1. Volhard method could be used to analyze both silver and halides ions. True False 2. The indicator for the Mohr method is Fe3+. True False 3. Mohr method is an example of a back-titration method. True False
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1. Volhard method could be used to analyze both silver and halides ions.
- True
- False
2. The indicator for the Mohr method is Fe3+.
- True
- False
3. Mohr method is an example of a back-titration method.
- True
- False
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- What volume of 0.0105 -M HBr solution is required to titrate 125 mL of a 0.0100 – M Ca(OH)2 solution? Ca(OH) 2(aq) + 2HBr(aq) → CaBr2(aq)2H2O(1) a. 0.0776 mL b. 24.8 mL c. 77.26 mL d. 0.248 mLA solution containing KCl (74.551 g/mol) is analyzed by the Mohr method. A 0.5863 g sample is dissolved in 100 mL of water and titrated to the Ag2CrO4 end point, requiring 42.20 mL of 0.0350 M AgNO3. A blank titration requires 0.80 mL of titrant to reach the same end point. Report the %KCl in the sampleWhich of the statements given below is correct? A. Iodometry is a method in which 12 solution is used as a titrant and the substances that can reduce iodine to iodine can be determined. B. Starch indicator is added to the medium at the beginning of the titration. C. All metal salts other than alkali salts dissolved in water cause hardness properties. D. 1 German hardness is the hardness of water containing cation equivalent to 1 mg CaCO3 per 100 mL.
- A 20.00 ml sample of 0.520 M oxalic acid is titrated with 26.50 ml of an unknown KmnO4 solution. a). How many moles of oxalic acid were present in this titration? b). How many moles of KMmO4 were needed for the reaction? c). What is the molarity of the KMnO4 solutionThe Borax solution (Na2B4O7) was standardized by titrating 20.00 mL of sample with 1.044 M solution of H2SO4. It takes 2.63 mL of this H2SO4 to reach the end point. What was the concentration of this Borax solution? B4O72-(aq) + 7 H2O(l) → 2 B(OH)3(aq) + 2 B(OH)4- (aq) 2 B(OH)4- (aq) + H 2SO4(aq) → 2 B(OH)3(aq) + 2 H2O(l) + SO42- (aq)The Borax solution (Na2B4O7) was standardized by titrating 20.00 mL of sample with 1.044 M solution of H2SO4. It takes 2.63 mL of this H2SO4 to reach the end point. What was the concentration of this Borax solution?B4O7 2– (aq) + 7 H2O(l) → 2 B(OH)3(aq) + 2 B(OH)4 – (aq) 2 B(OH)4 – (aq) + H2SO4(aq) → 2 B(OH)3(aq) + 2 H2O(l) + SO4 2– (aq)
- The lead in a 0.2000-g sample is precipitated as PbCrO4. The precipitate is filtered, washed, and dissolved in acid giving a solution containing dichromate ions and lead ions. The dichromate requires 15.50 ml of 0.1 M ferrous sulfate for titration. Calculate the percentage of lead in the sample.The Kjeldahl method was used to determine the nitrogen content of a soil sample. 25 g soil sample was digested and the liberated ammonia distilled into 10 mL of 0.05 M HCI, which was used in the subsequent back titration. The unreacted HCL required 13.25 mL of 0.025 M NaOH for complete titration. Calculate the Total Kjeldahl Nitrogen (TKN) in mgkg-' N.0.300 g of a nitrogen-containing sample is analyzed by the Kjeldahl method and the released ammonia is collect in boric acid. The resulting solution (borate) is titrated with 0.100 M HCl consuming 25.0 mL. What is the percentage of nitrogen in the sample? (Pat N, 14.0)
- 31 What volume of 0.0125 M HBr solution is required to titrate 1.25mL of a 0.100M Ca(OH)2 solution? Ca(OH)2 + 2HBr ----------> CaBr2 + 2H2 Select one: a. 400. mL b. 120. mL c. 200. mL d. 400.mLStandardization of 0.10 M HCl1. Take three (3) clean and properly labeled 250-mL Erlenmeyer flasks. Into the three flasks, weigh 0.1 g of the primary standard Na2CO3 to the nearest 0.1 mg. Record the weights of the primary standard.2. Add about 75.0 mL of boiled distilled water and swirl to dissolve the solids.3. Add 2 to 3 drops of phenolphthalein indicator. Record the initial burette reading and titrate with the prepared 0.10 M HCl solution until phenolphthalein endpoint.4. Record the final burette reading for each titration in your data sheetDetermination of Ksp and Molar Solubility1. Add Ca(OH)2 to 250.0 mL distilled water with stirring until equilibrium is achieved. 2. Filter the undissolved precipitate. Measure out 50.0 mL of the supernate into a 250-mL Erlenmeyer flask using a pipette.3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved.4. Record the volume the HCl solution used. Perform two more trials.…Standardization of 0.10 M HCl1. Take three (3) clean and properly labeled 250-mL Erlenmeyer flasks. Into the three flasks, weigh 0.1 g of the primary standard Na2CO3 to the nearest 0.1 mg. Record the weights of the primary standard.2. Add about 75.0 mL of boiled distilled water and swirl to dissolve the solids.3. Add 2 to 3 drops of phenolphthalein indicator. Record the initial burette reading and titrate with the prepared 0.10 M HCl solution until phenolphthalein endpoint.4. Record the final burette reading for each titration in your data sheetDetermination of Ksp and Molar Solubility1. Add Ca(OH)2 to 250.0 mL distilled water with stirring until equilibrium is achieved. 2. Filter the undissolved precipitate. Measure out 50.0 mL of the supernate into a 250-mL Erlenmeyer flask using a pipette.3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved.4. Record the volume the HCl solution used. Perform two more trials.…