9. The % w/w of I- in a 0.2144-g sample was determined by Volhard titration. After adding 50.00 mL of 0.04980 M AGNO3 and allowing the precipitate to form, the remaining silver was back titrated with 0.05322 M KSCN, requiring 22.76 mL to reach the end point. (MM of I = 126.904 g/mol) Reactions: Ag*+I"→ Agl Ag* + SCN¯ → Ag(SCN) Calculate the:

9. The % w/w of I- in a 0.2144-g sample was determined by Volhard titration. After adding 50.00 mL of 0.04980 M AGNO3 and allowing the precipitate to form, the remaining silver was back titrated with 0.05322 M KSCN, requiring 22.76 mL to reach the end point. (MM of I = 126.904 g/mol) Reactions: Ag+I"→ Agl Ag + SCN¯ → Ag(SCN) Calculate the:

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.23QAP

See similar textbooks

Similar questions

A solid sample containing some Fe2+ion had a total mass of .9791 g. It required 18.2 ml of 0.02304 M KMnO4 to titrate the Fe2+ in the dissolved sample to a pink endpoint. How many moles of Fe2+ were in the the sample? How many grams of irion were present in the sample and what was the mass percent iron in the sample?
A sample of freshly precipitated and filtered silver chloride weighs 459.0 mg. If 1.00 % of the silver chloride becomes photo decomposed, what is the precipitate’s weigh?
The level of dissolved oxygen in a water sample can be determined by the Winkler method. In a typical analysis, a 100.0-mL sample is made basic, and treated with a solution of MnSO4, resulting in the formation of MnO2. An excess of KI is added, and the solution is acidified, resulting in the formation of Mn2+ and I2. The liberated I2 is titrated with a solution of 0.00870 M Na2S2O3, requiring 8.90 mL to reach the starch indicator end point. Calculate the concentration of dissolved oxygen as parts per million of O2.
The mass of K3PO4 needed to prepare 250.0mL of an aqueous solution in which PO4-3 concentration is 0.0550M. The answer is ……………………… How many grams of silver sample is equal to 0.0417 mole of silver The answer is ……………………… When 38.0 mL of 0.1250 M H2SO4 is added to 100 mL of a solution of PbI2, a precipitate of PbSO4 forms. The PbSO4 is then filtered from the solution, dried, and weighed. If the recovered PbSO4 is found to have a mass of 0.0471g, what was the concentration of iodide ions in the original solution The answer is ……………………………… Express 96.342 m using 2 significant figures The answer is ………………………………. The oxidation number of sulfur in (Na2S2O5) is? The answer is ………………………………
If 20.0 mL of 0.250 M sodium chloride is added to 25.0 mL of 0.200 M silver (I) perchlorate, what mass (g) of precipitate will be formed?
(a) If the molar solubility of Cu3(PO4)2 at 25 oC is 1.67e-08 mol/L, what is the Ksp at this temperature?Ksp = _______(b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3?solubility = ______ mol/L
The arsenic in a 1.22-g sample of a pesticide was converted toAsO43- by suitable chemical treatment. It was then titratedusing Ag+ to form Ag3AsO4 as a precipitate. (a) What is theoxidation state of As in AsO43-? (b) Name Ag3AsO4 by analogyto the corresponding compound containing phosphorusin place of arsenic. (c) If it took 25.0 mL of 0.102 M Ag+to reach the equivalence point in this titration, what is themass percentage of arsenic in the pesticide?
A mixture containing PbCO3 is treated with HNO3 to completely dissolve the PbCO3. The resulting solution required 29.22 mL of 0.122 M Na2SO4 to completely precipitate all the lead. Q1: Mass of Pb in original mixture Q2: If HCl had been used to dissolve the powder, would the same amount of PbSO4 also form??
A 20 mL volume of 0.015 M KIO3 containing an excess of KI, is added to a 0.312 g sample of a Real Lemon solution containing vitamin C. The Yellow-brown solution, caused by excess I2 is titrated to a colorless starch endpoint with 11.3 mL pf 0.106M Na2S2O3. Question: Calculate the percent by mass of Vitamin C in the Real Lemon Sample
It is required to know the concentration of an aqueous solution of H2SO4 that appeared in the laboratoryChemistry III and it's unlabeled. To this end, a student of analytical chemistry carried out the followingProcedure: He took 5.00 mL of a fresh and standardized solution of 0.525M NaOH and brought them to a250.0 mL balloon to be completed with distilled water. Subsequently, he poured 15.00 mL of the solutionH2SO4 of unknown concentration in an Erlenmeyer flask and added 2 drops of phenolphthalein.Using a burette filled with the last NaOH solution, he noticed that when adding 39.40 mL of the hydroxidethe Erlenmeyer solution reached a faint but permanent pink. With the above dataDetermine the concentration and pH of the H2SO4 solution.
the thiourea in a 1.455-g sample of organic material was extracted into a dilute H2SO4 solution and titrated with 37.31 mL of 0.009372 M Hg21 via the reaction. Find the percentage of (NH2) 2CS (76.12 g/mol)in the sample?
From the solution in Products 2, it was filtered and heated further until it was dried. This produced a precipitate with 0.3592 g.what is the molecular weight of the unknown metal cation?what is the identity of the metal in the unknown solution?