• 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 (VI) Acid that has a concentration between 0.05 and 0.15 mol dm.

Extracts from this document...

Introduction

Plan for the practical Assessment Aim - to find the accurate concentration of Sulphuric (VI) Acid that has a concentration between 0.05 and 0.15 mol dm� Apparatus 1. Standard Solution Scales 250cm� Volumetric Flask 100cm� Beaker 2. Titration Clamp Stand Burette Pipette Filler Beaker White Tile (iii) Chemicals Distilled Water Calcium Carbonate Sulphuric Acid Method for finding the Standard Solution 1. Calculate the mass of 1 mole of Sodium Carbonate by adding together the element's relative atomic masses, which can be found on a periodic table. 2. Calculate the mass of 0.1 moles of Calcium Carbonate. This is done by using the mass of 1 mole (calculated in step 1) ...read more.

Middle

As it is impossible with the equipment given to get exactly the right mass, note down the actual mass, given by the scales, to three decimal places. 5. Add 100cm� of distilled water to the weighed out Sodium Carbonate and stir until you cant see anymore Calcium Carbonate as it has all dissolved. Pour this into the 250cm� volumetric flask and fill up to the 250cm� line with distilled water. 6. After you have done this you can find the actual concentration of the solution by using the following equation: Moles of Sodium Carbonate in 250cm� = Mass dissolved Mass of 1 mole The second half of this experiment is titration. ...read more.

Conclusion

If it is swallowed, wash out mouth and give one or two glasses of water. Don't induce vomiting. Seek medical advice as soon as possible. If it is splashed into the eye flood the eye with gently running tap water for 10 minutes. Seek medical advice If it is spilt on clothes or skin remove the clothes quickly and wipe as much liquid as possible away with a dry clothe before drenching the area with lots of water. If a large area of skin was affected or blistering seek medical advice. If it is spilt in the laboratory, wear eye protection and gloves and cover with mineral absorbent and scoop into a bucket. Add anhydrous sodium carbonate and leave to react. Once the reaction has occurred add lots of cold water. ...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. Determine the concentration of sulphuric acid - Plan

    * Place the funnel into the 50.00cm3 burette. Ensure the burette tap is closed and fill the burette with the aqueous sulphuric acid. Record the initial burette reading. * Pipette 25.0cm3 of the Sodium Hydroxide solution into a 25.0cm3 conical flask. * Add 2-3 drops of the Methyl orange indicator to the conical flask * Run the aqueous

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

    of sodium carbonate, as it can been seen from the above equation. So far I have worked out the number of moles of acid used and the precise volume of an average titre and this means that I am ready to work out the specific concentration of the sulphuric acid.

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

    The solution should be delivered quickly until a couple of ml from the endpoint, swirling the flask after each point. 4) The endpoint should be approached slowly, a drop at a time. 5) The end of the reaction is when the first colour change is observed, which is yellow.

  2. In this experiment I am finding out how much sulphuric acid is present in ...

    Methyl Orange Methyl orange is toxic if swallowed, spilled or inhaled. Avoid skin contact with the solution or the solid. Wear safety goggles and gloves, for protection of spillages on skin and eyes. Small volume of Methyl orange solution can be flushed down a sink with a large quantity of

  1. To find the accurate concentration of sulphuric acid, by making up a standard solution, ...

    Reweigh it on an analytic balance. Make sure that the doors of the balance are shut 5 Record the mass. 6 Empty the weighing bottle into 100cm3, clean beaker and reweigh the empty bottle. Record the mass on a chart like this: Analytical Balance: Weight of Bottle and Solid X

  2. Find out the accurate concentration of an aid solution thought to have a concentration ...

    Run in small volumes of sodium carbonate solution until the first occurrence of a permanent peach colour in the titration mixture. This is the end point. 7. Record the final reading by reading off the burette at eye-level from the base of the meniscus and calculate the volume of sodium carbonate solution that has been used.

  1. Find the exact concentration of an acid solution. It is believed to have a ...

    I believe that 25cm� of sulphuric acid and 10 drops of indicator will be adequate to gain satisfactory results. 'Acids and alkalis are classified as 'strong' or 'weak' depending on the extent to which they form ions when dissolved in water.'

  2. Determine the concentration of lime water.

    Detailed method of procedure used To start the experiment I firstly need to dilute the Hydrochloric acid. By using a pipette and a flask it is a good way of making sure the experiment is accurate. I need to dilute the acid to 0.125 moles.

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