A 0.1220 g vitamin C tablet was dissolves in acid. A 25.00 ml aliquot of 0.01740 M KIO3 was added along with excess KI. The resulting solution was titrated with 0.07210 M Na2S2O3, requiring 21.44 mL to reach the endpoint. calculate percent by weight of ascorbic acid in the tablet.
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- The concentration of Cl– in a 300.0-mL sample of water drawn from a fresh water acquifer suffering from encroachment of sea water, was determined by titrating with 0.0516 M Hg(NO3)2. The sample was acidified and titrated to the diphenylcarbazone end point, requiring 6.18 mL of the titrant. Report the concentration of Cl–in parts per millionApproximately 6.0mL of concentrated perchloric acid (70%) was transferred to a bottle and diluted with about 1.0L of water. A sample containing 251.5 mg of primary standard Na2B4O7.10H2O required 27.41 mL of the HClO4 solution to reach the methyl red end point. Calculate the molar concentration of the HClO4 (Fwt = 382g/mole)John wanted to determine the protein content of his blood. To do so, he obtained 1.00 mLof blood, and diluted it to 10.00 mL. From that solution, he subjected 1.00 mL to Kjeldahl analysis. After digestion, the liberated NH3 was distilled in a flask containing exactly 25.00 mL of 0.0150 M H3BO3. Titration requires 5.85 mL of standard 0.0150 M NaOH to reach the desired endpoint. If a typical blood sample contains 15.45 g N per 100 g protein, calculatethe protein content (in g/mL) in the sample of John’s blood.
- John wanted to determine the protein content of his blood. To do so, he obtained 1.00 mL of blood, and diluted it to 10.00 mL. From that solution, he subjected 1.00 mL to Kjeldahl analysis. After digestion, the liberated NH3 was distilled in a flask containing exactly 25.00 mL of 0.0150 M H3BO3. Titration requires 5.85 mL of standard 0.0150 M NaOH to reach the desired endpoint. If a typical blood sample contains 15.45 g N per 100 g protein, calculate the protein content (in g/mL) in the sample of John’s blood.Calcium fluoride is considered as a relatively insoluble compound and therefore lime or slakedlime has been considered as a possible material to remove excess fluoride in water of boreholesin certain parts of the country. The solubility product of CaF2 is Ksp = 3 x 10 – 11 and that ofCa(OH)2 isKsp =8x10-61. How much lime can be added to the water to remove 10 mg of F- ion per litre ofborehole water?(The atomic masses are Ca: 40.08; F: 19.00; O: 16; H: 1)What weight of the soda ash (impure Na2CO3) should be taken for analysis in order that the number of milliliters of 0.500 N acid used will be equal to one-half of the percentage of Na2CO3 in the sample? Note: Please include the complete solution. Thanks!
- A Fajans titration of a 0.7908-g sample required 45.32 mL of 0.1046 M AgNO3 . Express the results of this analysis in terms of the percentage of BaCl2 * H2O. (Use a MW value in 4 decimal places)A mixture contains Na2CO3, NaOH and inert matter. A sample weighing 1.500 g requires 28.85 ml of 0.5000N HCl to reach the a phenolphthalein endpoint and an additional 23.85 ml to reach the methyl orange end point. What are the percentages Na2CO3 and NaOH?In order to adjust the Potassium Permanganate solution, 0.0544g Na2C2O4 was taken and necessary experimental procedures were performed on it and the titrant consumption was found to be 7.9 mL. Accordingly, what is the concentration of KMnO4?
- Dissolved 0.273 grams of pure sodium oxalate (NaCO) in distilled water and added sulfuric acid and titration the solution at 70 ° C by using 42.68 ml of KMNO. solution and has exceeded end point limits by using 1.46 ml of standard oxalic acid (HCO) with 0.1024 N Calculate the normlity of KMNO Note that the molecular weight of sodium oxalate (NaCO) = 134 and its equivalent weight = 67A piece of Gold weighing 12,359 Kg is suspected of being contaminated with Iron. To perform an instrumental analysis and To confirm whether or not it contains Fe, a portion of the sample (0.954 g) is taken from the piece and dissolved with 25 mL of aqua regia. Heats up For its complete dissolution, it is cooled and made up to 100 mL. A 10 mL aliquot is taken from this solution and made up to 50 mL. From This last solution is given the appropriate treatment to visualize Fe+2, for which the 1,10-phenanthroline reagent is added. (it forms a complex that is red in color) and is taken to a visible spectrophotometer and with a 12 mm cell a absorbance of 0.45. Previously, a calibration curve of Fe+2 was obtained under the same instrumental conditions obtaining the following data: (view table) Calculate the purity of the gold piece, assuming impurities only due to Fe.The total cation content of natural water is often determined by exchanging the cations for hydrogen ions on a strong acid ion-exchange resin. A 25.00 mL sample of a natural water was diluted to 100.00 ML with distilled water, and 2.06 g of a cation - exchange resin was added. After stirring, the mixture was filtered and the solid remaining on the filter paper was washed with three 15.00 mL portions of water. The filtrate and washings required 16.30 mL of 0.0282 M NaOH to give a bromocresol green end point. a) Calculate the number of millimoles of cation present in exactly 1.00 L of sample. b ) Report the results in terms of milligrams of CaCO3 per liter. Only typed solution.