dentify the type of titration method. Choose the best answer. - ✓ can be carried out at low pH or extremely acidic conditions ✓ makes use of adsorption indicators ✓the indicator reaction produces a reddish-brown precipitate - ✓ forms complex with EDTA ✓requires a second titrant for back-titration ✓indicator can either be potassium chromate or sodium chromate - The indicator dye turns the sample into a greenish-yellow solution and turns pink when dye is adsorbed on ppt A. Fajan B. Mohr C. Volhard D. None of the above

dentify the type of titration method. Choose the best answer. - ✓ can be carried out at low pH or extremely acidic conditions ✓ makes use of adsorption indicators ✓the indicator reaction produces a reddish-brown precipitate - ✓ forms complex with EDTA ✓requires a second titrant for back-titration ✓indicator can either be potassium chromate or sodium chromate - The indicator dye turns the sample into a greenish-yellow solution and turns pink when dye is adsorbed on ppt A. Fajan B. Mohr C. Volhard D. None of the above

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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Complex Ion Formation and Precipitation Reactions i. A 1-L water sample was submitted for determination of chloride ion. 100.00mL the sample was analyzed using the Volhard method. 50.00 mL of 0.0929N AgNO3 was added to the sample and was back titrated with 12.50mL of 0.0510N KSCN solution to reach the end point. Find ppm Cl- in the water sample. ii. Using Mohr method, the chloride content of a mineral water was determined. 50.00mL of the sample was titrated with 10.80mL of 0.05N AgNO3 solution to reach end point. Determine the concentration of Cl- in ppm. iii. Calculate the hardness of a water sample such that 100.00mL of the sample required 35.00mL of 0.1051M EDTA solution to reach the end point.
Identify the type of titration method. Choose the best answer. can be carried out at low pH or extremely acidic conditions ✓ makes use of adsorption indicators ✓the indicator reaction produces a reddish- brown precipitate forms complex with EDTA requires a second titrant for back-titration indicator can either be potassium chromate or sodium chromate The indicator dye turns the sample into a greenish-yellow solution and turns pink when dye is adsorbed on ppt A. Fajan B. Volhard C. None of the above D. Mohr
13. A sample contained Cr(III) species. A 25.00 mL portion of this sample is combined with 10.00 mL of a 0.0875 M solution that contains a complexing agent, CDTA. This mixture is heated to boiling for several minutes to allow the CDTA to complex with Cr(III) species. The mixture is then cooled, and the excess CDTA is measured by a back titration using 0.0258 M Bi³+, required 4.20 mL to reach end point. Determine the original concentration of Cr(III) species in the sample [Molar ratio of CDTA:Cr(III): Bi³+ = 1:1:1]
Volhard titration. A 30.00-mL solution of unknown I2 was treated with 50.00 mL of 0.365 0 M AgNO3. The precipitated AgI was filtered off, and the filtrate (plus Fe31) was titrated with 0.287 0 M KSCN. When 37.60 mL had been added, the solution turned red. How many milligrams of I2 were present in the original solution?
Which rapid and quantitative analysis requires a sample solution of metal ion to be titrated against a standard solution of EDTA, in the presence of a buffer?* Alkalimetric Replacement Back Titration Direct Which agent is added into a solution if direct titration is deemed to proceed slowly?* Indicator Titrant Catalyst Demasking agent Which method uses an excess solution of EDTA added to a sample and then pH is adjusted for back titration with a metal ion solution?* Replacement Residual Alkalimetric Direct Which reagent will form a more stable complex with interfering ions rather than the with the indicator and EDTA?* Masking agents Demasking agents Chelating agents Complex agents Which of the following contains a set of incorrectly paired words?* Chelatometry - Complexation / Precipitimetry - Argentometric…
A 0.87 g sample containing Ni (Mwt 58.693) was precipitated with dimethylglyoxime as Ni(II)/DMG complex (Mwt 288.91). Find the percentage (%) of Ni in the sample if the precipitate weighed 3.20 g.
vity/Student Guide Big Idea Assessments A certain brand of zinc cold medicine is marketed as containing 5.0 mg of zinc in every lozenge. A student team decides to test this claim with a complexometric titration. Xylenol orange forms a red complex with zinc ions, but is yellow when it is free. EDTA is able to form much stronger complexes with zinc ions. For their analysis, the students dissolve one colorless lozenge in a small amount of buffer. They add a few drops of the xylenol orange indicator, then titrate with EDTA. The end point is achieved with 19.36 mL of EDTA. 1. How do the students know when the end point is achieved? Describe what happens to the substances involved in the reaction when the end point is achieved. Explain any observations that may be noted by the students. 2. What concentration of EDTA should the students use so that approximately 25 mL of titrant would be needed to reach the end point if the lozenge contained the 5.0 mg of zinc claimed by the manufacturer? 3.…
5. A 300.0 mg sample containing Na,CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
All of the following regarding Argentometric titration are correct except: a. Chromate indicator is used in Mohr method b. Smaller values of Ksp give sharper break or inflection at end point c. Increasing reagent concentration makes the change in pAg smaller. d. Volhard's method involves adding excess AgNO3 to the analyte, then back titration with standard SCN solution. e. Fajan's method depends on adsorption of fluorescence indicator on the colloidal precipitate formed Please fill in the space with one of the following characters (a or b or c or d or e) Answer:
A 25.00 mL unknown water sample is titrated with a standardized 0.0140 M EDTA solution. It is determined that 8.54 mL of EDTA is required to reach the end point. The blank titre was determined to be 1.50 mL. Determine the concentration of Calcium in the water sample in ppm. (mwt. of CaCO3 = 100.0892 g/mol).
5. A water supply company, One Team, found out that their water supply had been contaminated with a sparingly soluble magnesium salt. They requested the help of Magent Analytical Laboratory to identify the magnesium salt. They chose to identify this using Ksp determination after narrowing it down to 2 salts: Salt MgCO3 Mg(OH)2 Theoretical Ksp 3.5 x 10-8 1.8 x 10-11 For the standardization of the HCl titrant, 5.230 mg Na2CO3 (98.9% purity, MW = 105.99 g/mol) required 24.4 mL of the titrant to reach the phenolphthalein endpoint. After isolating and precipitating the magnesium salt A, a portion was dissolved in distilled water in order to make a 250.0-mL saturated solution. The titration of a 50.0-mL aliquot of the saturated solution required 8.20 mL of HCl titrant to reach the phenolphthalein endpoint. Meanwhile, dissolving this magnesium salt in 250.0 mL of 0.0200 M MgCl2 required 1.51 mL of the same HCl titrant to titrate a 100.0-mL solution. a. What is the molarity of the HCl titrant?…
2. What concentration of OH is required to begin the precipitation of Cu(OH)2 from a solution containing 0.10 M Cu²+? Ksp for Cu(OH)2 = 2.2 x 10-20. a) 0.20 M b) 1.1 x 10-20 c) 4.7 x 10-10 d) 6.0 x 10-7 e) None of the above JAGill Dl Cl proginitato form?