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- Why use basic buffer solution in an experiment for hard water analysis?What makes bromocresol green and phenolphthalein suitable for the double-indicator process?Explain the reason behind the addition of the starch indicator near the endpoint for this analysis. What is the consequence when the solution is colorless before addition of the starch indicator?
- What factor affects the ‘strength’ of a buffer? Why was benzoic acid used as a solvent when making up the glucose stock standard solution?Describe why the inside wall of the flask is rinsed with deionized water during accurate titration. Does this washing affect the molar quantity of acetic acid in the sample? Describe..?In the Assay of Sodium Chloride, what is the purpose of adding nitric acid in the solution? It is used to prevent precipitation of silver as carbonate It is used to hasten chemical reaction It is used to precipitate silver bromide It is used to form a film over silver nitrate precipitate What is the permanent color expected at the end point in the standardization of 0.1 N Ammonium Thiocyanate? * Orange red Blue Red Yellow In the Standardization of 0.1 N Silver Nitrate, what is the purpose of allowing the mixture to stand in the dark? * It is used to aid in the formation of precipitate with large particles It is used to prevent the production of free silver It is used to acquire a purplish color in the precipitate It is used to maximize the reduction of silver chloride In the standardization of 0.1 N Silver Nitrate, what is the most suitable temperature to dry the Silver Chloride precipitate to constant weight? * 115° C 110° C 100° C 120° C Which is NOT…
- Standard solution : 0.201 grams of acetylsalicylic acid was combined with 10 mL of 0.5 M NaOH, then transfered to a 100 mL flask and filled the rest of the way with water Then 0.500 mLs of the standard solution was transfered to a 10.00 mL flask and diluted to the 10 mL mark with 0.02 M of buffered iron chloride. Number of moles of NaOH = 0.005 moles Since the reaction between acetylsalicylic acid and NaOH is a 1:1 reaction, the number of moles of acetylsalicylic acid used in the reaction is also 0.005 moles. the concentration from analysis question 5: acetylsalicylic acid in the 100.00 mL volumetric flask is 0.050 M. From your plot, what is the value of εb? From the Beer- Lambert law For the aspirin sample, calculate the concentration of acetylsalicylic acid present using the value of εb that you found The concentration from analysis question 5 represents the concentration in the 10.00 mL sample that was prepared in the volumetric flask using an aliquot of the solution in the…An impure sample containing carbonate and sodium bicarbonate, weighing 0.5 g, was taken. It was dissolved in distilled water and then flushed with 0.1 N hydrochloric acid. If the burette reading at the end point of the phenolphthalein index is 10.5 milliliters, and at the orange methyl index end point it is equal to 30.1 milliliters. So, the percentage of sodium bicarbonate in the sample is ............., knowing that the molecular weight of sodium bicarbonate is 84 g/mol.Discuss the role of indicators for the titration procedure *
- Determine each statement if it is positive or negative base on the chemical structure in the picture. Green flame with Beilstein’s test White precipitate with silver nitrate Black residue due to complete combustion White precipitate with BaCl2 solution Yellow precipitate with ammonium molybdate Red precipitate with Millon’s Reagent Violet color with FeCl3 SolutionWhich are TRUE for the use of indicators with dichromate? I Dichromate is orange and changes color to green when reduced. The color change is abrupt enough to serve as an indicator.II The equivalence point for dichromate can be determined using Pt and calomel electrodes.III Dichromate end points are determined using the distinct color changes of diphenylamine sulfonic acid or diphenylbenzidine sulfonic acid indicators.IV In basic solution, the orange dichromate solution changes color to yellow when reduced to chromate anion. The color change is abrupt enough to serve as an indicator. A. I and III B. II and III C. I and IV D. II and IV E. I, II, and IVAssess the suitability of methyl orange to signal the equivalence point in weak acid and strong base of the experiment. Use the pH range over which the methyl orange changed colors to make this determination. If you conclude that methyl orange would not reliably indicate the equivalence point in this reaction, then suggest an alternative indicator which would be more appropriate.