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- You were assigned to assay a product sample of milk of magnesia. A 0.600-g sample was reacted with 25.00 mL 0.10590 N H2SO4 . The excess unreacted acid in the solution required 13.00 mL of 0.09500 N NaOH when titrated to reach the methyl red end point. Determine the dosage strength of the product in terms of % Mg(OH)2 content. Type your answer in 2 decimal places, numbers only.A copper(II) sulfate solution of unknown concentration is placed in a colorimeter and an absorbance reading of 0.46 is recorded. Using the same solution cell, a 0.055 Μ solution of copper(II) sulfate gives an absorbance reading of 0.34. What is the concentration of the first solution?Which among these is the most important piece of data in a gravimetric analysis? Mass of analyte Mass of weighing form Mass of crucible Mass of precipitating agent
- Treatment of ammonia with phenol in the presence of hypochlorite yields indophenol, a blue product that absrobs light at 625 nm, which çan be used for the spectrophotometric determination of ammonia. gan OCF OH + NH3 indophenol anion To determinè the ammonia concentration in a sample of lake water, three samples are prepared. In sample A, 10.0 mL of lake water is mixed with 5 mL of phenol solution and 2 mL of sodium hypochlorite solution, and diluted to 25.0 mL in a volumetric flask. In sample B, 10.0 mL of lake water is mixed with 5 mL of phenol solution, 2 mL of sodium hypochlorite solution, and 2.50 mL of a 5.50 x 10-4 M ammonia solution, and diluted to 25.0 mL. Sample C is a reagent blank. It contains 10.0 mL of distilled water, 5 mL of phenol solution, and 2 mL of sodium hypochlorite solution, diluted to 25.0 mL. The absorbance of the three samples is then measured at 625 nm in a 1.00 cm cuvette. The results are shown in the table. Sample Absorbance (625 nm) A 0.361 B 0.608 C…this type of analysis refers to the determination of the identity of the analyte in the sampleIn the determination of iron in fortified cereals by atomic absorption, 0.9133 g of sample was weighed. After a previous treatment, it was dissolved and diluted to 100 mL, an aliquot of 25.0 mL was taken, this was diluted to 100 mL and this solution presented an absorbance reading of 0.251. A series of iron standards of the following concentrations were prepared: 0.0; 1.0; 2.0; 2.5 and 3.0 ppm. Whose absorbances were 0.0; 0.241; 0.405; 0.520 and 0.640. Determine the iron concentration in mg/100 g of sample.
- Gold can be determined in solutions containing high concentrations of diverse ions by ICP-AES. Aliquots of 50.0 mL of the sample solution were transferred to each of four 100.0 mL volumetric flasks. A solution was prepared containing 10.0 mg/L Au in 20% H2SO4 and quantities of this solution were added to the sample solutions to give 0, 2.5, 5, and 10 mg/L added Au in each of the flasks. The solutions were made up to a total volume of 100.0 mL, mixed, and analysed by ICP-AES. The resulting data are presented in the following table. Added Au, mg/L Emission Intensity Count 12,568 19,324 26,622 40,021 0.0 2.5 5.0 10.0 Calculate the concentration of gold in the original sample.Nitrite ion, NO2-, is a preservative for bacon and other foods, but it is potentially carcinogenic. A spectrophotometric determination of NO2- makes use of the following reactions: A 5.00 cm cell was used to measure absorbance. Here is an abbreviated procedure for the determination. 1. To 50.0 mL of unknown solution containing nitrite is added 1.00 mL of sulfanilic acid solution. 2. After 10 min, 2.00 mL of 1-aminonapthalene solution and 1.00 mL of buffer are added. 3. After 15 min, the absorbance is read at 520 nm in a 5.00-cm cell. The following solutions were annaylzed: A. 50.0 mL of food extract known to contain no nitrite(that is a neglible amount); final absorbance =0.153 B. 50.0 mL of food extract suspected of containg nitrite ; final absorbance= 0.622 C. Same as B, but with 10 microliters of 7.50x10^-3 M NaNO2 added to the 50.0 mL sample; final absorbance= 0.967 a) Calculate the molar absorptivity of the colored product. Remember that a 5.00 cm cell was used b) How many…3 The gravimetric analysis of nickel in copper and iron, what is the purpose of "dipping" the precipitation in this experiment
- A 0.2985 g sample of an antibiotic powder was dissolved in HCl and the solution diluted to 100.0 mL. A 20.00 ml aliquot was transferred to a flask and followed by 25.00 ml of 0.01886 M KBRO3. An excess of KBr was added to form Br2, and the flask was stoppered. After 10 min, during which time the Br2 brominated the sulfanilamide, an excess of KI was added. The liberated iodine titrated with 12.88 ml of 0.1235 M sodium thiosulfate. Calculate the percent sulfanilamide (NH2C,H4SO2NH2) in the powder. Bro, + 5Br + 6H* 3Br, + 3H,0 NH2 NH2 Br. Br + 2B12 + 2H++ 2Br SO,NH2 SO,NH2 sulfanilamide Br, + 51 2Br + 12 excess 2 + 25,0,- 25,0,2 + 21- - MM: NH2C6H4SO2NH2 = 172.21 KBRO3 = 167.00 KBr 119.00The Kjeldahl method was used to analyse the nitrogen content in 0.6723 g of food sample. The amount of liberated NH3 in the sample was reacted with 50.0 mL of 0.1050 M HCl. The excess acid required 12.35 mL back titration with 0.0915 M NaOH. Calculate the % nitrogen in the sample.Why is blank titration necessary in the iodine value determination?