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

Finding the concentration of a chemical. Outline of procedures: to prepare a standard solution of sodium carbonate and carry out a series of titrations to determine the concentration of hydrochloric acid.

Extracts from this document...


Title of experiment: preparation of standards sodium carbonate solution Outline of procedures: to prepare a standard solution of sodium carbonate and carry out a series of titrations to determine the concentration of hydrochloric acid. Finding the concentration of a chemical A solution of known concentration is called a standard solution. Hazardous substances being made or used. Nature of hazards Quantities being used Control measures and precautions Sodium carbonate Hydrochloric acid Irritant corrosive 2.65g small Wear goggles Wear lab coat and goggles. Any non-chemical hazards and precautions to be taken Any spills to be wiped immediately Disposal of residues. Done by Technician Apparatus: * balance * weighing bottle * spatula * beaker * glass rod * wash bottle * filter funnel * volumetric flask * pipette * teat pipette * conical flask * burette Method To prepare a standard solution first I will calculate the mass of solute needed. ...read more.


The steps I will take to complete this experiment are as follows. 1: Measurements To make 250cm3 of 1.00mol/l solution of sodium carbonate I will use the following measurements: Mass of 1.00 mol of Na2CO3 = 106g Mass of Na2CO3 needed to make 1.00 l of a 0.100mol/l solution = 10.6g Mass of Na2CO3 needed to make 250cm3 of a 0.100mol/l solution = 2065g 2: Mass of weighing bottle = 9.277g Calculated mass of anhydrous sodium carbonate = 2.65g Mass of weighing bottle + solid = 11.93 g 3: (i) With a clean dry spatula I added anhydrous sodium carbonate to the weighing bottle using a top pan balance until the weighing bottle and contents reached the combined mass that I had calculated. (ii) I then poured 100cm3 of distilled water into a clean beaker and carefully tipped the sodium carbonate into the beaker. ...read more.


(iii) I stopped when the solution turned pink and measured the level of HCL left in the pipette. (iv) Then repeated these steps three times to get a fair result Trial 2 3 Average Final burette reading 21.50cm3 20.90cm3 21.10cm3 Initial burette reading 0.00cm3 0.00cm3 0.00cm3 Titre 21.50cm3 20.90cm3 21.10cm3 21.00cm3 Results: Na2CO3 + 2HCL --> NaCl + H2O + CO2 Mols of Na2Co3 = 0.0025 Ratio = 1:2 Mols of HCL = 0.005 Concentration of HCL = 0.238mols/dm3 Conclusion: In this experiment I was able to find out the concentration of a chemical through many experiments. This experiment was carried out under conditions similar to those in an industrial process but there were a couple of differences which include the amount of chemoicals available to us which hampered our chances of experimenting with different types of chemicals. I think this experiment was a success because I achieved my goal and learnt a lot from it. ?? ?? ?? ?? Page:1 Mohamed hassan student number: 20042512 ...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. Electronic spectroscopy - Homoleptic chromium(III) complexes and the spectrochemical series.

    simply states that the crystal field effects of each ligand type are purely additive and hence that the crystal field environment around the metal centre is an average of these effects. It can be expressed mathematically as ? (MXaYb) = a/a+b ?

  2. The basic aim of this experiment is to determine the percentage concentration of Iron ...

    all over the table, as it may stain - If spillage occurs, wipe off immediately - When pouring solutions into burette, if possible, do it on the floor, or below you eye level to ensure that the solution you are pouring will not spill all over.

  1. Titration with a primary standard.

    This will introduce error into your volume measurements. Liquid should drain cleanly from the sides if the inside of the buret is clean. The teflon stopcock should pull out easily from the end of the buret. Remove the stopcock before cleaning the buret. Scrub out the barrel of the buret with detergent and a buret brush.

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

    Pipette - is required to add small amounts of solution, up to a specific graduation point. Beaker - is primarily used to storage, sulphuric acid in this case. Top pan balance - is needed to measure 2.65g of anhydrous sodium carbonate exactly.

  1. To determine the concentration of a sodium carbonate solution

    The apparatus needed for the titration:- * Labels- so we can tell which beaker or flasks contains what. * 1x Burette- so to measure the acid drop by drop how much is used.

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

    the temperature that produces the most accurate results). At a temperature of 0oc Firstly work out the moles of Potassium Manganate (VII) (aq) in the titration. Moles = Concentration x Volume Moles = 0.01 mol dm -3 x 28.82

  1. Analysing the ethanoic acid concentration in different types of vinegars.

    However as the vinegars are a mixture of various acids I cannot obtain a Ka value for it and so will not be able to work out a value for the [Acid] from the vinegars from my pH readings. However I will still measure the pH of the vinegars, as

  2. Softening hard water with sodium carbonate (Na2CO3)

    highly flammable, additionally wear safety specs to prevent any splashes going into your eyes. ==> It is important to ensure that all the tubes are shaken an equal number of times so that in each case the softened water has an equal chance to form a lather with the soap.

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