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Titration of acid and alkaline

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Introduction

Planning The main task at hand is to find the concentration of a given volume acid. I am going to complete this task by using a method called titration. Titration is the process of finding the concentration of the given acid or base by neutralizing the solution using a known volume and concentration of alkaline or acid. In this case I know that the concentration of the unknown acid will lie between 0.05 and 0.15 mole dm��, so for my alkaline I am going to create a concentration of 0.1 mole dm��. I have chosen this concentration because it is the average median of where the acid concentration could fall. To complete this titration I need to know when the solution will be neutralised, to know when the solution will be neutral I need to use an indicator. An indicator indicates when the solution reaches PH level 7; this is normally indicated by a colour change. The acid that I will need to find the concentration of is sulphuric acid (H2SO4) and the alkaline that I will be able to control is sodium carbonate (Na2CO3). This indicator I am going to use needs to be strong acid based because I am using a strong acid (H2SO4) ...read more.

Middle

Once I have made the solution of sodium carbonate I should then be able to find the concentration of the sulphuric acid to do this I need to complete the titration. Once the titration has been complete I can then collect the results for example if 30cm� of alkaline neutralised the 25cm� of acid then I can find out the concentration of the acid. Because I know the concentration of the alkaline (0.1 mole per dm��) I can find the acid but I need to find the concentration in 30 cm�. I do this by 30/1000 x 0.1 = 0.003 mole so in the 25 cm� of acid there is 0.003 mole. To find the concentration in a litre 1000/25 = 40 so I need to 40 x 0.003 = 1.2 mole. Method To begin this titration I need to create my solution, I need to weigh 2.65g of anhydrous sodium carbonate I will do this by weighing a beaker and then weighing out 2.65g of anhydrous sodium carbonate into the beaker. To weigh the chemicals and the beaker I will use a digital balance that is capable of weighing within 0.01g, this is for increased accuracy. ...read more.

Conclusion

Sulphuric acid (H2SO4) is a corrosive substance and should be cleaned with plenty of water if it comes into contact with eyes or skin. If ingested it can cause severe problems straight away and you should seek medical attention. Sodium carbonate (Na2Co3) if inhaled may cause irritation to the respiratory tract. If it comes in contact with the skin it can cause irritation with redness again it should be rinsed with water. If alkaline comes in contact with the eyes it should be rinsed for about 10 minutes. Methyl orange should be treated the same as the acid and alkaline as explained as above. Accuracy Using a burette has a tolerance of 0.1 cm� this means that if the burette is full then it could be out by 0.1 cm� so if it's full to 5cm� then it could be inaccurate by 0.01 cm�. I will also use a white tile that I will place under the acid with the indicator in, to exaggerate the colour change this will help me see the change in colour and determine when the solution is neutralised. I should also make sure that everything that measure is to the bottom of the meniscus. To ensure there is no contamination I will rinse each piece of equipment and apparatus off with distilled water before use. ...read more.

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