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- A 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.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?Explain brieflyWhat would happen to the total hardness if the solution was buffered to pH 13.00? What is done to the soda ash solution when the pre-equivalence point of the methyl orange endpoint is reached? What compound is trying to be removed?
- b. 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?Explain why in Mohr's method neutral medium should be used in titration of AgNO3?In this activity, you will develop an experimental procedure to solve a problem. Consider the followingscenario:You are the manager of a chemical stockroom, and find a bottle containing approximately one liter of aclear and colorless solution of unknown identity and concentration. Your only clue to its identity is thatit was found between bottles of silver fluoride and sodium fluoride, so it is likely an aqueous solution ofone of those two compounds. You will need to develop a procedure to determine the following:a) The identity of the unknown solutionb) The concentration of the unknown solutionWrite out a precise procedure, which includes all glassware, reagents, and steps. You will also need towrite the calculations that you would need to determine the concentration of the solution. Assume thatyou have access to any reagent you might need
- 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.The sulfur content of insoluble sulfides that do not readilydissolve in acid can be measured by oxidation with Br2to SO42.25Metal ions are then replaced with Hby an ion-exchange column,and sulfate is precipitated as BaSO4with a known excess ofBaCl2. The excess Ba2is then titrated with EDTA to determinehow much was present. (To make the indicator end point clearer,a small, known quantity of Zn2also is added. The EDTA titratesboth the Ba2and the Zn2.) Knowing the excess Ba2, we cancalculate how much sulfur was in the original material. To analyzethe mineral sphalerite (ZnS, FM 97.46), 5.89 mg of powderedsolid were suspended in a mixture of CCl4and H2O containing1.5 mmol Br2. After 1 h at 20 C and 2 h at 50 C, the powder dis-solved and the solvent and excess Br2were removed by heating.The residue was dissolved in 3 mL of water and passed throughan ion-exchange column to replace Zn2with H. Then 5.000 mLof 0.014 63 M BaCl2were added to precipitate all sulfate as BaSO4.After the addition of…A 25.00 ml of Ni2+ solution was diluted in HCl and treated with 25.00 ml of 0.05283 MNa2EDTA. The solution was neutralized with NaOH followed by addition of acetate buffer untilthe pH 5.5. The solution turns yellow after addition of few drops of xylenol orange indicator.Back titration using standard 0.022 MZn2+ at pH 5.5 requires 17.61 ml until end point, onwhich the solution will turn red. Calculate for the molarity of the unknown.
- What volume of 0.317 M KOH solution will be required to titrate 25.00 ml of 0.285 MHNO3?A suitable target for the titration is 30.0 cm3 of 0.025 moldm-3 Br2(aq) Justify why a much smaller target titre would not be appropriate Calculate the amount in moles of bromine in the target titer Justification? calculate a suitable massof alive oil to transfer to the volumetric flask using your answer to of above question and the structure of Y Assume that the olive oil contains 85/- of Y by mass (If you were unable to calculate the amount of bromine in the target titer,you should assume it is 6.25×10^-8 mol .this in not the correct amount)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.