The method of standard additions was used to determine nitrite in a soil sample. A 1.00-mL portion of the sample was mixed with 22.00 mL of a colorimetric reagent, and the nitrite was converted to a colored product that produced a blank-corrected absorbance of 0.350. To 54.00 mL of the original sample, 1.00 mL of a standard solution of 1.00 × 10-³ M nitrite was added. The same color-forming procedure was followed, and the new absorbance was 0.560. What was the concentration of nitrite in the original undiluted sample? -3 Concentration = M
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- A 1.6 g sample of a compound is transfered to a 100 mL volumetric flask, filled to the mark with distilled water, and thoroughly mixed. Twenty five milliters of this solution is drawn from the flask using a volumetric pipet, transfered to another 100 mL volumetric flask, and filled to the mark and mixed. The grams of compound in the second volumetric flask is: A. 1.6 B. 1.2 C. 0.80 D. 0.40Come up with a dilution scheme for a test solution starting from 1000 μg/mL Mn stock solution so that the concentration of permanganate in the solution just prior to measurement is approx. 20 μg/mL MnO4-. Carefully read the units!For the analysis of unknown soda and vinegar samples, 25.0 mL soda and 1.0 mL vinegar samples were diluted to 50.0 mL in separate Erlenmeyer flasks. KHP, 0.85 g, (Purity = 99.98%; Molar mass = 204.22 g/mol) was titrated with 11.5 mL of NaOH. After the standardization step, it required 0.0143 L of NaOH to reach the endpoint with the soda sample while it took 0.00885 L with the vinegar sample. Phenolphthalein was used as the indicator for the experiment. Express all final answers in 2 significant figures. a. Determine the concentration of the titrant (NaOH) b. Determine the concentration of the unknown vinegar sample. c. Determine the concentration of the unknown soda sample.
- If the mass of the original sample of alloy was 0.7459 ± 0.0005 g and the mass of precipitated CuSCN was 0.2275 ± 0.0005 g and the volumetric flasks used had a 0.05% error, what is the error in the calculated percentage mass of Cu in the alloy? Assume no error in the molecular masses. Provide your answer as an absolute error.Tartaric acid, H2C4H4O6, is a diprotic acid that naturally occurs in the production of apple wine. Emma was tasked to find out the acid content in a 50.0 mL wine sample by titrating it with a standardized solution of NaOH. She was able to establish the working concentration of the NaOH solution by using 17.61 mL of NaOH to titrate a primary standard of KHP that weighed 1.501 g. The grams and %w/w of Tartaric acid present in the 50.0 mL wine sample were then determined by titrating a 12.50 mL aliquot using 21.78 mL of the standardized NaOH solution. H2C4H4O6 (aq) + 2NaOH (aq) ↔ Na2C4H4O6 (aq) + 2H2O (l) Assume that the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of H2C4H4O6 = 150.087 g/mol What is the molar concentration of the prepared NaOH solution?…Solutions of cyanide salts are still widely used in the extraction of gold metal from its ores. It is thereforenecessary to regularly monitor the quality of the reagents used to make such solutions.The purity of a sample of solid potassium cyanide is determined as follows: 5.00 g of the impure potassium cyanide is weighed off, and quantitatively transferred into a100.00 mL volumetric flask, dissolved and made up to the mark. A 10.00 mL portion of this solution is pipetted into a conical flask, and titrated with a 0.200 MKMnO4 solution. The endpoint of the titration is determined when the colourless solution in the conical flask turns abright pink due to the presence of excess permanganate ions. The average titration value is 20.69 mL of the KMnO4 solution.The reaction stoichiometry is as follows: 2KMno4(aq) + 3KCN(aq) + H2O(l) → 2MnO2(s) +3KOCN(aq) + 2KOH(aq) 1.1 Determine the percentage purity of the potassium cyanide.
- In one trial of the standardization of a Na2S2O3 solution, a 10.00 mL volume of 5.00×10-3 M KIO3 is pipetted into a 250 mL Erlenmeyer flask. The solution is titrated to the endpoint with 15.96 mL of the Na2S2O3 solution. What is the molar concentration of this sodium thiosulfate solution?The active ingredient in a zinc nutritional supplement is ZnSO4⋅7H2OZnSO4⋅7H2O (molar mass = 287.58 g/mol). Ten zinc tablets containing a mix of the active ingredient and an inactive filler were ground and mixed together thoroughly. The total mass of these 10 tablets was 11.82511.825 g. A 2.2062.206 g sample of the finely ground tablets was dissolved in an acidic solution. The solution was neutralized with ammonia and subsequently warmed in a water bath. Addition of (NH4)3PO4(NH4)3PO4 to the solution resulted in the precipitation of ZnNH4PO4ZnNH4PO4. The precipitate was filtered and dried, then ignited to produce 0.2440.244 g of Zn2P2O7Zn2P2O7 (molar mass = 304.76 g/mol). What is the mass percent of ZnSO4⋅7H2OZnSO4⋅7H2O in each tablet?The aluminum in a 2.200-g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al2O3⋅xH2O. The precipitate was filtered and ignited at 1000°C to give anhydrous Al2O3, which weighed 0.3006 g. Express the result of this analysis in terms of a. %NH4Al(SO4)2 b. %Al2O3 c. %Al
- An aqueous solution of sodium chloride,NaCl , is made by dissolving 1.01 grams of sodium chloride in sufficient water in a 50.0 mL volumetric flask, and then adding enough water to fill the flask to the mark. What is the weight/volume percentage of sodium chloride in the solution? Weight/volume percentage = %You are required to standardize a dilute solution of sulphuric acid, and undertake the following steps:(i) 4.805 g of solid sodium tetraborate (Na2B4O7) are added to a 250 mL volumetric flask, and the solution made up to the mark with distilled water.(ii) 25.00 mL aliquots of the stock solution from (i) are transferred to conical flasks, for titration against the sulphuric acid solution in the burette.(iii) You perform titrations using two different indicators: bromocresol green, and phenolphthalein.With bromocresol green, the average titre volume is 22.50 cm3, while with phenolphthalein, the average volume is 9.50 cm3.(a) Write the balanced equation for the reaction between Na2B4O7 and sulphuric acidTartaric acid, H2C4H4O6, is a diprotic acid that naturally occurs in the production of wine. Jose was tasked to find out the acid content in a 100.0 mL wine sample by titrating it with a standardized solution of NaOH. He was able to establish the working concentration of the NaOH solution by using 35.21 mL of it to titrate a primary standard of KHP that weighed 3.001 g. The grams and %w/w of Tartaric acid present in the 100.0 mL wine sample were then determined by titrating a 25.00 mL aliquot using 43.56 mL of the standardized NaOH solution. H2C4H4O6 (aq) + 2NaOH (aq) ↔ Na2C4H4O6 (aq) + 2H2O (l) Assume that the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of H2C4H4O6 = 150.087 g/mol What is the molar concentration of the prepared NaOH solution?…