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- Write the balanced NET ionic equation for the reaction when Pb(NO₃)₂ and KI are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.4) A chemist was employed to analyse a particular lawn fertiliser, and dissolved 15.0g of the sample in water. Excess barium chloride was added to precipitate all the sulphate as barium sulphate according to the equation: Ba2+(ap)+SO42-(aq)-> BaSO4(s) When the precipitate was filtered, dried and weighed it had a mass of 4.67g. What was the percentage by mass of sulphate in the lawn fertiliser?3. The concentration of acetylsalicylic acid, C9H8O4, in aspirin tablets is determined by hydrolyzing it to the salicylate ion, C7H5O3-, and de¬termining its concentration spectrofluorometrically. A stock standard solution is prepared by weighing 0.0774 g of salicylic acid, C7H6O3, into a 1-L volumetric flask and diluting to volume. A set of calibration standards is prepared by pipeting 0, 2.00, 4.00, 6.00, 8.00, and 10.00 mL of the stock solution into separate 100-mL volumetric flasks that contain 2.00 mL of 4 M NaOH and diluting to volume. Fluorescence is measured at an emission wavelength of 400 nm using an excitation wavelength of 310 nm with results shown in the following table. (a) Why is the excitation wavelength (310 nm) shorter than the emission wavelength (400 nm)?(b) How is the emission wavelength isolated from the excitation wavelength in a fluorescence instrument?
- First, complete the balancing of the chemical equation below. Second, calculate the volume (in mL) of 0.0250 M KMnO4 solution needed to completely react with 10.0 g of an advertised 3% by mass H2O2 solution (i.e., 3.00 g H2O2/100 g solution) in the presence of excess acid. ?MnO41-(aq) + ?H2O2 (aq) + 6H3O1+(aq)------> 2Mn2+(aq) +5O2 (g) + 14 H2O (l)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 15.23 mL of the Na2S2O3 solution. What is the molar concentration of this sodium thiosulfate solution?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?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. %AlWatch this video of a double displacement experiment: https://www.youtube.com/watch?v=mph8Hq_75vU Write the balanced chemical reactions, including state of the matter What is the precipitate that forms, and which color is it?
- 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 acidFor a precipitation reaction to be useful in a gravimetric analysis, the product of the reaction must be insoluble. Is Kc > 1, < 1, or ≈ 1 for a useful precipitation reaction?Predict the products for the following single-displacement reaction and write a balanced molecular equation. Be sure to include all phase labels. Cu(s) + AgNO3(aq) ——> ?