorine was heated. A sample of the white solid that formed reacted with hydrogen to yield 81 mL of xenon (at STP) and hydrogen fluoride, which was collected in water, giving a solution of hydrofluoric acid. The hydrofluoric acid solution was titrated, and 68.43 mL of 0.3172 M sodium hydroxide was required to reach the equivalence point. Determine the empirical formula for the white solid and write balanced chemical equations for the reactions involving xenon.
The following analytical procedures were used for the determination of chlorate (ClO3-). 10.00 mL of solutionA containing chlorate is analyzed. The chlorate is reduced with granulated zinc (to chloride).The excess zinc is dissolved in acid, after which the sample is filtered. The filtered sample is added70.00 mL 0.100 M AgNO3 solution dropwise. The precipitate is filtered off, washed and dried.It weighs 0.6003 grams. Calculate the chlorate concentration in solution A
Sodium oxalate, Na2C2O4Na2C2O4, in solution is oxidized to CO2(g)CO2(g) by MnO−4MnO4− which is reduced to Mn2+Mn2+. A 50.3 −mL−mL volume of a solution of MnO−4MnO4− is required to titrate a 0.342 −g−g sample of sodium oxalate. This solution of MnO−4MnO4− is then used to analyze uranium-containing samples. A 4.60 −g−g sample of a uranium-containing material requires 33.0 mLmL of the solution for titration. The oxidation of the uranium can be represented by the change UO2+→UO2+2UO2+→UO22+. Part A Calculate the percentage of uranium in the sample.
27) The cycle of copper reactions illustrates important principles of chemical reactions. The cycle begins with elemental copper, which in a first reaction is oxidized to copper(II) cation. Copper(II) is then carried through different solid forms. In the last step, copper(II) cation is reduced, the copper metal is regenerated, and the cycle is closed. The five key steps are (see attached picture). Assume that you want to carry out a sequence of cycle reactions. b) What volume of 16M HNO3 solution provides the required amount of the acid?
In the gravimetric analysis, precipitation method, solubility of %so3 What happends in the ignition process? What is the product after the precipitate is ignited?

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