If the legal minimum acetic acid content in vinegar is 1.50M, which of the two vinegar enthusiasts- Rei, Akari, or BOTH, are allowed to sell their vinegars for business?
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- Suggest a strategy using selective precipitation (which salts containing precipitating ion would you add and in what order) to purify wastewater contaminated with Ag+, Ba2+, Fe3+ and Na+. The purified water should only contain Na+ which is safe to drink.If Sn3(PO4)2 solution is to be subjected to argentometric titration, a) Write the balanced titration reaction. (products are Ag3PO4(s),, other ions are spectator ions b) Write the stoichiometric relationship (fundamental eqn) between the titrant (AgNO3) and the titrand (Sn3(PO4)2. c) Is this a feasible titration technique? Why?Please answer the following question: Suggest a strategy using selective precipitation (which salts containing precipitating ion would you add and in what order) to purify wastewater contaminated with Ag+, Ba2+, Fe3+ and Na+. The purified water should only contain Na+ which is safe to drink.
- 16.The titration of an aliquot of 6 mL of acetic acid of commercial use, with NaOH 0.1 , was made by titration, so that to reach the equivalence point 40 ml of NaOH were consumed.Determine the percentage concentration (m/m) of the acetic acid, if its density is 1.05 g/ml. HC2H3O2 acetic acidBalance in acid medium: iodate ion + sulfite ion : then {HNO3} : iodine + sulfate ion 10 ml of 6N HNO3 are mixed with 15 ml of 10N sodium sulfite. How many milliliters of 1.4 M sodium iodate are needed for the reaction to take place?A vinegar solution was prepared by diluting 25.00 mL of vinegar to 250.0 mL. From this solution, 50.00 mL portion was taken, and this required 30.00 mL of 0.1000M NaOH solution to reach neutralization end point. What is the percentage (w/v) of HOAc in the sample? Mol wt HOAc = 60.0 g/mol
- To determine the concentration of glucose in the packaged juice industry, 50 mL of sample is analyzed. Analysis of it (and other reducing sugars) was carried out there using triiodide back titration. An excess volume of 75.00 mL of 0.338 M triiodide standard solution in alkaline medium was added to the glucose solution. The resulting solution was acidified and the excess triiodide was titrated with 18.37 mL of standard 0.526 M thiosulfate solution. Calculate is the concentration in ppm in the sample. In alkaline medium: Glucose (C6H12O6) / Gluconate (C6H11O7-), Triiodide (I3- ) / Iodide (I-) In acid medium: Thiosulfate (S2O32-) / Tetrathionate (S4O62-), Triiodide (I3- ) / Iodide (I-)A mixture of NaBr, Nal and NaNO3 weighs 0.6500 g. With AgNO3, a precipitate of the two halides is obtained and is found to weigh 0.9390 g. When heated in a current of C2, the precipitate is converted entirely to AgCi weighing 0.6566 g. What is the %NaNO3 in the original sample?A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 303 mg of oxalic acid, a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 104.5 mL of sodium hydroxidesolution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 3 significant digits.
- As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content using gravimetric analysis with sodium tetraphenylborate, Na+B(C6H5)4−. Unfortunately, the amount of potassium, which also precipitates with sodium tetraphenylborate, is non‑negligible and must be accounted for in the analysis. Assume that all potassium in the soil is present as K2CO3 and all ammonium is present as NH4Cl. A 5.095 g soil sample was dissolved to give 0.500 L of solution. A 150.0 mL aliquot was acidified and excess sodium tetraphenylborate was added to precipitate both K+ and NH4+ ions completely. B(C6H5)4-+K+⟶KB(C6H5)4(s) B(C6H5)4-+NH4+⟶NH4B(C6H5)4(s) The resulting precipitate amounted to 0.269 g. A new 300.0 mL aliquot of the original solution was made alkaline and heated to remove all of the NH4+ as NH3. The resulting solution was then acidified, and excess sodium tetraphenylborate was added to give 0.129 g of precipitate. Find the mass percentages of NH4Cl and…The SO2 present in air is mainly responsible for the phenomenon of acid rain. The concentration of SO2 can be determined by titrating against a standard permanganate solution as follows: 5SO2 + 2MnO4- + 2H2O ---> 5SO42- + 2Ms2 + 4H+ Calculate the number of grams of SO2 in a sample of air if 4.90mL of 0.00700M KMnO4 solution are required for the titration. Be sure your answer has the correct number of significant digits.Mg(OH)2 is a sparingly soluble salt with a solubility product, Ksp, of 5.61×10−11. It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams. What is the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2 dissolved in a 0.200 M NaOH solution? Express your answer numerically as the ratio of molar solubility in H2O to the molar solubility in NaOH.