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- Each equilibria has several disturbances. Each one needs to be addressed separately. For each disturbance to the equilibrium reaction, state how the disturbance affected the equilibrium (shifting it left or shifting it right). Explain specifically what occurred and how it pairs with the observation. Pour about 1 milliliter of deionized water to each of three test tubes. Add 1 drop of 0.1 M Fe(NO3)3 and 1 drop of 0.1 M KSCN to each test tube. Add two more drops of 0.1 M Fe(NO3)3 to one of the tubes, and two more drops of 0.1 M KSCN to another of the test tubes. Try to compare the colors of the solutions as quantitatively as possible. Record your observations and explain what happened using Le Châtelier's principle. Part 5: Iron/Thiocyanate Equilibrium Fe,* {pale yellow} + SCNFe(SCN)2²*{deep red) Add 1 drop of 0.1 M Fe(NO₂), to each test tube Add 1 drop of 0.1 M KSCN to each test tube. Add two more drops of 0.1 M Fe(NO3)3 to one of the tubes. Add two more drops of 0.1 M KSCN to the other…In following these steps . Complete the table and provide th given chemical reactions in the qualitative analaysis of Group 3 Cations. Procedure 1. Place 20 drops of each of the following aqueous solutions to separate centrifuge tubes: 0.1M Cr (NO3)3, 0.1M Al (NO3)3, 0.1M Co (NO3)2, 0.1M Zn (NO3)2, 0.1M Mn (OH)2, 0.1M Ni (NO3)2, 0.1 M Fe (NO3)3. Make each solution basic by adding few drops of 6M NH4OH. Confirm using a litmus paper. 2. Add 5 drops of freshly prepared 6M (NH4)2S to each centrifuge tube. Place the samples in thecentrifuge machine for 3 mins. After centrifuge record results. Decant the supernatant liquid of all the samples. 3. Add one drop of NH4OH in each centrifuge tubes. Add 20 drops of distilled water in eachcentrifuge tubes. Then add a few drops of 6M HCl in each solution. Place the samples in the water bath for 10 mins. After water bath, centrifuge the samples for 3 mins. 4. After centrifuge, add a few drops of 6M NH4Cl in each sample. Decant the supernatant liquid…In a reaction involving the iodination of acetone, the following reaction mixture was used: 5.00mL 4.0M acetone, 5.00mL 1.0 M HCl, 5.00mL 0.0050 M I2, and 10.0 mL water. what was the molarity of the acetone in the reaction mixture? (Recall that M1V1=M2V2) the color of the above reaction mixture disappeared in 250 seconds. What was the rate of the reaction?
- Assay of sodium nitrite is an example of assay under? Cerimetry Iodometry Permanganometry Iodimetry BrominimetryWhich of the two salts is hydrolyzed to a greater extent under equal conditions(KCN or KClO), why? Confirm your answer by calculating the hydrolysis constant. Write ionic-molecular and molecular hydrolysis equation. What pH of the medium will be observed during the hydrolysis of this saltas (acidic or alkaline) Are solutions of these compounds dangerous to humans? Why?Consider the following scenerio in answering Questions 2 through 4: An equilibrium mixture of the reaction observed in Experiment 3 is set up by mixing 5.0 mL of 0.0020 M Fe3*(aq), 2.0 mL of 0.0020 M SCN- (aq), and 3.0 mL of deionized H20. The absorbance of the equilibrium mixture was measured to be 0.185. What is the initial concentration of SCN ([SCN]o) for this mixture? This is the concentration that would be listed in the "initial" row of an ICE table.
- Why do you add NaHCO3 to the sample solutions in the determination of chloride by the Mohr Method (Analytical Chemistry)AgOH(s) + H3O*(ag) + Cl-(aq) 2 AgCl(s) + 2H2O (R11) Write out the reactions that would occur if nitric acid was used instead of hydrochloric acid.A kinetic isotope effect (ku/Kp) of~1.05 has been estimated for the following reaction. Please provide a reasonable explanation for the origin of this kinetic isotope effect. F3C. Br F3C. F•BF3 Br Br 50 °C H/D H/D.
- System 3: NaHSO3 and KMnO4 Do three variations: [3A], [3B] & [3C] [3A] Acidic solution In large test tube, 0.1 M NaHSO3 (2 mL) + 3 drops of 0.5 M H₂SO4; then add 10 drops of 0.1 M KMnO4, drop by drop. The sign of reaction will be the loss of the permanganate color. [3B] Slightly basic solution 0.1 M NaHSO3 (2 mL) + 2 drops 1 M NaOH; then add 0.1 M KMnO4 dropwise (about 10 drops). [3C] Strongly basic solution 0.1 M NaHSO3 (2 mL) + 1 mL 6 M NaOH; then add 0.1 M KMnO4 dropwise (about 10 drops). Note two reactions: the first, a color change, is unique to system [3C]; the second, a precipitate, is like that of [3B]. Please write balane redox reaction, hint HSO3- > HSO4-, H2SO4+MnO4-->MnSO4Write the products structures and mechanisms CO2H A = N. H (cat.) HO (a) ? NC. CN OMe solvent Ph (i) (ii)How to solve for the reaction rate order and rate constant of the dissolution of CuO given only the pH per time below? Time (min) pH 0 0 3 0.05 6 0.12 9 0.23 12 0.34 15 0.45
