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:

Chemistry by OpenStax (2015-05-04)

1st Edition

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Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

Problem 79E: In a titration of cyanide ion, 28.72 mL of 0.0100 M AgNO3 is added before precipitation begins. [The...

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In a titration of cyanide ion, 28.72 mL of 0.0100 M AgNO3 is added before precipitation begins. [The reaction of Ag+ with CN- goes to completion, producing the Ag(CN)2- complex. Precipitation of solid AgCN takes place when excess Ag+ is added to the solution, above the amount needed to complete the formation of Ag(CN)2-. How many grams of NaCN were in the original sample?
The following solutions are mixed: 1.0 L of 0.00010 M NaOH and 1.0 L of 0.0014 M MgSO4. Is a precipitate expected? Explain.
A 0.7336-g sample of an alloy that contains copper and zinc is dissolved in 8 M HCl and diluted to 100 mL in a volumetric flask. In one analysis, the zinc (At. Mass = 65.38 g/mol) in a 25.00-mL portion of the solution is precipitated as ZnNH4PO4, and isolated as Zn2P2O7 (FM = 304.70g/mol), yielding 0.1163 g. The copper (At. Mass = 63.55 g/mol) in a separate 25.00-mL portion of the solution is treated to precipitate CuSCN (121.63 g/mol), yielding 0.2383 g. Calculate the %w/w Zn and the %w/w Cu in the sample.
4. A 0.1036-g sample containing only BaCl, and NaCl is dissolved in 50 mL of distilled water. Titrating with 0.07916 M AgNO3 requires 19.46 mL to reach the Fajans endpoint. Report the % (w/w) BaCl2 in the sample. [Ans. 29.86 % (w/w)]
A 4.912-g sample of a petroleum product was burnedin a tube furnace, and the SO2produced was collectedin 3% H2O2.Reaction:SO2(g)+H2O2→H2SO4A 25.00-mL portion of 0.00873 M NaOH was introducedinto the solution of H2SO4, following whichthe excess base was back-titrated with 15.17 mL of0.01102 M HCl. Calculate the sulfur concentrationin the sample in parts per million.
The % (w/w) I- in a 0.6712-g sample was determined by Volhard titration. After adding 50.00 mL of 0.05619 M AgNO3 and allowing the precipitate to form, the remaining silver was back-titrated with 0.05322 M KSCN, requiring 35.14 mL to reach the endpoint. Report the %(w/w) I- in the sample. [Ans. 17.76 % (w /w)]
The % (w/w) I- (MM = 126.9) in a 0.5812-g sample was determined by Volhard titration. After adding 50.00 mL of 0.06912 M AgNO3 and allowing the precipitate to form, the remaining silver was back-titrated with 0.07012 M KSCN, requiring 36.17 mL to reach the endpoint. Report the %(w/w) I- in the sample. 17.76 % 20.08 % 35.52 % 40.16%
An 800.0 mg sample containing sulfate was treated with a slight excess of Bac vielding a precipitate that contained 4.3 mg of co-precipitated BaCO3. After i and cooling, the precipitate (BaSO4+ BaCO3) weighed 377.0 mg. Calculate th following:
Q2: A 3.275 g sample of K2CrO4 yielded a precipitate of Cr,03 which weighed 1.075 g. Calculate Cr % and the purity of the salt.
The % w/w I– in a 0.6712-g sample was determined by Volhard titration. After adding 50.00 mL of 0.05619 M AgNO3 and allowing the precipitate to form, the remaining silver was back titrated with 0.05322 M KSCN, requiring 35.14 mL to reach end point. AgNO3 + I– → AgI (s) + NO3– Ag+ + SCN– → AgSCN How many millimoles of AgNO3 reacted with I–? How many milligrams of I– (MM=126.9 g/mol) were present in the sample? What is the % w/w I– in the sample?
A 0.5131-g sample containing KBr is dissolved in 50 mL distilled water. Titrating with 0.04614 M AgNO3 requires 25.13 mL to reach the Mohr endpoint. A blank titration requires 0.65 mL to reach the same endpoint. Report the % (w/w) KBr in the sample. [Ans. 26.19 % (w /w)]
The bismuth in 0.7405 g of an alloy was precipitated as BIOCI and separated from the solution by filtration. The washed precipitate was dissolved in nitric acid and treated with 10.00 mL of 0.1498 M AgNO3, causing the precipitation of AgCl. The excess AgNO; required 12.92 mL of 0.1008 M KSCN for titration. Calculate the % Bi in the sample. 6. (Answer : %Bi = 5.54%)

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