procedure in Table 4.1. Use the concentration of KSCN, volume of KSCN and total final volume of each solution (each standard solution will be 20.00 mL) to calculate the FeSCN²+ concentration in each of the four standard solutions.
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Molarity of Fe(NO3)3 = 0.200 M
Molarity of KSCN = 0.00200 M
It is desired to calculate concentration of FeSCN2+ in all tubes.
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- On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?Rei and Akari, two vinegar enthusiasts, are each tasked to determine the aceticacid content of their respective vinegar concoctions by titration. First, a 1M-labeled KOH solution was standardized against the KHP (MW = 204.22 g/mol)standard that is 99.4% pure. In the process, 0.540 g KHP was found to require2.80 mL of the KOH solution to completely react up to the phenolphthaleinendpoint. Then, Rei and Akari both prepared their samples by taking 10.0-mLaliquots of each vinegar and diluting them to 25.0 mL. Using the same titrant andindicator, Rei’s vinegar required 18.60 mL of the standardized titrant to reach theendpoint, while Akari’s vinegar required 16.50 mL of the same titrant to reach thesame endpoint. What is the exact concentration of the KOH titrant in molarity? What is the balanced chemical equation between the analyte and the titrant? What is the color transition (color X color Y) expected throughout thecourse of titration? What is the acetic acid concentration of Rei’s and…Mark and John, two vinegar enthusiasts, are each tasked to determine the acetic acid content of their respective vinegar concoctions by titration. First, a 1 M-labeled KOH solution was standardized against the KHP (MW = 204.22 g/mol) standard that is 99.4% pure. In the process, 0.540 g KHP was found to require 2.80 mL of the KOH solution to completely react up to the phenolphthalein endpoint. Then, Mark and John both prepared their samples by taking 10.0-mL aliquots of each vinegar and diluting them to 25.0 mL. Using the same titrant and indicator, Mark’s vinegar required 18.60 mL of the standardized titrant to reach the endpoint, while John’s vinegar required 16.50 mL of the same titrant to reach the same endpoint. Question: What is the acetic acid concentration of Mark’s and John’s vinegar in molarity given that the Concentration of KOH is 9386 M?
- Mark and John, two vinegar enthusiasts, are each tasked to determine the acetic acid content of their respective vinegar concoctions by titration. First, a 1 M-labeled KOH solution was standardized against the KHP (MW = 204.22 g/mol) standard that is 99.4% pure. In the process, 0.540 g KHP was found to require 2.80 mL of the KOH solution to completely react up to the phenolphthalein endpoint. Then, Mark and John both prepared their samples by taking 10.0-mL aliquots of each vinegar and diluting them to 25.0 mL. Using the same titrant and indicator, Mark’s vinegar required 18.60 mL of the standardized titrant to reach the endpoint, while John’s vinegar required 16.50 mL of the same titrant to reach the same endpoint. Question: What is the exact concentration of the KOH titrant in molarity? What is the balanced chemical equation between the analyte and the titrant? What is the color transition (color X ? color Y) expected throughout the course of titration?In the standardization of HCl using pure anhydrous sodium carbonate as the primarystandard for methyl orange as an indicator, 1.0 mL HCl was found to be equivalent to 0.05gof sodium carbonate (MW =106). The normality of HCl is:To determine , by gravimetric analysis, the concentration of barium ions (Ba2+) in a given solution, 25.00cm3 of it are pipetted into a beaker and an excess of dilute sulphuric acid is added to it. The precipitate then obtained (BaSO4) is filtered, dried and weighed. The mass of the precipitate is found to be 1.167g Calculate the concentration of barium ions in the solution? (only 2 decimal places). _________Mol/L
- The concentration of arsenic in an insecticide can be determined gravimetrically through its precipitation as MgNH4AsO4. After the formation of the precipitate, it must be ignited for total conversion to Mg2As2O7, which is then cooled and weighed. Considering that a sample of 1,627 g of the insecticide produced 106.5 mg of Mg2As2O7, determine the% (m/m) As2O3 in the insecticide. Given the molar masses: Mg2As2O7 = 310.447 g / mol and As2O3 = 197.841 g / molThe following analytical procedures were used for the determination of chlorate (ClO3-). 10.00 mL of solutionA containing chlorate is analyzed. The chlorate is reduced with granulated zinc (to chloride).The excess zinc is dissolved in acid, after which the sample is filtered. The filtered sample is added70.00 mL 0.100 M AgNO3 solution dropwise. The precipitate is filtered off, washed and dried.It weighs 0.6003 grams. Calculate the chlorate concentration in solution APlease Complete the balance and label the raction type Complete and Balance Reaction Type Mg + O2 --> Zn + HCl --> H2O2 --> Fe + CuSO4 --> Pb(NO3)2 + H2SO4 --> CaCO3 + HCl --> CuSO4 * 5H2O --> CaO + H2O --> FeSO4 + KMnO4 --> Na2CO3 + HCl -->
- Assume that 1.00 mL (1.02 g) of crude product mixture is obtained from the reactionbefore the washing steps, and the distribution constant of the product mixture in brine isK = (Cmixture/Cbrine) = 50.0. Assuming that after mixing the product mixture volume isstill 1.00 mL (i.e., the volume lost is small), and the volume of the first brine wash layeris 2.00 mL. What mass (grams) of product mixture is lost (dissolves) in the first brinewash? (See Technique 13.2, p 53.) Show work.A solid sample containing chloride ion is analyzed by argentimetric titration to find the percentage chloride by mass. The procedure involves the preparation of a solution made from primary standard sodium chloride (molar mass = 58.443 g mol-1). Aliquots of NaCl solution will be titrated with silver nitrate solution to accurately determine the AgNO3 concentration. The standardized silver nitrate will be used to titrate aliquots of unknown chloride solution, thus allowing for the determination of the percentage chloride in the original solid sample. To detect the endpoint of the titration the adsorption indicator dichlorofluorescein is used. Please solve for the highlighted portions.The tartaric acid, H2C4H4O6 (150.087 g/mol ) concentration in 100.0 mL wine sample was determined using 0.4050 M sodium hydroxide standard solution. In the experiment, the %w/w of tartaric acid present in the wine sample by analyzing and titrating only 25.00 mL aliquot from the 100-ml wine sample. The endpoint of titration was reached upon the addition of exactly 43.56 mL NaOH solution? (Assume the density of the wine sample is 1.000 g/mL) H2C4H4O6 + 2NaOH⟶Na2C4H4O6+2H2O What is the total (%w/w) acid content in the wine sample? 1.324 %w/w 2.648 %w/w 5.296 %w/w 10.59 %w/w