The goal of the experiment is to synthesize a bromohexane compound from 1-hexene and HBr(aq) under reflux conditions and use the silver nitrate and sodium iodide tests to determine if the product is a primary or secondary hydrocarbon. The heterogeneous reaction mixture contains 1-hexene, 48% HBr(aq), and tetrabutylammonium bromide and was heated to under reflux conditions. Heating under reflux means that the reaction mixture is heated at its boiling point so that the reaction can proceed at a faster rate. The attached reflux condenser allows volatile substances to return to the reaction flask so that no material is lost. Since alkenes are immiscible with concentrated HBr, tetrabutylammonium bromide is used as a phase-transfer catalyst.
Sodium Bicarbonate mixed with Hydrochloric acid. The chemical reaction observed showed that there was fizzing and bubbling, this is evidence that a new gas was being produced. This new gas, CO2 was generated from the reaction. After the fizzing stopped a liquid was leftover leading me to conclude the liquid leftover leading me to conclude the liquid leftover was the NaCl and H2O 4. You found a sample of a solution that has a faint odor resembling vinegar (an acid).
Experiment 1 In this experiment we added different Alkali metals to water and noted the observations with Universal Indicator. PROCEDURE 1. First we took some amount of water in a beaker and added 2-3 drops of Universal Indicator 2. Then we cut the Sodium metal into small pieces 3. Then we added the cut pieces to water in the beaker and noted the change observed.
Bubbles are produced continuously from the time the tablet enters the water until the time when the reaction between sodium bicarbonate and citric acid ceases. The disappearance of bubbles can be used as a qualitative indicator for the completion of the chemical reaction and the production of the sodium citrate solution. The chemicals in the final solution are sodium bicarbonate, and citric acid, to make a sodium citrate solution. The solute is the Alka-Seltzer tablet and the solvent is the
The original reaction done by Kolbe involved the formation of sodium phenoxide through the evaporation of a molar equivalent mixture of phenol and aqueous sodium hydroxide. The hygroscopic sodium phenoxide is then heated while carbon dioxide gas is passed over the molten salt. The mixture is then further heated to give the dianion of salicylic acid along with carbon dioxide and phenol both of which distill away from the mixture. Under these
Due to the hydroxide ions, both solutions turn pink and become effervescing with hydrogen gas. Below are the equations of the reactions : Mg(s) + 2H2O(aq) → Mg(OH)2(aq) + H2(aq) Ca(s) + 2H2O(aq) → Ca(OH)2(aq) + H2(aq) Calcium is more reactive than Magnesium. Therefore, Ca(OH)2 changes to pink faster than Mg(OH)2 because Calcium is located below Magnesium in the periodic table. Calcium donates electrons faster than Magnesium. Part 2 .
Aluminum (s) + Sulfuric acid (aq) > Hydrogen (g) + Aluminum sulfate (aq) 2 Al (s) + 3 H2SO4 (aq) > 3 H2 (g) + Al2(SO4)3 (aq) This reaction undergoes physical and chemical changes, there is a chemical change as there are new products formed and a physical change as there are changes in state. 3. The reaction between silver nitrate and sodium chloride to form sodium nitrate and silver chloride. AgNO3 (aq) + NaCl (aq) → NaNO3 (aq) + AgCl (s) This reaction undergoes physical changes as there is a change in state and also there is a change in colour, after the reaction occurs, a white precipitate is formed. The reaction also undergoes a chemical change as 2 new products are formed.
Alyah al Mutairi Mr. Washington Biology class H 14.12.15 Deciding the behavior of amylase under the implement of excess pH levels Problem: To verify if amylase maintains to operate with the influence of hydrochloric acid Prelab: Independent variable: pH levels Dependent variable: The effect of pH enzyme action Control: Positive: Saliva and HCL+ saliva Negative: Water Constant: Iodine solution (indicator) Hypothesis: At least two out of the three procedures will be indicated as starch, due to the fact that amylase is the first enzyme that breaks down carbohydrates Materials: • Paper • Pen/pencil • Saliva • Water • Hydrochloric acid • Pipette • Iodine solution • Construction paper • Timer Procedure: 1. A sheet of paper was
I can now calculate the density (aka the concentration), of them before and after. Then I can take the change in density over the change in time to determine the rate of chemical reaction. This is because a chemical reaction will affect a solution’s concentration, and to determine the rate, I just need to factor time into the scenario. Furthermore, I can do this multiple times, all with different concentrations of HCl and different amounts of calcium carbonate (as it is diluted in water, and water has a different mass than the acid), to determine how the original concentration of HCl affects the rate. Hypothesis: My hypothesis is that the rate can be measured as ∆ρ/∆t=rate of reaction Additionally, I hypothesize that I can use variations of the original concentration of the solution of HCl with water to figure out how the original concentration changes rate of reaction.
In direct titrations, the number of moles of acid can be easily derived by simply manipulating with the values of acid and base given in the experiment. In back titration, excessive volumes of acid are always added. Of which, only a certain quantity would be neutralised. The number of moles of acid is eventually derived from titrating this excess acid with a strong base and using mole fractions to calculate. The quantity of acid neutralised is obtained by subtracting the moles of acid given at the start of the experiment, with the moles of acid titrated.