25 ml of diluted unknown acid solution to 100ml beaker by using 25 volumetric pipet. 10ml of deionized water and 3 drops of phenlpthalin indicator the beaker labeled as 3. Potentiometric titration acid solutions 125 ml of NaOH was obtaining in a beaker and 50 ml of NaOH transfer to buret the tip and the meniscus is at below 0 ml. one magnetic stirring bar placed in a beaker contain one of the known solution on a stir. The pH recorded by using pH electrode before adding NaOH.
Add two drops of food coloring to the beaker of distilled water and mix thoroughly. Measure out a dropperful of bleach into a plastic pipet and set it aside until Step 8. 6. Calibrate the colorimeter a. Prepare a blank by filling an empty cuvette ¾ full with distilled water.
Define also the overall order of a reaction and describe how it’s found. Explain how the iodine clock reaction works and the method it employs to find the order of a reaction with respect to a particular reactant. Experimental: Apparatus: 3 -100 cm3 beakers, 1 thermometer, 0-100 0C, 8 burettes with beakers and funnel for filling, clamps and stands, stop clock or watch. Reagents: Potassium peroxodisulphate (VI) solution [0.100 mol dm-3 and 0.050 mol dm-3 K2S2 O8], Potassium iodide solution, [0.500, mol dm-3 and 0.250 moldm-3, KI], Sodium thiosulphate solution, [0.010 mol dm-3 Na2S2O3], Starch solution, 0.2% Procedure: 1. Using a burette, run 5.0 cm3 of 0.100 mol dm-3 peroxodisulphate solution into a 100 cm3 beaker.
Purpose: The purpose of this lab is to verify Hess’s Law of Additivity of Reaction Enthalpies Chemical Reaction/Physical Reaction: 1.) Na(aq) + OH(aq) -> NaOH(s) 2.) NaOH + HC2H3O2(aq) -> H2O(l) + Na(aq) + C2H3O2 3.) Na(aq) + OH(aq) + HC2H3O2(aq) -> H2O(l) + Na(aq) + C2H3O2 List of Materials:Digital Thermometer, foamed polystyrene cups (3), 250 mL beaker,Weighing boat or small beaker, Graduated cylinders, 100mL(1), 25 mL(2),sodium hydroxide pellets, sodium hydroxide 2.0M, Acetic acid 1.0M and 2.0M. Safety Considerations: Always have safety goggles covering your eyes, do not inhale the fumes of chemicals used.
Using a pipet, transfer the methylene chloride solution to a 50 mL Erlenmeyer flask. To this solution, add a scoop of anhydrous sodium sulfate (Na2SO4), in order to remove the last traces of water. 10. While the solution is drying, weigh (tare) a 50 mL beaker to the nearest 0.001 g on a balance. Record this tare weight in Table 1 on the DATA SHEET.
7. Decant liquid of Beaker 1 into funnel. Remaining solids in Beaker 1, use distilled water to remove and into beaker 8. Place beaker 2 on hotplate and let boil until 10mL remain. Continue to boil on low until 2-3 mL remains.
The excess acid will be reacted with sodium hydroxide to determine how much acid remains. The amount of acid that reacted with the eggshell and the amount of calcium carbonate in the eggshell itself will be determined using this data. Procedure: The volume of drops from dropping pipettes designated for acid and base was calculated by measuring the volume of 20 drops from each pipette in a graduated cylinder, then calculating the volume per drop. These pipettes were used in all other volume measurements. Eggshell was ground, and a mass of 0.1 gram was transferred to an Erlenmeyer flask.
6) More distilled water was added until the water sat on the bottom of the meniscus; the volumetric flask was labelled with my name, the date and the product within the flask. Results Mass of empty boat | *To two decimal places *To two decimal places 0.97 g* | Mass of boat + powder | 2.03 g* |
Laboratory Report: Experiment 1 Standardization of hydrochloric acid by sodium carbonate solution Name: Cheung Chun Hin, Harry Class: 6L (12) Date: 11-9-2009 Objective: To determine the concentration of hydrochloric acid using sodium carbonate solution as a primary standard in volumetric analysis (acid-base titration) Principle of method: The concentration of the hydrochloric acid can be determined by the titration reaction between hydrochloric acid and sodium carbonate solution. Na2CO3 (aq) + 2HCl (aq) H2O (l) + CO2 (g) + 2NaCl (aq) From the above equation, We measure the volume of hydrochloric acid used in the titration (the difference of reading on the burette) and use it in calculating the concentration of hydrochloric acid. So the molarity of the hydrochloric acid Procedures: 1. The mass of anhydrous sodium carbonate required was weighed to prepare 250.0 cm3 of 0.05M sodium carbonate solution. 2.
Dependent Variable- Titration point of the solution. Variables- None, no graph. Part One 1.Obtain safety goggles! 2.Get and thoroughly wash out a 50 mL buret. 3.Fill the buret with thiosulfate; record the volume on the data table.