• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

Titration of acid and alkaline

Extracts from this document...


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.


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.


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.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Aqueous Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related GCSE Aqueous Chemistry essays

  1. Marked by a teacher

    chemistry coursework

    4 star(s)

    This part of my conclusion does not support my prediction. Evaluation The procedure used to carry out the experiment proved to be excellent, although the only problem was trying to establish the end point of the experiment.

  2. Softening hard water with sodium carbonate (Na2CO3)

    ==> The definition of a lather must remain constant throughout the experiment, a lather is of a height of 2 cm. or more and lasts for at least 10 seconds. 5) Increase the amount of soap solution in each boiling tube by 0.1 cm3 and shake each tube twenty times.

  1. To carry out a titration between a strong acid and a weak alkali, to ...

    all of the solution from the funnel into the graduated volumetric flask. I can work out the percentage error for my measurements, using this formula: Formula: True Value - Experimental Value x 100 True Value I can work out the percentage error for the concentration of my sulphuric acid solution.

  2. Planning of Titration

    The solution should be delivered quickly until a couple of ml from the endpoint. * Prepare the solution to be analyzed by placing it in a clean or rinsed with distilled water conical flask. Add the indicator methyl orange to the sulphuric acid.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work