One of the following statements is incorrect: O A primary standard should be highly pure, has atmospheric stability and absence of hydrated water O Titration error is the difference between equivalence point volume and end point volume O Standardization is not required when the titrant solution molarity is approximate O A standard solution should react completely with the analyte with a definite chemical equation O Back-titration is required when the rate of the reaction slow

One of the following statements is incorrect: O A primary standard should be highly pure, has atmospheric stability and absence of hydrated water O Titration error is the difference between equivalence point volume and end point volume O Standardization is not required when the titrant solution molarity is approximate O A standard solution should react completely with the analyte with a definite chemical equation O Back-titration is required when the rate of the reaction slow

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter24: Coulometry

Section: Chapter Questions

Problem 24.12QAP

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One of the following statements is incorrect: O Titration error is the difference between equivalence point volume and end point volume O A primary standard should be highly pure, has atmospheric stability and absence of hydrated water O Back-titration is required when the rate of the reaction slow O A standard solution should react completely with the analyte with a definite chemical equation O tandardization is not required when the titrant solution molarity is approximate
One of the following statements is incorrect Select one: O Back-titration is required when the rate of the reaction slow. 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. O A primary standard should be highly pure, has atmospheric stability and absence of hydrated water. O Titration error is the difference between equivalence point volume and end point volume.
One of the following statements is incorrect: oStandardization is not required when the titrant solution molarity is approximate O Back-titration is required when the rate of the reaction slow O A primary standard should be highly pure, has atmospheric stability and absence of hydrated water oTitration error is the difference between equivalence point volume and end point volume O A standard solution should react completely with the analyte with a definite chemical equation
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.
Acid-Base titration: Standardization of 0.1 M NAOH Trial 1 Mass KHP used, g 0.297 g Final reading Volume NaOH, mL 15.59 mL Initial reading Volume NaOH, mL 0.23 mL Volume NaOH consumed, mL 15.36 mL Moles KHP used Moles NaOH used Molarity of NaOH solution
One of the following statements is incorrect: Titration error is the difference between equivalence point volume and end point volume Back-titration is required when the rate of the reaction slow Standardization is not required when the titrant solution molarity is approximate A standard solution should react completely with the analyte with a definite chemical equation A primary standard O should be highly pure, has atmospheric stability and absence of hydrated water
5. A 300.0 mg sample containing Na,CO3, NaHCO, 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.
Which of listed methods belongs to complexometric titration? mercurimetry; thiocyanate-metry; hexacyanoferrate-metry; sulfate-metry.
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?
If 2.00 ml of 0.200M NAOH are added to 1.00 L of 0.100M CaCl2, will a precipitate form? Ksp Ca(OH)2= 8.0 x 10-6 Sample answer format: 1.0x10-14(YES) (Note: Case, Space, and format sensitive)
11. A 0.485 g sample containing chloride was titrated with 36.8 mL of 0.1060 M AgNO3 stock solution. Express the results of this analysis in:a) Percent by weight of Clb) Weight percent Cl2c) Percent by weight of CaCl2d) Weight percent of AlC13
Concentration sodium thiosulfate solution used: 0.056 mol L-1 ACCURATE TITRATION VOLUME OF SODIUM THIOSULFATE SOLUTION USED Volume titration 1, (mL) Volume titration 2, (mL) Your Group 15.80 15.75 Group 1 16.05 15.70 Group 2 16.30 16.25 ANALYSIS Average volume used, (ml) Standard deviation Number of moles sodium thiosulfate used, (mol) Number of moles calcium iodate in solution, (mol) Volume of calcium iodate used, (mL) Concentration of saturated calcium iodate solution (mol L-¹) Unrounded value 15.9750 0.26220 0.00089400 0.00036700 A Rounded value 15.97 0.262 8.94 x 10-4 10.0 Minimize