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

Titration I will neutralize the sulphuric acid with a base, which will be Sodium Carbonate (Na2 CO3),

Extracts from this document...


FINDING OUT HOW MUCH ACID IS IN A SOLUTION The aim of this experiment is to find out the concentration of acid in an acidic solution. The acidic solution I will be using is sulphuric acid, and the concentration of this solution is somewhere between 0.05 and 0.15 mol dm-3. I have to find an accurate value for this concentration and to obtain my results I will use a titration. A titration is a method of quantitive analysis, which can be used when 2 solutions react together. I will neutralize the sulphuric acid with a base, which will be Sodium Carbonate (Na2 CO3), which will already have a set concentration. I use an indicator, Methyl Orange, because when you do a titration between a strong acid and a weak alkali, as I am, Methyl Orange is the indicator used. Reaction Equation Na2 CO3 (aq) + H2 SO4 (aq) Na2 SO4 (aq) + H2O (l) + CO2 The mass of Sodium Carbonate I will need to use is shown below... Na2 CO3 = 2 X sodium + 1 X carbon + 3 X oxygen = 46 + 12 + 48 = 106 grams However this is the amount of grams for 1 mole of sodium carbonate. I need 0.1-mol dm-3 of it because this sum is between 0.05 and 0.15 dm-3 so I will divide by 10... ...read more.


> Now add 3 drops of Methyl Orange indicator to the conical flask > Use a clean, dry 100cm3 beaker to fill a burette with the sulphuric acid. Run a little of the solution out of the burette into the beaker to make sure the jet is full of solution > Record the volume reading on the burette before starting the titration and read the burette to the nearest 0.05cm3 > Add sulphuric acid in small volumes to the solution in the conical flask, swirling the flask after each addition. When the solution turns light pink stop the adding of sulphuric acid. > Record the final burette reading and calculate the volume of solution you have to run out of the flask The first titration I am going to do will be a trial run to make sure I know exactly what I am supposed to do. After wards I will repeat the titration until 3 concordant results are achieved within 0.1cm3 of each other. References Teacher support coursework guidance AS/A level GCE chemistry (salters) page 30 Activity E12 - salters advanced chemistry activity pack Hazcard 95 - sodium salts Hazcard 98 - sulphuric acid Hazcard 32 - Indicators Implementing Mass of glass weighing bottle = 50.08 grams Mass of weighing bottle and sodium Carbonate = 52.73 grams Mass of Sodium Carbonate = 2.65 grams I work out the mass ...read more.


To try and see when the solution turned pink I used a white tile underneath the conical flask. Basically I cannot tell the exact point when the solution turns into a pinky colour. This meant that each titration would not be exactly the same so wouldn't be a fair test. To improve this I could use computer and real time video recording because this would be far more reliable and accurate than my recording would be. The computer could save the colour of the original titration, and then the second titration could be done whilst someone is looking at the computer screen so they could see the exact point when the titration should be stopped. Another problem with my experiment was that I might not have shaken the conical flask particularly well when I was trying to dissolve the Sodium Carbonate in the distilled water. To make my results more interesting to analyse I could have done more titrations, this would mean I'd obtain a better average result and so I could find out a more precise answer for the concentration of the sulphuric acid. The exact answer to the concentration of the sulphuric acid was 0.099 (2 decimal places), but I have rounded this figure up to 0.1 mols dm-3, as I believe it takes into account the possibility of a percentage error. Finding out how much acid is in a solution Alex Pitt 1 ...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. How much Iron (II) in 100 grams of Spinach Oleracea?

    Three values within 0.1 cm3 of each other need to recorded in this experiment, as an average titre needs to be obtained. If points within 0.1 cm3 of each other are used the average results will be more accurate. This will also ensure that any random results are noted and

  2. Softening hard water with sodium carbonate (Na2CO3)

    The sodium ions stay dissolved in the water, but they don't cause water to become hard. This justifies my prediction because a greater quantity of Na2CO3 added to the water, means an increased number of CO32- ions. The more CO32- ions there are, the greater the amount of calcium that

  1. In order to find out the exact concentration of sulphuric acid, I will have ...

    The end-point should occur between 20-30cm3, if it does not the solution might have been mixed incorrectly. 22. By the end of the titration, the solution should resemble quite a dark yellowish/orange colour. 23. Now you will have to repeat the titration at least two more times and record the results, which appear to be in a close range.

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

    Make sure you wash it out with distilled water first to ensure there is no contamination. Place a beaker underneath the burette and place a funnel at the top. Fill it with sulphuric acid solution using the funnel to prevent sulphuric acid solution from splashing into your eye.

  1. Determine the concentration of sulphuric acid by acid-base titration.

    If a solution, add mineral absorbent and scoop up into a bucket. Rinse area of spill and the cloth or mop thoroughly. Sulphuric acid Dangerous with: water. Vigorous reaction when the concentrated acid is diluted. Always add the concentrated acid slowly to cold water when diluting, never the reverse.

  2. How to find the accurate concentration of the Sulphuric Acid.

    Recording correct results and measurements are essential to work out the exact concentration of the Sulphuric Acid used. When involved in a titration there are errors or uncertainties related to the precision of the equipment used. Therefore with the use of small-scaled pipettes, pipette fillers and burettes, precision is better and less errors will be caused.

  1. Chemistry Practical: Finding the water content of Na2 CO3 .xH2O by Titration

    Ensure that there is no air bubbles trapped. Step 3. Using the pipette filler place 25cm3 of the sodium hydroxide solution in the clean conical flask. Step 4. Add 4 or 5 drops of methyl orange indicator to the contents of the flask.

  2. Planning of Titration

    * A Volumetric Flask holds 250 cm3 solution but when using the formula c = n/v then the volume is 0.250 dm3 * C = n/v therefore 0.10 = n/0.250 so n = 0.025 mol * Now number of moles of Na2CO3 = mass/Mr so 0.025 mol = grams/Mr *

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