Condition of permanganatometric titration of sodium oxalate includes: pH = 1 and heating of analyte solution till 70° C; pH = 7 and heating of analyte solution till 70° C; pH = 10 and heating of analyte solution till 70°C; pH = 1 under room temperature; %3D
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- An alkaline sample of sodium compounds weighing 1.196 g was dissolved in water, cooled at 15 deg C, treated with 2 drops of phenolphthalein indicator and titrated with 1.058 N H2SO4 requiring 6.8 mL to render the solution colorless. Upon adding 2 drops of methyl orange and continuing the titration 16.5 mL more of the acid was needed to complete analysis. What is the quantitative composition of the sample?A 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was addedDetermination of sodium carbonate by acidimetric titration involves: Direct titration by acid solution with usage as indicator either methyl orange or phenolphthalein; heating of analyte till 70° C; Direct titration by acid solution with sequential usage of 2 indicators: methyl orange and phenolphthalein; Back titration by acid solution with usage as indicator phenolphthalein;
- A substance contains 0.5 g of magnesium hydroxide as the only basic ingredient . The sunstamce is analysed by dissolving it and titrating with a standard hydrochloric acid solution .The hydrochloric acid solution used in this titration is made by diluting 200 ml of 2M standardised solution to 500 ml 1.Calculate the volume of the HCl solution required to neutralize two of these indigestion substaces dissolved in water to make 35ml solution and calculate the concentration of Cl- in the final solution in mol.dm-31. A 0.3516 g sample of commercial phosphate detergent was ignited at a heat to destroy the organic matter. The residue was taken up in hot HCI which converted P to H3PO4. The phosphate was precipitated as MGNH4PO4.6H2O by addition of Mg+ followed by aqueous NH3. After being filtered and washed, the precipitate was converted to Mg2P2O7 by ignition at 1000 OC. This residue weighed 0.2161 g. Calculate the percent P (30.974) in the sample? Ans 17.11%A 10.00cm3 portion of the 100.00cm3 HCl solut was taken from the volumetric flask and was titrated with KOH (aq). It was neeutralized by 24.35cm3 of potassium hydroxide od concentration 0.0500moldm-3. Calculate the concentrat of the original concentrated hydrochloric acid in moldm-3.
- Water sample from different river water was subjected to a qualitative alkaline analysis by titrating against 0.1250 MHC1 and using phenolphthalein and bromocresol green end point. The table below shows the volumes of acid needed to titrate 25.00-mL portions of each sample and their corresponding end point, separately. Use this information to deduce the composition of the solutions. Calculate the molar concentration of each solute. Volume (mL) Phenolphthalein end Bromocresol green Solute identity concentration end point Volume (mL) Molar Sample point 22.40 of solute/s 1 22.41 2 0.00 33.40 3 15.67 42.13 4 29.64 36.42To determine the concentration of glucose in the packaged juice industry, 50 mL of sample is analyzed. Analysis of it (and other reducing sugars) was carried out there using triiodide back titration. An excess volume of 75.00 mL of 0.338 M triiodide standard solution in alkaline medium was added to the glucose solution. The resulting solution was acidified and the excess triiodide was titrated with 18.37 mL of standard 0.526 M thiosulfate solution. Calculate is the concentration in ppm in the sample. In alkaline medium: Glucose (C6H12O6) / Gluconate (C6H11O7-), Triiodide (I3- ) / Iodide (I-) In acid medium: Thiosulfate (S2O32-) / Tetrathionate (S4O62-), Triiodide (I3- ) / Iodide (I-)A NazCO3 standard solution is prepared by transferring 2.4817 grams of primary standard-grade sodium carbonate to a 250.0 mL volumetric flask, dissolving the sample in -100 ml of distilled deionized water, and diluted to the mark. A 25.00 mL aliquot is taken and titrated with 42.65 mL of HCI solution to the bromocresol green endpoint. Calculate the concentration of the HCI solution. (A 0.1598 M B 0.1098 M c) 0.3196 M (D) 0.05490 M
- The active ingredient in a certain toilet cleaner that claims to 'remove lime scale and rust' is hydrochloric acid of approximate concentration 10.9 mol/L. To analyze this toilet cleaner, a quality control chemist first delivered a 10-mL aliquot of the toilet cleaner into a 250-mL volumetric flask, then made up the diluted solution. She then titrated a 25 mL aliquot of this diluted solution against standard sodium hydroxide solution of concentration 0.46 mol/L. The expected titre (or volume of the titrant in mL) would be approximately:E. Analysis of a mixture consisting of NaOH + NażCO3 + inert matter gives the following data: Sample portions are titrated. With one portion, an end point with phenolphthalein is obtained in cold solution, with 44.52 mL of 0.5000 N HCI. The other portion requires 46.53 mL of the acid for an end point with methyl orange. Calculate the percentage composition of the original sample. 10.00 g. Its aqueous solution is diluted to 250.0 mL and two separate 25.00 mLA 4.912-g sample of a petroleum product was burnedin a tube furnace, and the SO2produced was collectedin 3% H2O2.Reaction:SO2(g)+H2O2→H2SO4A 25.00-mL portion of 0.00873 M NaOH was introducedinto the solution of H2SO4, following whichthe excess base was back-titrated with 15.17 mL of0.01102 M HCl. Calculate the sulfur concentrationin the sample in parts per million.