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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.Using basic conditions, MnO4- can be used as titrant for the analysis of Mn2+, with both the analyte and the titrant ending up as MnO2. In the analysis of a mineral sample for manganese, a 0.5165-g sample is dissolved, and the manganese is reduced to Mn2+. The solution is made basic and titrated with 0.03358 M KMnO4, requiring 34.88 mL to reach the endpoint. Calculate the %w/w Mn in the mineral sample. Answer: % Mn =400 g sample containing chloride ions (MW=35.45 g/mol) was dissolved in 50.0mL of distilled water. A 15.0 mL aliquot was taken, and was further diluted to 50.0 mL using distilled water. The diluted solution was then titrated using a 0.0989 M AgNO3 solution, and it consumed a total of 31.9 mL of the titrant in order to reach the end point. What is the concentration of the undiluted chloride solution? Round off to three (3) significant figures. What is the % (w/v) concentration of the undiluted chloride solution? Round off to two (2) decimal points. What is the % (w/w) of Cl- composition of the sample? Round off to two (2) decimal points.
- a) What mass of Fe(NH4)2(SO4)2•2H2O(s) is required to prepare a 500 mL solution containing 100 ppm (m:v) in Fe? b) Using this stock solution, what aliquot must be used to prepare calibration solutions, 100 mL volume, of the following concentrations: 0.100 ppm, 0.500 ppm, 2.00 ppm, 4.00 ppm, and 7.00 ppm.A 20 ml aliquot of malonic acid solution was treated with 10.0 ml of 0.25M Ce4+ leading to the reaction CH2(COOH)2 + 6Ce4+ + 2H2O ® HCOOH + 2CO2 + 6Ce3+ + 6H+ After standing for 10 minutes at 60oC, the solution was cooled and the x’ss Ce4+ was titrated with 0.1M Fe2+, requiring 14.4 ml to reach the ferroin end point. Calculate the M of the malonic in the sample.1. 1093-g sample of impure Na2CO3 was analyzed by residual precipitimetry. 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. The percentage Na2CO3 (MW = 106.0 g/mole) in the tested sample is ________ % ? Note: Express final answer using least number of significant figures. 2. The alkalinity of natural waters is usually controlled by OH- (MW = 17.01 g/mole), CO3-2 (MW = 60.01 g/mole), and HCO3- (MW = 61.01 g/mole), which may be present singularly or in combination. Titrating a 10.0-mL sample to a phenolphthalein endpoint requires 38.12 mL of a 0.5812 M solution of HCl, and an additional 18.67 mL of the same titrant to reach the methyl orange endpoint. The composition of the sample is _________% CO3-2 and ___________ % OH- Note: Express final answers using least number of significant figures.
- 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)Prepare 1.0 L of a 50.00 ppm iron solution from the solid Fe(NH4)2(SO4)2 of the80.0% purity. Clearly describe how to prepare this solution. If doneChlorimetric iron analysis using the calibration curve method, specify theform of preparation of 100.0 ml of each of the following standard solutions withcontents of 1.00, 5.00, 15.00 and 20.00 ppm of Fe respectively from the solutionmother (It suppose that the answers are: 0.3180, 2.00, 10.00, 20.00, 30.00 and 40.00 ml of the mother solution and dilute exactly to 100.0 mL with deionized water)calculate the mass of Sn when 50 mL of a sample containing Sn2+ is titrated with 42.00 mL of 0.0150M MnO4- to reach endpoint
- 1. A newly discovered iron ore was weighted (5.408 g) and worked up to produced 0.3785 g of ignited Fe2O3 precipitate. What is the percent purity of the iron in the sample? 2. Distinguish between equivalence point and end point.Use the following atomic masses (in g/mol): Mg = 24.31; H = 1; S = 32.06; O = 16; Na = 23; Cl = 35. 45; Ca = 40.08; C = 12.01; N = 14.01; Mg = 24.31 5.A sample of Chlorpheniramine Maleate (99.82%) weighing 0.502g was assayed by non-aqueous titrimetry and was found to be equivalent to 22.2mL of perchloric acid. Calculate for the normality of perchloric acid. Each mL of 0.1N perchloric acid is equivalent to 19.54mg of Chlorpheniramine Maleate.Ten grams of soil were displaced with 250 mL of 1 M ammonium acetate and made to a final volume of 1 L. Analysis of the final l-L solution showed 20 mg/L Ca, 2 mg/L Mg, 1 mg/L K, and 0.5 mg/L Na. Estimate exchangeable cations in meq/100 g soil.