Repeat this step with 10, 20, and 30 pebbles. Part 3: Liquids 1. Obtain a container of solution A, and pour it into the graduate cylinder to the 20.0mL mark. Use a dropper pipet to obtain an exact reading. 2.
Finding the Concentration of a Sample of Sulphuric Acid The purpose of our experiment is to find the concentration of a sample of sulphuric acid accurately. We are provided with a range of indicators, solid anhydrous sodium carbonate and access to all laboratory glassware and equipment. Apparatus needed: - ------------------- Requirements to produce a Sodium Carbonate solution: - ====================================================== Electronic Balance (accurate to 2 decimal places) Goggles Spatula Distilled Water (250cm3) Anhydrous Sodium Carbonate (2.65g) Beaker - 250cm3 Stirring Rod Petri Dish Pipette Volumetric flask Requirements for the titration experiment: - ============================================ Goggles Burette (50cm3) Stand and Clamp Conical flask Sulphuric (IV) Acid (n*50cm3 based on how many repeats are conducted) Prepared Sodium Carbonate Solution Methyl Orange Indicator (10cm3) Funnel Pipette Pipette filler White Tile Method ------ Method for the production of Sodium Carbonate solution ====================================================== 1. Use the volumetric flask to get 250cm3 of distilled water 2. Place 2.65g of sodium carbonate in a petri dish (weighed on the electronic balance).
Calculate 20% of water and 80% of Hydrochloric acid for a solution of 150ml in total. Stir the solution in the beaker labeled “ Hydrochloric acid: 80%”. Leave it on the side. Pour 50ml of sodium Thiosulphate in the beaker labelled “Reaction” Now place the “X” under the beaker labelled “Reaction” Pour 50ml of “Hydrochloric acid: 20%” to “Reaction” Start timing Stop timing when the “X” is no longer visible. Record the reaction time in seconds in the data table.
Investigating How Quickly Amylase Breaks Down Starch With Varying Temperatures Instructions List I gathered the equipment shown below. I put 3 drops of iodine in each chamber of the spotting tile. I boiled the kettle and mixed together water from the kettle with water from the tap so the water reaches the correct temperature. The water was put into a beaker. 5ml of starch was put into a test tube.
A substitute we used the thermometer. Methods Trial Test In a 100ml beaker 30mls of water was placed the temperature of the water was recorded. 1 teaspoon of Ammonium Nitrate was added to the water and stirred until dissolved. The temperature was then recorded again. This was to see the difference between the initial temperature and the final temperature.
Secondly, measure as accurately as possible 25ml² of Sodium Phiosulphate and 5ml² of Hydrochloric acid. Thirdly, pour the measured amount of Sodium Phiosulphate into the beaker and then add the Hydrochloric acid. Once this is added start the timer. Finally, once the cross has completely disappeared stop the clock and make a not of the time it took for the mixture to become one. NOTE: This procedure was produced with different concentrations.
The measurement was .995g. The salicylic acid was transferred into a 125 ml Erlenmeyer flask and the acetic was given by the lab instructor. Three drops of 85% phosphoric acid. While swirling and mixing more was added and then clamp onto the sing stand in the boiling water for 8 minutes. 1 mL drops of water was added in the flask.
Temperature Changes During the Addition of Sulphuric Acid and Sodium Hydroxide Solution Aim To investigate the temperature changes during the addition of sulphuric acid and sodium hydroxide solution. Introduction In this experiment we are using sodium hydroxide, sodium hydroxide, sulphuric acid. We are trying to find out how much acid it takes to neutralise alkaline. But there are many things that could effect my final result and I think that the main thing will be measuring the acid and alkali out accurately so that the experiment was fair. Prediction We planned the experiment as a class and so we have all predicted that the same thing will happen to the results.
Finding the Ka of Ethanoic Acid Aim: ==== To find out the Ka of ethanoic acid, chloroethanoic acid and dichloroethanoic acid. Procedure: ========== 1. The pH meter is calibrated, using a buffer solution of accurately known pH. 2. 20.0cm3 of 0.10M ethanoic acid was pipetted into a conical flask.