A1.223 g sample containing arsenic (As) was converted to H3AS0, by suitable treatment. 40.00 ml. of 0.07891 M AGNO3 was thenadded to the acid to precipitate arsenic quantitatively as AgAs01. The excess AgNO3was back-titrated with 11.27 ml. of 0.1000 MKSCN ; the Reacti on was Cal culate the percent of As,03 in the sample.1. O5.472. O2.233. O11.154. O66.925. O33.45

The question is based on the concept of quantitative analysis. We have to calculate percentage…

A 1.223 g sample containing arsenic (As) was converted to H3As0, by suitable treatment. 40.00 ml. of 0.07891 M AGNO3 was then added to the acid to precipitate arsenic quantitatively as AggAso1. The excess AgNO3was back titrated with 11.27 mL of 0.1000 M KSCN ; the Reacti on was Calcul ate the percent of As,03 in the sample. 1. O5.47 2. O2.23 3. O11.15 4. O 66.92 5. O33.45

A 1.223 g sample containing arsenic (As) was converted to H3As0, by suitable treatment. 40.00 ml. of 0.07891 M AGNO3 was then added to the acid to precipitate arsenic quantitatively as AggAso1. The excess AgNO3was back titrated with 11.27 mL of 0.1000 M KSCN ; the Reacti on was Calcul ate the percent of As,03 in the sample. 1. O5.47 2. O2.23 3. O11.15 4. O 66.92 5. O33.45

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter13: Titrations In Analytical Chemistry

Section: Chapter Questions

Problem 13.22QAP

See similar textbooks

Similar questions

A chemist dissolves a 1.497-g sample of a type of metal (an alloy of Sn, Pb, Sb, and Cu) in nitric acid, and metastannic acid, H2SnO3, is precipitated. She heats the precipitate to drive off the water, which leaves 0.4909 g of tin(IV) oxide. What was the percentage of [in in the original sample?
Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
1. 0.646 g of sample containing BaCl2.2H2O (244.26 g/mol) was dissolved and enoughpotassium chromate was added. After filtering, the precipitate was dissolved in acid andenough KI was added and titrated with thiosulfate. Since 48.7 mL of 0.137 M thiosulfateis used for this, what is the percentage of BaCl2.2H2O in the sample?K2Cr2O7 + 7H2SO4 + 6KI  4K2SO4 + Cr2(SO4)3 + 7H2O + 3I2
6. The phosphorus content in a 0.3004-g sample was precipitated as (NH4);PO4 .12M0O3 a slightly soluble precipitate. The precipitate was filtered, washed, and further redissolved in acid. The resulting solution was treated with an excess of Pb²* resulting in the formation of 0.3017 g of PbMoO4. Calculate the % w/w of P2Os.||
(Last Day Promotio... Kronos Worktorce... Maame Acheampo... MIDTERM M [Review Topics] [References] Use the References to access important values if needed for this question. How many grams of Ag,CO3 will precipitate when excess Na,CO3 solution is added to 77.0 mL of 0.690 M AGNO, solution? 2AGNO3(aq) + Na,CO3(aq) Ag,CO3(s) + 2NAN03(aq) + 2NaNO3(aq) Submit Answer Retry Entire Group 9 more group attempts remaining
The ascorbic acid, C,H;Os (176.124 g/mmol) content of a bottle of peach juice containing 2.50 L was determined by titration with a standard solution of potassium iodate, KIO3. The KIO; solution was prepared by dissolving 100.4 mg primary standard grade KIO; (214.001 mg/mmol) to a final volume of 250.0 mL. To a 200.00-mL aliquot of the sample, 10 mL of KI, 10 mL of HCl and 5 mL of starch solution were added and subsequently titrated, requiring 18.19 mL of the KIO; titrant. The relevant reactions are given below: KIO; + 5KI + 6H* → 3l2 + 6K* + 3H;0 CH;O, + l2→ CH,O, + 21- + 2H* a. How many millimoles of ascorbic acid is in the titrated sample? b. What is the mass of ascorbic acid per bottle of the peach juice?
0.900 g KIO3 was dissolved to give a 50.00 mL Iodate solution. 35.00 mL aliquot reactedwith the iodide to form triiodide. The liberated triiodide was titrated and consumed 8.65 mL of theS2O32- solution to reach endpoint. Calculate the concentration in molarity of the Na2S2O3solution.
Calculate the hinal Concentaton of k' lag), CoO¢ (aq), Ba"cq prepared by addig o.100L of to 0.150L of 0.250 M Ba Bra 2t nd br aq) in a soluteon 0.200 M KCO, ( for ba Ca Qu , K, = , Ksp 2.3x108)
A sample containing phosphorus weighs 4.2580g. The phosphorus in the sample is converted into phosphate ion and precipitated as silver phosphate through the addition of 50mL of 0.0820M of silver nitrate. The excess silver nitrate was back titrated with 4.06mL of 0.0625M of potassium thiocyanate. Calculate the % phosphorus pentoxide in the sample.
Read and urete on the selection of a proper Indicator • What is an Indicator Chemistry Of work ? )u Factors which result in Indicator f an acıd/base Indicator (how does it Colour Chawge of an Indicator Cuhat is ?) range ranges of different lndicators Indicator which Indicafors reaction may be used for which Indicator • General rule for Cho.ce of an . Itow to determine range at which an Indicator whe of wHl Change colour