A 300.0-mg sample containing H3PO4 and inert material was diluted with water and titrated with 0.05000M NaOH. The endpoint was reached after 29,00mL of the titrant was added. Calculate the % H3PO4. (97,994 g/mole) in the sample. H3PO4 + NaOH > Na,HPO, + 2H2O
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A 300.0-mg sample containing H3PO4 and inert
material was diluted with water and titrated with
0.05000M NaOH. The endpoint was reached after
29,00mL of the titrant was added. Calculate the %
H3PO4. (97,994 g/mole) in the sample.
H3PO4 + NaOH > Na,HPO, + 2H2O
Step by step
Solved in 3 steps
- 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)A 0.1093-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of 0.06911 M AgNO3, the sample was back-titrated with 0.05781 M KSCN, requiring 27.36 mL to reach the endpoint. Report the purity of the Na2CO3 sample. [Ans. 90.9 % (w /w )]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.
- A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask. 20.00 mL aliquot was mixed with 30.00 mL water and subjected to digestion with concentrated H2SO4. The ammonia produced is collected in 30.00 mL of 0.0500 M HCl and the excess acid is back titrated with 0.0500 M NaOH, requiring 6.80 mL. Calculate the weight percent urea [(NH2)2CO, FW=60.06 g/mol] in the sample. Please use the factor label method in answering.A 1.0 g sample containing urea was dissolved in water and diluted in a 100.00 mL volumetric flask. 20.00 mL aliquot was mixed with 30.00 mL water and subjected to digestion with concentrated H2SO4. The ammonia produced is collected in 30.00 mL of 0.0500 M HCl and the excess acid is back titrated with 0.0500 M NaOH, requiring 6.80 mL. Calculate the weight percent urea [(NH2)2CO, FW=60.06 g/mol] in the sample.Twenty sodium salicylate tablets labeled 325 mg were dispersed in sufficient water to make 200.0 mL. A 15.0–mL aliquot of the filtrate was titrated to a bromophenol blue endpoint in the usual way by 32.11 mL of 0.1000 N hydrochloric acid. Calculate the amount of sodium salicylate in each tablet, and from that, the percentage of the labeled amount. (NaC7H5O3 MW = 160.11 g/mol) Amount of sodium salicylate in each tablet = % labelled amount =
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- The SO2 present in air is mainly responsible for the phenomenon of acid rain. The concentration of SO2 can be determined by titrating against a standard permanganate solution as follows: 5SO2 + 2MnO4- + 2H2O ---> 5SO42- + 2Ms2 + 4H+ Calculate the number of grams of SO2 in a sample of air if 4.90mL of 0.00700M KMnO4 solution are required for the titration. Be sure your answer has the correct number of significant digits.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 = 67An aqueous solution of 0.2100 g of a mixture containing potassium cyanide and potassium chloride required 14.56 mL of 0.1000 M silver nitrate to produce a faint permanent turbidity; 30.00 mL more of the silver nitrate was added (an excess) and the precipitate of AgCl and AgCN filtered off from the solution. The filtrate and washings were titrated with 13.06 mL 0.1000 M thiocyanate solution. Calculate the percentages of KCl and KCN in the sample.