e) via:.Lisbeth MylaCHEM 3321A Back titration - HomeworkA solution containing Cl- was analyzed as follows in a back titration. A solution containing (excess) Ag + isadded, and the AgCl precipitate is filtered and removed.The excess Ag is then titrated with SCN-Ag+ (aq) + Cl(aq) -Ag+ (aq) + SCN (aq)-------> AgCl (s)--------> AgSCN (aq)In one analysis, 25.00 mL of 0.01840 M AgNO3 (aq) was added to 50.00 mL of a solution containingdissolved chloride. The resulting AgCl (s) was filtered and removed. The excess Ag+ (aq) remainingrequired 14.25 mL of 0.02008 M SCN (aq) to reach the endpoint.What is the original concentration of Cl (aq) in the original 50.00 mL soln?

Question: The excess Ag⁺ remaining required 14.25 mL of 0.02008 M HCl to reach the…

Answered: e) via:. Lisbeth Myla CHEM 3321 A Back…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.35QAP

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A student wanted to determine the amount of NaOCI in a commercial bleaching solution. He diluted 2 g of bleach in a 100 ml volumetric flask. A 50 ml sample of the diluted bleach was mixed with excess acidified potassium iodide KI and a few drops of an indicator. The resulting solution was titrated with Na-S.O, solution. The titration required 17 mL of 0.05M Na,S,O, solution. The series of reactions that take place during this experiment: 21+OCI+ 2H1₂ + Cl + H₂O 1₂+28,0,³ →21+S,0,² a) Calculate the number of moles of OCI- in 50 mL diluted bleach and in 100 mL.
26.
An acid-base indicator, HIn, dissociates according to the following reaction in an aqueous solution. K. Hin HIn(aq) = In (ag)+ H* (aq) The protonated form of the indicator, HIn, has a molar absorptivity of 2777 M-1.cm-1 and the deprotonated form, In¬, has a molar absorptivity of 19024 M-1·cm-1 at 440 nm. The pH of a solution containing a mixture of HIn and In- is adjusted to 5.86. The total concentration of HIn and In- is 0.000184 M. The absorbance of this solution was measured at 440 nm in a 1.00 cm cuvette and was determined to be 0.884. Calculate pka for HIn.
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5 SO2 + 2 MnO4- + H2O ---> 5 SO42- + 2 Mn2+ + 4 H+ The MnO4- solution is poured in a burette and then titrated till the equivalent point is aquired. How many L are needed of MnO4? (the burette starts at 5,7 and is 37,3 after titration)
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ng resourc.. (27) Could've Been - [References] Calculate the pH at the halfway point and at the equivalence point for each of the following titrations. a. 100.0 mL of 0.30 M HC7H502 (Ka = 6.4 x 10-5) titrated by 0.10 M NaOH pH at the halfway point = pH at the equivalence point = b. 100.0 mL of 0.40 M C2H;NH2 (K½ = 5.6 × 10¬4) titrated by 0.10 M HNO3 pH at the halfway point = pH at the equivalence point = c. 100.0 mL of 0.70 M HC1 titrated by 0.15 M NaOH pH at the halfway point = pH at the equivalence point =
The phosphate in a 3.000 g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO3. The solution was filtered and the filtrate required 18.23 mL of 0.1377 M KSCN for titration to the FeSCN2+ end point. Calculate the percentage of phosphate in the detergent.
A PO4* in 100 ml water sample is precipitated as A93PO4 by adding 100 ml 0.2 M AGNO3. Then excess AgNO3 is back-titrated with 50 ml 0.2 M KSCN. What is the molar analytical concentration of PO4 in sample? Chemical reactions are as follows: PO+3Ag*A93PO4(s) Ag* + SCN AGSCN(s) Lütfen birini seçin: a. 0.033 М b. 0.02 M c. 0.017 M d. 0.066 M
A 270.00 mL solution of 0.00150 M AB4 is added to a 380.00 mL solution of 0.00250 M C3D4. What is pQsp for A3D4?
2- Ahmed has done four types of titrations of 1M and 50 ml for both acid and base (Conductometric Titration of Strong Acid with Strong Base , Potentiometric Titration of Weak Acid with Strong Base , Potentiometric Titration of Strong Acid with Strong Base and Conductometric Titration of Weak Acid with Strong Base ). He plotted the results in curves as shown below. Match between the type of titration and his results 3- Ahmed standardized NaOH (10 ml) with KHP( mass=1 g , MW= 204 g/mol ). Calculate the concentration of standardized NaOH? 4- Calculate pka for a weak acid titrated with strong base using the curve shown below? 14 12- 10- 8 6- 4- 2- 0- 10 20 30 40 50 5- If the solute moved 3 cm in paper chromatography and R, was 0.5. How long in cm the solvent has moved?
A solution of HClO4 was standardized by dissolving 0.4008 g of primary-standardgrade HgO in a solution of KBr: HgO(s) + 4Br- + H2O --> HgBr42- + 2OH-. The liberated OH- consumed 43.75 mL of the acid. Calculate the molar concentration of the HClO4.

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