Place a funnel into the top of the burette and then rinse the burette out by letting some sulphuric acid run through it. 3. Make sure the burette tap is closed and then fill the burette with
The flask was swirled continuously to ensure the Sodium Hydroxide is thoroughly mixed. 6. Stop the flow of the base when the Acid ‘A’ changes it color to light pink. 7. Repeat the process again with the second batch of Acid ‘A’ and record the results.
Remember, the sodium chloride will remove the histones and help break down the cell membrane. I then had to add 1 mL, 20 drops, of a premixed, 25% liquid dishwashing detergent to the test tube. As you know, dishwasher detergent is used to clean dishes by destroying fats; it does the same thing with cells. It disposes of the lipids and proteins that make up a cell. These would include the nucleus and the cell membrane.
The accuracy of titration results depends very much on the correct detection of the end point. Chemicals: Ethanedioic acid-2-water crystals Dilute sodium hydroxide solution Phenolphthalein Deionized water Apparatus: Beakers (100 cm3 ) x 4 Conical flasks (250 cm3 ) Pipette (25.0 cm3 ) Pipette filler Burette (50.0 cm3 ) Stand and clamp Volumetric flask (250.0cm3 ) Wash bottle White tile Glass rod Weighing bottle Electronic balance Stopper Chemical Reaction involved: Procedures: 1. Clean all the glassware involved in this experiment (e.g. burette, pipette, conical flasks, weighing bottle, volumetric flask, etc.) with deionized water as directed by the teacher.
I will use this to measure out the Hydrochloric acid and Distilled water because there volume together will equal 10cmÂ³. If I use a 50cmÂ³ Measuring cylinder, I won't be able to get a good enough accuracy. Stopwatch- For timing the experiment Pipette for measuring out accurately and piping back excess Hydrochloric acid Piece of paper with a black cross on it like this: To find out when the experiment has ended. It is dark and thick because I want to clearly see when the experiment has finished Paper towels: For washing beakers and measuring cylinders out. [IMAGE] 1.
The remaining solution should be blue. Bring the beaker back to the lab station and add ~ 10 mL of distilled water. Stir the mixture, all the while adding ~ 8 mL of 6M of NaOH to the beaker. Check with litmus paper to ensure that it is slightly basic. Fill the beaker with up to 100 mL mark with distilled water.
Investigating the Concentrations of Unknown Acids Aim To find out each of the concentrations of the hydrochloric acids in the Winchesters labelled A-E. This is going to be carries out by titrating the acid with NaOH. Equipment needed for this investigation Pipette - 25ml Burette Phenolphthalein Conical flask Beaker Funnel Pipette filler Clamp NaOH - the known acid of 0.1M HCl - the unknown concentration of acids White tile My predictions I predict that the different acid solutions of the HCl will be less than 0.1M because the Winchesters were topped up with water, which would have obviously weakened the concentration of the acid making the number of moles less than 0.1. Safety precautions when doing the experiment: v The equipment should be used carefully to prevent breakage of any glass. v The acids should be used carefully avoiding spillages and if any acid came into contact it should be rinsed with water immediately to prevent any irritation to the skin.
Next, take out the excess powder until the weight is 1gm. Then use two measuring cylinders, with each measuring the amount of water and dilute hydrochloric acid that should be added, e.g. when there is 30mls of acid, 0mls of water will be added; when there is 25mls of acid, 5mls of water will be added, and so on. The total amount will always be 30mls. Afterwards, I will pour the powder into a beaker that contain correct amount of acid in it and use a stop clock to time how long it will take for the powder to disappear.
Finding the Concentration of Calcium Hydroxide by Titration with Hydrochloric Acid. The Problem Perform a titration upon Calcium Hydroxide to find the concentration by using Hydrochloric Acid of 3 different concentrations as following 2 molar, 0.5 molar and 0.1 molar. In order to calculate the results must be within 0.05cm3 of each other. Apparatus Burette Volumetric Pipette Beakers Conical Flasks Volumetric Flasks Funnel Clamp Stand White Tile Fair Test For a fair test I will have to make sure that I change the equipment for each test so that the residue of the last test doesn't alter my results and also I must use the same amounts measured as accurately as possible. Preliminary Work The first experiment will have will have to be a titration with the given amounts of Hydrochloric Acid to see whereabouts my equilibrium will lie.
Then I will measure out the correct amounts of HCL and CaCO3(s) using a measuring cylinder for the HCL and the scales to measure the CaCO3(s) . These will be 20ml of HCL and 50g of CaCO3(s). Ounce I have done this I will fill the measuring cylinder with water, turn it up side down in the tub, making sure there are no air bubbles present and hold it up using the stand and clamp. Next I will slide the delivery tube up into the measuring cylinder. Finally I will use the piece of card to drop the CaCO3(s) into the test tube of HCL and secure the end of the delivery tube onto the top of the test tube so it can start to collect CO2, which will displace the water revealing the amount of CO2 given of from the reaction.