Fill the burette with 0.005mol dm-3 potassium manganate(VII) solution. 6. Pour some of the thyme extract solution into a 250cm3 plastic beaker. 7. Using a measuring cylinder, add 50cm3 of 1.0mol dm-3 sulphuric(VI) acid to the thyme extract in the conical flask.
LAB 1 NAME: Amy Rampersad. DATE: Saturday 7th April, 2012. TITLE: PREPARATION OF A SOLUBLE SALT BY A TITRATION METHOD. AIM: To prepare Sodium Chloride crystals by Titration of Sodium Hydroxide with Hydrochloric Acid. APPARATUS: Burette (50 cmᶾ), Pipette (25 cmᶾ), two conical flasks (250 cmᶾ), two beakers (250 cmᶾ), funnel, wash bottle, retort stand, boss and clamp, evaporating dish, pipette filler, hot-plate.
To do this, first take the number of drops used to achieve the monolayer (1 drop) and convert it to mL using the calibrated number of drops per mL. Then multiply the number of grams of sodium stearate per milliliter of solution. Finally, convert to moles through the molar mass of sodium stearate. HINT: The molar mass of sodium stearate is 296.5 g/mole. Answer = 1.06*10^7 moles/top layer 5.
Stoichiometry of a Precipitation Reaction October 1, 2013 Chem 131A-011 Partner: Purpose: This lab exercise combines the study of a precipitation reaction with stoichiometry. The amount of product produced in the precipitation reaction will be predicted to determine the theoretical yield. The reactants and products will be measured to determine the actual yield and the percent yield. Procedure: * 1.0 g of CaCl2·2H2O was put in a 100-mL beaker. * 25 mL of distilled water was stirred in to form the calcium chloride solution.
The synthesis of NaCl further identified the ionic compound by reacting sodium hydroxide and hydrochloric acid and obtaining solid sodium chloride. The synthesized compound formed was used to perform another flame test and the chloride anion test, which further solidified the identification of NaCl as the ionic compound. Introduction The purpose of the experiment was to identify unknown ionic compound
Lab 2, Week 2 BOND LAB Introduction The purpose of this lab is to find and learn the properties of ionic and covalent bonds, also to learn the physical properties of each substance; such as melting point, solubility and conductivity, type of bond in the compound. Also in this experiment, tests on these properties will be performed enabling the classification of compound bonds as ionic or covalent. Procedure Part A - Melting Point 1. Obtain six watch glasses. Place a two-gram sample of the following compounds in a separate watch glass: * Watch Glass #1: 2g of Calcium Chloride * Watch Glass #2: 2g of Citric Acid * Watch Glass #3: 2g of Phenyl Salicylate * Watch Glass #4: 2g of Potassium Iodide * Watch Glass #5: 2g of Sodium Chloride * Watch Glass #6: 2g of Sucrose 1.
For the third part of the experiment, the process of part 1 was repeated using sodium hydroxide. 5 drops of 0.10 M sodium hydroxide were placed in wells 1 and 2, and 5 drops of distilled water were placed in wells 2 through 6. A toothpick was used to stir the mixture in well 2, resulting in 0.05 M of sodium hydroxide. A pipet was used to extract the solution from well 2 and 5 drops were added to well 2. The dilution process was repeated for the remaining wells, as completed in part 1.
Let’s experiment and observe Whether these ions will have a reaction or indeed soluble in water. Experimental Procedure Let’s begin this experiment by obtaining a 100ml beaker from our equipment tool bar list, then we are going to add 50ml(s) of Potassium Chromate 1M solution to that beaker, The next step we are going to add another ionic compound of 50ml of Lead (11) nitrate 1M into the same beaker as the Potassium Chromate. As we observe the beaker, we notice a reaction has occurred and a precipitate has formed and settled on the bottom of the beaker. The next step is we are going to filter the resulting precipitate into a 250 ml Erlenmeyer Flask with a Buchner funnel. Now that we have filtered the precipitate, we will then place the resulting precipitate into a test tube to measure the weight.
For reaction (II) Pb (NO3)2 + 2KI -> PbI2+2KNO3 Lead nitrate is soluble, so it gets written as ions. The same goes for potassium iodide and potassium nitrate. Complete Ionic equation: 2 K+1 + I-1 + Pb2+ + NO32- -> PbI2 + 2K+1 + NO3-1 Net Ionic Equation: Pb+2 + 2 I-1 -> PbI2 Warm-Up Exercise 2 In this lab you will mix 25 mL of 0.05M lead nitrate with 1.4 mL of 0.025M sodium carbonate. After the reaction occurs, you will filter the solution to remove the precipitate. You will then test the remaining solution for excess lead ion and for excess carbonate ion… Imagine that you mix the two volumes and then freeze frame the reaction so the it does not proceed: 1.
C. The final pH is 7. D. Water is produced. 2. Which salt could be prepared by a method involving crystallization as a final stage? A. barium sulphate B. calcium carbonate C. silver chloride D. sodium nitrate 3.