Compare the two quantities based on the given condition: Gravimetric determination of chloride as AgCl I. Mass of precipitate if peptization occurred II. Mass of precipitate if occlusion occurred (a) I > II (b) I = II (c) I < II (d) The two quantities cannot be compared due to insufficient information.

Compare the two quantities based on the given condition: Gravimetric determination of chloride as AgCl I. Mass of precipitate if peptization occurred II. Mass of precipitate if occlusion occurred (a) I > II (b) I = II (c) I < II (d) The two quantities cannot be compared due to insufficient information.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter20: Applications Of Oxidation/reduction Titrations

Section: Chapter Questions

Problem 20.26QAP

See similar textbooks

Similar questions

The following salts were added to a beaker of distilled water: NaCl (NH2)2CO; Ca(NO;)2 Which of the following products will precipitate out of solution? O NH CI O CaCO, FONTHN O O NaCO;
The chloride in the sample is to be determined gravimetrically by precipitating and weighing AgCl. What weight in grams of sample should be taken so that the percentage of Cl is obtained by simply multiplying the weight of the AgCl precipitate by 10?
6. The mercury in a 0.839 g sample was precipitated with an excess paraperiodic acid, H¿IO, 5Hg + 2H,IO, → Hg;(IO,); + 10H The precipitate was filtered, washed free of precipitating agent, dried and weighed, 0.3408 g being recovered. Calculate the percentage of Hg,Cl, in the sample.
1. A 0.3516 g sample of commercial phosphate detergent was ignited at a heat to destroy the organic matter. The residue was taken up in hot HCI which converted P to H3PO4. The phosphate was precipitated as MGNH4PO4.6H2O by addition of Mg+ followed by aqueous NH3. After being filtered and washed, the precipitate was converted to Mg2P2O7 by ignition at 1000 OC. This residue weighed 0.2161 g. Calculate the percent P (30.974) in the sample? Ans 17.11%
11. (ii) A student was given 400 cm of aqueous ammonia solution, NH,(ag), The student was asked to determine how many moles of NH, had been dissolved to prepare the solution. The student titrated 25.0cm of NH.(ag) and found that it reacted exactiy with 32.5cm3 of 0.100 mol dm sulturic acid. The equation for this reaction is shown below. 2NH,(aq) + H,SO,(aq) → (NH)SO,(aq) Calculate the amount, in moles, of NH, in the original 400 cm3 solution. mol answer =
The aluminum in a 1.200-g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al2O3.xH2O. The precipitate was filtered and ignited at to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysis in terms of %NH4Al(So4)2 %Al2O3 %Al
A stock standard concentration of 101.25ppm was prepared of Cu. What are the actual concentrations of the working standards prepared in 100mL volumetric flasks, using 1mL, 5mL, 8mL, and 10mL volumes of the stock standard?
A solution was prepared by dissolving 367 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give 750.0 mL. Calculate (a) the molar analytical concentration and Normality of K3Fe(CN)6. (b) the molar concentration of K+. (c) the molar concentration of Fe(CN)63-. (d) the weight/volume percentage of K3Fe(CN)6.
I would like to prepare standards by conducting a serial dilution of 2mg/ml BSA down to 0.0625mg/ml BSA. How many standard solutions will I have? What are the concentrations of these standard solutions?
As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content using gravimetric analysis with sodium tetraphenylborate, Na*B(C,H,). Unfortunately, the amount of potassium, which also precipitates with sodium tetraphenylborate, is non-negligible and must be accounted for in the analysis. Assume that all potassium in the soil is present as K,CO, and all ammonium is present as NH,Cl. A 5.045 g soil sample was dissolved to give 0.500 L of solution. A 125.0 mL aliquot was acidified and excess sodium tetraphenylborate was added to precipitate both K* and NH ions completely. B(C,H,), + K* KB(C,H,),(s) Compound Formula mass 358.33 g/mol KB(C,H,), NH,B(C,H,), K, CO, B(C,H ), + NH NH,B(C,H,), (s) 337.27 g/mol 138.21 g/mol The resulting precipitate amounted to 0.247 g. A new 250.0 mL aliquot of the original solution was made alkaline and heated to remove all of the NH as NH,. NH,CI 53.492 g/mol The resulting solution was then acidified, and excess sodium…
9. An aqueous solution of sulfuric acid is prepared by mixing a secondary standard of sulfuric acid with deionized water. The aforementioned acid is to be used as a titrant hence its concentration must be accurately determined. To do this, Engr. Polinar, standardized the titrant by titrating two liters of ammonia at 0.90 atm and 30 deg C. From the experiment, 134 mL of the titrant was necessary to neutralize the ammonia. Determine the concentration of the acid in terms of normality? 10. Engr. Forcadela is optimizing a plastic formulation by manipulating the phosgene concentration injected as a gas during the reaction. To obtain credible results, he considered the propensity of phosgene to dissociate into carbon monoxide and chlorine gas at 395 deg C. Performing an experiment at the aforementioned temperature, an equilibrium is reached amongst the species where the total pressure is at 3 atm. If the equilibrium constant expression in terms of concentration for the reaction at 395 deg C…
What is the percentage purity a sample of (A/²S04)3 if a 0.5000 g sample produced a precipitate of BaSO4 weighing 0.1000 g