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Method for Titration Process

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Method for Titration Process: PREPERATION OF TITRATION: Once the 25 ml of sodium carbonate is transferred into the conical flask, and 3 droplets of methyl orange is added, the preparation of sulphuric acid is required to be ready. Obtain approximately 100 ml of sulphuric acid, with its mystery concentration, in a beaker. I shall obtain the clamp and place it on the table. I will also obtain the burette and attach it to the clamp, where it will be held up in the air. Beforehand, the burette was washed with sulphuric acid, to wash off any other substances that were in the burette. This assists to obtain reliable data, and remove any contaminated material inside. Insert small amount of sulphuric acid to wash the burette. Whilst screwing the burette onto the clamp, care should be taken whilst attaching it, because the burette shouldn't be tightly screwed. IT should be stable whilst it is attached to the clamp. If it is tightly screwed, it can cause the burette to break. On top of the burette, place the funnel on top, and get ready to insert the sulphuric acid. I made sure that the tap was turned off, by twisting it until, the handle was facing horizontally. ...read more.


This table will help me to determine the average titre: I shall do a dry run, which is just a practice run through of the experiment. After that I shall start the actual experiment. My dry run may not be accurate, because it was my first time, and I may have made some mistakes. Do therefore, I shall learn from my mistakes in the dry run, and use my skills to carry out the experiment. I shall be doing 5 repeats so I gain reliable data. The repetition shall show the reliability, and I shall stop doing the experiment, once I receive 2 concordant titres. The glassware needs to be cleaned every time I do a repeat. I do this by washing the glassware, with the solution that is going to go in. for example, I shall wash the burette with sulphuric acid, because sulphuric acid shall go into the burette. I shall wash the bulb burette with sodium carbonate, because sodium carbonate will be going into the bulb burette. However, only small amounts of the solutions will be used to clean the equipment, because every drop of the solutions is important in the experiment. References: http://www.chemguide.co.uk/physical/acidbaseeqia/indicators.html This web page helped to explain the indicator methyl orange. ...read more.


Therefore, you divide it by 4) 2.65g is needed to make 250 ml of Na2 CO3 (0.25 dm�) with the concentration 0.1 mol dm��. Therefore, Na2 CO3 contains 0.025 moles, due to 2.65 g produces 0.1 mol dm� (0.025 x 106 = 2.65 g) ...Concentration of Sodium Carbonate...: Concentration = no. of moles / volume Concentration = 0.025 moles / 0.25 dm� Concentration = 0.1 mol dm� Here is the balanced equation of the neutralization reaction between sulphuric acid and sodium carbonate: 1 : 1 ratio Na2 CO3 (aq) + H2SO4 Na2SO4 (aq) + H2O (l) + CO2 (g) 0.25 : 0.25 25 ml 28.2 ml 0.1 mol dm� There is a ratio between the number of moles between sodium carbonate and sulphuric acid. It is a 1:1 ratio, therefore, the number of moles in sulphuric acid must be the same as sodium carbonate (0.25mol dm�). 25 ml of 0.1 mol dm� of Na2 CO3 is neutralized by 28.2 ml of H2SO4. What is the concentration of sulphuric acid used? Concentration of Sulphuric Acid: Concentration = no. of moles / volume Moles Volume (mol dm�) (dm�) Na2 CO3 0.0250 0.2500 H2SO4 0.0250 0.0282 Concentration = 0.0250 / 0.0282 = 0.8865 mol dm� I have found out that 28.2 cm� of sulphuric acid with the concentration of 0.8865 mol dm�, was needed to neutralise 25 ml of 0.025 mol dm� of sodium carbonate. ...read more.

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