After reacting two liquid reactants with eachother and allowing them to reflux for 2 hours. There was very poor percentage yield of product. Why?
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After reacting two liquid reactants with eachother and allowing them to reflux for 2 hours. There was very poor percentage yield of product. Why?
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- A K2SO4 solution is prepared by weighing out a certain amount of the pure solid reagent,dissolving it to 500.0 mL in a volumetric flask. An aliquot was taken from this solution.of 25.00 ml and diluted to 500.0 ml. An aliquot of 5.00 was taken from this new solution anddiluted to 50.00 ml. A chemical analysis of this new solution showed a 0.100%(w/v)in K+. Calculate the weight of the pure solid K2SO4 used for the preparation of the original solution.and its concentration in each volumetric flask. The answer is 2.23x10^2gPlease help me in these 4 questions. Thank you!Ans. Number 2
- 1.063 g of p-acetamidophenol was measured out into a 50 mL round bottom flask along with 8 mL of 1M NaOH in ethanol and a stir bar. This mixture was heated at reflux for 15 min. It was allowed to cool and then 0.80 mL of bromoethane was added to the reaction. The mixture was then heated at reflux for another 15 min. After heating, the solution was poured onto a mixture of ice and water and further cooled on ice and then the solid was collected by vacuum filtration. This solid was then recrystallized from ethanol and water. The final mass of the purified phenacetin was 0.42250 g and it had a melting point of 127 - 130 C. The TLC plate shows (from left to right) pure p-acetamidophenol, the reaction mixture before pouring it on ice/water, phenacetin after recrystallization. The solvent used was a mixture of 80% ethyl acetate and 20% heptane with 0.5% acetic acid added. QUESTION: Using the given TLC plate can you describe the results and what does the TCL plate tell about the purity?Write the balanced NET ionic equation for the reaction when aqueous SrBr₂ and aqueous K₂SO₄ are mixed in solution to form solid SrSO₄ and aqueous KBr. Be sure to include the proper phases for all species within the reaction.but my prof said the answer is H2SO4,NaCN and H2O for solvent. why did he answer like above? and please tell me how did u find KCN and HCN what makes you answer like that Should i have to memorize some solvent or reagent? then let me kno that list
- Please send me the question in 30 minutes it's very urgent plzProvide the balanced reaction for this experiment? a piece of weigh paper (or weigh boat) and tare it out on the balance. Weigh out between 1.000 to 1.200 g of KHP. Record the exact mass in your data table for Trial 1. Pour your KHP sample in flask #1. (4) Repeat step 3 two more times for flasks #2 a nd #3. (5) To each flask, add approximately 30 mL of distilled water. Warm the flasks slightly and swirl them until all the KHP is dissolved. (6) Obtain about 250 mL of NaOH in a clean, dry 250 mL Erlenmeyer flask. Stopper the flask until you are rea dy for the solution in step 6d. (7) Obtain one buret and clean it. (a) First, rinse the buret a couple of times with tap water, pouring the water from a beaker. (b) Then, scrub the buret with a detergent solution, using a long - handled buret brush. (c) Next, rinse out the detergent with tap water several times and finally with distilled water. Be sure to also drain through the tip. (d) After draining the distilled water, rinse the buret…The concentration of ammonia in a cleaning product was determined by back titration.Firstly, 10.00 cm3 of the cleaning product was pipetted into a large conical flask,containing 250.00cm3 of 0.50 mol/l HCl to give Solution A.Following a period of reaction and shaking, 50.00cm3 of Solution A was removed anddiluted to 250 cm3 with water in a volumetric flask to give Solution B.20 cm3 samples of Solution B were titrated against 0.05 mol/l Na2CO3 solution, givingan average titre of 12.45 cm3. i) Write equations for the reactions that have taken place.ii) Determine the concentration of NH3 in the original cleaning product in mol/l,g/l, ppm, and % w/v.
- 02:21 4G File Details 4CH003/UM1: Fundamentals of... Introduction Perhaps the cleanest method of conducting an oxidation is by catalytic oxidation, since this minimizes the problem of removal of unwanted by- products. However, the conditions used are often vigorous and require the use of specialized equipment. By comparison, the product of a "chemical" oxidation may be more difficult to purify due to the presence of the reduced form of the oxidizing agent and potential "tars" that may arise from "over- oxidation". Because chemical oxidation can be carried out using conventional equipment they are more popular. dissolving sodium or potassium dichromate in acid is a commonly used oxidizing agent, being classed as a relatively powerful oxidant and having water soluble by-products (Cr III salts). Sulphuric acid is generally used if the material to be oxidized is water soluble and glacial acetic acid is used if it is Chromic acid, prepared in-situ by not. Alcohols are readily oxidized to…xpress numerical result with an accuracy of: Х,Х 1. The substance to be analyzed – is deep-pink colored, highly soluble in water salt. Reaction with NH3 gives blue-colored precipitate, which can be dissolved in NH3 surplus accompanied by dirty-yellow colored solution formation. After precipitation of cation by “sodium carbonate drawing out” method, supernatant was independently treated by silver nitrate solution and barium chloride solution (in acid medium in both cases) – any precipitation hasn`t been observed. Addition of antipyrin in acid medium changes color to red. What kind of substance is this? Explain you answer, provide chemical equationsYield