One of the following statements is incorrect: A primary standard should be highly pure, has atmospheric stability and absence of hydrated water O A standard solution should react completely with the analyte without a definite chemical equation Standardization is required when the titrant solution molarity is approximate Back-titration is required when the rate of the reaction slow Titration error is the difference between equivalence point volume and end point volume

One of the following statements is incorrect: A primary standard should be highly pure, has atmospheric stability and absence of hydrated water O A standard solution should react completely with the analyte without a definite chemical equation Standardization is required when the titrant solution molarity is approximate Back-titration is required when the rate of the reaction slow Titration error is the difference between equivalence point volume and end point volume

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter20: Molecular Spectroscopy And Photochemistry

Section: Chapter Questions

Problem 67CP

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Which of the following accurately corresponds to the composition of the precipitate obtained from a mixture of proteins A and B (properties below) by employing the specified (NH4)2SO4 concentration assuming the salt is added in bulk i.e. one step? Protein % (NH4)2SO4 to precipitate A 40 B 70 a. At 30% (NH4)2SO4 : A b. At 40% (NH4)2SO4 : B c. At 60% (NH4)2SO4 : A d. At 70% (NH4)2SO4 : B e. None of the above
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Quantitative analysis of metal ions in pharmaceutical and cosmetic products can be done using direct and indirect complexometric titrations employing concepts of complex formation, masking, and blocking. For example, all Fe3+, Mg2+, Al3+ and Zn2+ can form a complex with EDTA at pH 10. However, at pH 5, Mg-EDTA complex formation is inhibited, whereas at pH 2, only Fe-EDTA complex formation is favored. Knowing these, an analyst tried to determine the % composition of a 0.1000 g sample containing soluble salts of Fe3+, Mg2+, and Al3+. The sample was initially dissolved in 250.0 mL of distilled water. To determine the total ion content of the sample, a 50.00 mL aliquot was buffered to pH 10.00 before adding 50.00 mL of 0.0500 M EDTA, and the excess EDTA was back titrated with 24.18 mL of 0.0750 M standard Zn2+ solution until the EBT endpoint. Another 50.00 mL aliquot was buffered to pH 2.00 and was added with small amount of SCN- producing blood-red Fe(SCN)2+ complex. This was titrated…
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Q: The concentration of the sulphate ion in a mineral water can be determinedby the turbidity which results from the addition of excess BaCl2, to a quantityof measured sample. A turbidometer used for this analysis has been standardisedwith a series of standard solutions of NaSO4. The following resultswere obtained:Standard solution Conc. (SO4)2− (mg/L) Reading of turbidometerS0 0.00 0.06S1 5.00 1.48S2 10.00 2.28S3 15.00 3.98S4 20.00 4.61i. In supposing that a linear relationship exists between the readings takenfrom the apparatus and the sulphur ion concentration, derive an equationrelating readings of the turbidometer and sulphate concentration(method of least squares).ii. Calculate the concentration of sulphate in a sample of mineral waterfor which the turbidometer gives a reading of 3.67.
What is/are the principle/s involved on ACIDIMETRIC ASSAY BY DOUBLE INDICATOR TITRATION?
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A student has a sea water sample which contains Ca2+ ions . Describe briefly how he willdetermine the concentration of Ca2+ ion in the sample using a simple titration. Explain the colourchanges at the endpoint. Which medium is suitable for performing the titration, acidic or basic medium and why?
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