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

To find the accurate concentration of sulphuric acid, by making up a standard solution, sodium carbonate, to titrate against the acid. The titration is therefore an acid-base reaction.

Extracts from this document...

Introduction

Finding the Accurate Concentration of Acid in a Solution. Aim: To find the accurate concentration of sulphuric acid, by making up a standard solution, sodium carbonate, to titrate against the acid. The titration is therefore an acid-base reaction. Na2CO3 + H2SO4 --> H20 + CO2 + Na2SO4 Apparatus: 250cm3 volumetric flask and its stopper Funnel Glass rod 1 Bottle of distilled water Weighing bottle 100cm3 beaker Spatula Top pan balance Analytical Balance Making a Standard Solution As I am only provided with anhydrous sodium carbonate, my idea is to find how much of this solid is needed to make up the standard solution for the titration. To do this I must determine the approximate number of moles of the alkaline I want. As the concentration of acid is approximately between, 0.05-0.15 mol/dm3, it is best if the concentration of the alkaline is approximately the same, as the ratio of sulphuric acid to sodium carbonate is 1:1. This allows equal volumes to be used. I have decided to take the mean value of 0.05-0.15 for the number of moles for the alkaline I want. Therefore: (0.05+0.15) / 2 = 0.1mol/dm3 Now that I know the number of moles, I can substitute the known into a formula and find the mass of anhydrous sodium carbonate needed to make up s standard solution. ...read more.

Middle

Make sure to run the solution and distilled water though the jet too. 2 Set up a clamp stand and place a white tile firmly by the leg 3 Close the tap on the burette and pour the acid through carefully. Fill the burette up to zero. Place a small, clean beaker under the burette and run the acid though into the beaker. This fills the jet and check to see if there are any air bubbles present. (The acid in the beaker can be poured into the burette again) 4 Connect burette to the clamp stand and read value off to 2 d. p using a magnifying glass. This is you initial reading. 5 Rinse a pipette with distilled water and the solution to be pipette. Connect the pipette to its pipette fuller by holding the ends together and pushing firmly. Then pipette out 25cm3(up to the mark present on the pipette itself) of standard solution (the alkaline) and bring the conical flask to the pipette and fill by pressing on the lever. 6 Wash out the sides of the conical flask by using distilled water, so all content are being titrated. Do this periodically for more accurate results. ...read more.

Conclusion

VOLUMETRIC FLASK- the best equipment for best dilution. WHITE TILE-ensures the reliability as you can see if any drop are present on it, informing toy that the experiment has lost some atoms and ions and therefore not accurate as it could be. Also when titration begins the colour can be easily contrasted against the white tile, indicating when to stop titrating. This eliminates the possibility of over titrating. SUFFIENT INDICATOR-too much indicator could mean the titration process needs to titrate the indicator as well as the acid. MENISCUS: a meniscus is the shape that the solution makes and is quite thick. Always be consistent and read from the bottom of the meniscus to the mark, as represented on the diagram below. REPEATS- all experiments are independent to each other so neither experiment has an influence the tire. Repeating the experiment till the titres are consistent increases reliability as the answer is evidently within range. A ROUGH TITRATION-the rough allows over titration to be made a, eliminating the possibility of over titration at the later stage. RISK ASSESMENT Sulphuric acid (H2SO4) - Between the moles 0.5-1.5, it is known irritant to the eyes and the skin. Wear goggles and gloves when handling. (ii) Anhydrous Sodium Carbonate (Na2S04) - Irritant to eyes. Wear goggles when handling. (iii) As several glass equipment is going to be used carefully handle them. Clear any spills. ...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. Planning of Titration

    the things listed above happening and also you wont be able to do the experiment properly which will affect the results so make sure that take time but work smoothly and accurately. Titration rough 1 2 3 4 5 Final Burette Reading (cm3)

  2. Preparation of Primary Standard and Acid Base Titration

    Discussion: 1. Mass of ethanedioic acid crystals used: = 2.50 g No. of moles of ethanedioic acid: = 2.50/ (12.0x2+1.0x2+16.0x4) = 0.02778 mole Molarity of ethanedioic acid = 0.02778/0.250 = 0.11112M No. of mole needed: = 0.11112 x (15.40/1000) = 1.711 x 10�� Equation: Mole ratio of C2H2O4 to NaOH is 1:2.

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

    Titration Curves I think that a titration curve for this reaction: H2SO4(aq) + Na2CO3(aq) � Na2SO4 (aq) + H2O(l) + CO2(g) is going to resemble letter S turned 900 anti-clockwise. The first part of the curve is going to be sloping downwards, because there will be a weak acid present in the solution.

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

    This is an acid-base titration therefore the chemical reaction I am expecting sulphuric acid to donate H, which will be accepted by the sodium carbonate. The end-point of this particular titration is when all the alkali has been neutralized and neither excess acid nor excess alkali is present in the solution.

  1. Finding out how much acid there is in a solution.

    Risk assessment * Always wear a lab-coat to protect your skin and cloths from harmful substances. * Wear goggles at all times during an experiments, to protect your eyes from chemicals. * Make sure that long hair is tied back and that any dangling clothes and jewellery are tucked away

  2. How much Iron (II) in 100 grams of Spinach Oleracea?

    = 0.0000985 mol dm-3 This answer tells me how many mols are present in 1000cm3 but as I only used 100cm3 solution I need to multiply my results by 1000. 0.0000985 x 1000 = 0.0985 mols dm-3 This answer is very close to the expected results of 0.1 mol dm-3 that I was expecting for this experiment.

  1. Titration I will neutralize the sulphuric acid with a base, which will be Sodium ...

    Methyl Orange Indicator This is a toxic indicator, so it is very harmful if consumed. Do take care when using and clean up any spillages if there are any afterwards. Also don't inhale the dusts when the bottle is opened as these can irritate your eyes and be harmful to your respiratory system.

  2. Experiment to determine the concentration of sulphuric acid

    For accuracy, the amount should be looked from under the line. The hydrochloric acid is put into the burette using the funnel. It is measured to approximately 0.00 cm� but does not have to be exactly this. The number is recorded.

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