ulometry is based on measu number of electrons that ticipate in a chemical react ventional titrations are bet n coulometric titrations whe all amounts of analte are
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- You have performed an iodimetric titration using a commercial vitamin C tablet. Based on the following information below, calculate the %(w/w) of vitamin C(MM=176.16 g/mol) in the tablet: Mass of tablet dissolved in 250.0 mL: 5.422 g Aliquot volume of sample titrated: 25.00 mL Concentration of KIO3: 0.023 M Final burrette volume: 41.31 mL Initial burrette volume: 8.89 mL Blank volume: 0.14 mLIn developing a method for the determination of formic acid by neutralization volumetry, an analyst calculated the pH as a function of the addition of NaOH for the titration of 30.00 mL of 0.1280 mol/L formic acid with standardized NaOH with concentration of 0.1570 mol/L. With respect to this titration curve, determine the pH of the solution after adding the following volumes of NaOH: 0.00 mL; 10.00 ml; 25 mL of titrant and at the equivalence point. Data: Ka=1.70x10-4. Present the results with two decimal places and show your calculations.A stock standard concentration of 101.25ppm was prepared of Cu. What are the actual concentrations of the working standards prepared in 100mL volumetric flasks, using 1mL, 5mL, 8mL, and 10mL volumes of the stock standard?
- The Ksp for silver chromate (Ag2CrO4) is 1.1x10-12. Using the same initial set up of 10mL of 1M silver nitrate is combined with 25mL of 0.1M sodium chromate, what is the mass of the silver chromate precipitate in grams?Will a precipitate form when 75ml of 0.20 M AgNo3 are combined with 266 mL of 0.050 M NaCl? The Ksp for AgCl=1.8 x 10^-10. ( Report Qsp)The solubility product constant of potassium bitartrate (KHC4H4O6) was determined by titrating a saturated solution of KHC4H4O6 with a standardized solution of 0.025 M NaOH, using phenolphthalein as indicator. The neutralization reaction is: HC4H4O6–(aq) + OH–(aq) ↔ C4H4O62–(aq) + H2O(l) The table below shows the data gathered from the experiment. Initial buret reading, mL 10.75 Final buret reading, mL 44.20 Volume of KHC4H4O6 solution, mL 25.00 Write the dissociation reaction for KHC4H4O6 and its molar solubility and solubility product constant.
- The solubility product constant of potassium bitartrate (KHC4H4O6) was determined by titrating a saturated solution of KHC4H4O6 with a standardized solution of 0.025 M NaOH, using phenolphthalein as indicator. The neutralization reaction is: HC4H4O6–(aq) + OH–(aq) ↔ C4H4O62–(aq) + H2O(l) The table below shows the data gathered from the experiment. Initial buret reading, mL 10.75 Final buret reading, mL 44.20 Volume of KHC4H4O6 solution, mL 25.00 Write the dissociation reaction for KHC4H4O6 and its molar solubility and solubility product constant. Determiner the ff. volume of NaOH used moles of OH- usedGiven the volume of 0.1416 M NaOH used determine the concentration of 16 ml sample each from aquaeous layer (Aq) and benzene layer (Or). To reach the end point of Aquqeous layer and organic layer 13.16 ml and 14.00 ml of NaOH used respectively using Phenolppthalein indicator. What will be the Kd of the system?1ml of 1mg/ml of diluted aspirin powder solution is titrated by 0.005M NaOH. Before titration, 5 ml ethanol, 14 ml CO2 free water, and 4 drops bromothymol blue indicator is added into diluted aspirin powder solution. Mass of 0.005M NaOH used is obtained by weight titration = 1.1384g . [Molar mass of aspirin =180.15]; for solution, 1g=1mL at 25 degree Celcius. Calculate the purity of the powder.
- b) In the development of a method for the determination of formic acid by neutralization volumetry, the pH was calculated as a function of the addition of NaOH for the titration of 25.00 mL of 0.1280 mol/L formic acid with NaOH standardized with concentration of 0.0670 mol/L. With reference to this titration curve, determine the pH of the solution after the addition of 5.00 mL of titrant and at the equivalence point. Data: Ka=1.70x10-4. Present the results with two places after the comma and show your calculations. c) Based on the table below, indicate which indicators could be used to determine the end point of this titration.An approximately 0.1-molar solution of NaOH is to be standardized by titration. Assume that the following materials are available. Clean, dry 50 mL buret •Analytical balance 250 mL Erlenmeyer flask •Wash bottle filled with distilled water Phenolphthalein indicator solution Potassium hydrogen phthalate, KHP, a solid monoprotic acid (to be used as the primary standard) Briefly describe the steps you would take, using the materials listed above, to standardize the NaOH solution. Describe (the set up) the calculations necessary to determine the concentration of the NaOH solution.Suppose 100 mL of 2.0 × 10–4 M Fe(NO3)3is added to 100 mL of 2.0 ×10–5 M KIO3. What is Qsp value? Will it precipitate?