Dissolve 1.7 g in a mixture of 2 ml. of nitric acid (-130 g/l) TS and 40 ml of water, and proceed as described under 2.2.1 Limit test for chlorides; the chloride content is not more than 0.15 mg/g. (International Pharmacopeia 9th ed.) The analyst recorded a weight of 1.8652 g of sample using an analytical balance. Which of the following sentence/s explain/s the correct answer? The weight is within the acceptable range of weight. O The analyst used an analytical balance. O The method is a qualitative process. O There is an excess of the number of decimal places reported.
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- Example /A0.527g sample of mixture containing NazCO; and NaHCO; and inert impurities phenolphthalein endpoint and a total of 43.8mL to reach the modified methyl orange endpoint, what is the percent each of Na CO3 and NaHCO; in mixture? is titrated with 0.109M HCІ, requiring 15.7mL to reach the Solution:Mass of Sample Volume of KMnO, solution used in titration Equivalents of permanganate used Equivalents of iron (II) in sample Moles of iron (II) in sample Grams of Iron in Sample % Iron in Sample Average % Iron in Unknown Instructor's Grade for Precision in Part B. Sample Calculations Part B: 0.58179 0.68719 28.19 ml 31,96m6 007662 00266 2 11 nA 22.41 mL of NaOH solution is required to reach the phenolphthalein endpoint in the standardization with 0.276 g of solid, monoprotic primary standard acid (MW 128.33) in a 25.00 mL solution. 12.34 mLof the same NaOH solution was added to titrate 5 mL of vinegar solution to the endpoint. Calculate the mass of acetic acid in this vinegar solution (d = 1.005 g/mL).
- simple steps Find the % of sodium carbonate in a sample if 5.002 g of the sample required 29.10 cm³ of 0.7344 mol dm-³ HCl for complete neutralisation. Make sure to solve the problem using the balanced equation. Solution (a) Determine moles of HC1 (titrant, known) (b) Use a balanced equation relate moles of analyte to moles of titrant (reaction ratio) (c) Determine mass of analyte (determine unknown) and % in sampleA solution of HCl was titrated against sodium carbonate. What is the average normality of acid in the given data? (MW Na₂CO3 = 106) T2 0.3479 0.3562 0.3042 Weight (g) Initial V (ml) 0.80 1.60 35.20 36.70 39.80 Final V (mL) Vol HCl used (mL) 35.10 39.40 N of HCl (eq/L) 0.1954 0.1870 Average N of HCl (eq/L)An 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.
- MAX OF 15 MINUTES A solution contains NaOH (FM = 40), NaHCO3 (FM = 84), and NazCO; (FM = 106), either alone or in a permissible combination. Titration of a 50 mL portion to a phenolphthalein end point requires 16.3 mL of 0.100 M HCI. A second 50.0-mL aliquot requires 38.2 mL of the HCI when titrated to a bromocresol green end point. %3D %3D What is the % w/w composition of the following? Express answers in two decimal places. If the component is not present, write 0.00 in the answer box. NAOH: NazCO3: NaHCO3: 96Why is it necessary to carry out the reduction of iron and then the titration, before goin on to the next sample? Procedure Weigh four (4) 0.3 g sample of the dried unknown into four 400 or 600 mL beakers. Add 50 mL of 6 M HCI to each sample beaker and heat in the fume hood until the solutions boil for 30 seconds or until the sample dissolves Obtain approximately 20 mL of stannous chloride solution (SnCl2) from the reagent hood Add SnCl2 to the hot unknown solution drop-wise with a disposable plastic pipet until the solution changes from yellow to light green Add three drops of SnCl2 solution in excess Remove the sample from the fume hood and cool the solution to room temperature (a room temperature tap water bath is OK but no ice) After cooling, rapidly add 10 mL of the saturated HgClh solution (obtained from the reagent hood). Allow the sample solution to stand for 3 minutes – a precipitate should form To the sample solution add 60 mL of 3 M H2SO4, 15 mL of 85% H3PO4 and 100 mL…Precipitimetry The chloride in a 4.321-g food sample was precipitated through the addition of 50.00 mL of a standard AgNO3 solution (10.00 mL AgNO3 = 11.22 mL KSCN). The precipitate was coated with nitrobenzene and the mixture was diluted to 250.0 mL. A 50.00 mL aliquot was taken from the diluted solution and required 4.56 mL back titration with a %3D standard KSCN solution (22.33 mL KSCN = 0.9758 g AgNO3). %3D Formula Masses: AgNO3 = 169.87; CI = 35.45 Calculate the following: 1. Molar concentration of KSCN solution M %3D 2. Molar concentration of AgNO3 solution M %3D 3. % (w/w) chloride in the original sample =
- One of the CHEM3341 student Ms. Fatima Al Wahaibi wanted to analyse phosphate ion concentration in Fertilizer industry wastewater sample collected from Rusayl Industrial Estate using spectrophotometer method. She mixed 200.00 mL of wastewater sample which contains only Na;PO, (unknown molarity) with 400.00 mL of 0.0200 M K,PO4 in a one liter beaker to make a Solution A. She then transferred 25.00 mL of Solution A to a 250.00 mL volumetric flask and added distilled water up to the calibration mark to make up Solution B. The Concentration of phosphate ions in Solution B is known to contain 3.00 x 103 mol/L from the spectrophotometric analysis at 460 nm using 1 cm cuvette. Calculate the concentration of phosphate ion in wastewater and how many phosphate ions are present in this wastewater.5. A 300.0 mg sample containing Na,CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.2) Move the 25.000 mL of 0.500 M KHP solution from the Stockroom to the Workbench area. 3) Add 0.2 mL of phenolphathalein indicator to the KHP solution. 4) Titrate the KHP solution with an approximately 1 M NaOH solution. 5) Volume (L) of NaOH used in titration 6) Moles of KHP used for titration (Eq. 3): 7) Moles of NaOH required for titration (= #6) 8) Molarity of the NaOH solution, Eq. 4. (show your calculation)