• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month
Page
  1. 1
    1
  2. 2
    2
  3. 3
    3
  4. 4
    4
  5. 5
    5
  6. 6
    6
  7. 7
    7
  8. 8
    8
  9. 9
    9
  10. 10
    10
  11. 11
    11
  12. 12
    12
  13. 13
    13
  14. 14
    14
  15. 15
    15
  16. 16
    16
  17. 17
    17
  18. 18
    18
  19. 19
    19

Find out how much acid there is in a solution

Extracts from this document...

Introduction

Planning 11. a) Identifies and defines a question or problem and devices a practical procedure that is comprehensive and coherent to respond to the question or problem; describes fine detail about the procedure. > Aim My aim is to find out how much acid there is in a solution. I have been provided with a sample of sulphuric acid solution which has a concentration between 0.05 and 0.15 mol dm��. I will need to find its accurate concentration by carrying out a quantitative analysis known as titration. > What is titration? A titration is a quantitative analysis which can allow you to determine the precise end-point of a reaction. This is when two solutions are reacted together. One solution of known concentration is placed in the burette. The second solution is placed in the conical flask. An indicator is involved depending on how strong or weak the acid or alkali is. The solution in the burette is run into the conical flask just enough until the reaction is complete. This can be indicated by the change in appearance of the solution. > Apparatus * Beaker(s) (100cm�) * Balance * Spatula * Anhydrous Sodium Carbonate (2.65g) * Distilled Water * Glass Rod * Funnel * Volumetric Flask (250cm�) (class B) * Rubber or Plastic bung * Burette (class B) * White Tile * Small Funnel * Sulphuric Acid * Conical Flask (250cm�) (class B) * Pipette (25ml) (class B) * Pipette Filter * Methyl Orange Indicator * Lab Coat * Goggles * Gloves > Method Making the Solution * Direct Weighing Version * Firstly, turn on the balance. Make sure the surface of the balance is clean. * Place the empty beaker on the balance and record it's mass. * Press the Reset or Tare button. Now the balance should read zero. * Use the spatula to carefully add 2.65g of Sodium Carbonate into the beaker. ...read more.

Middle

This will be indicated by the meniscus on the calibration line. The error will be 0.2cm� or 0.08% Pipette (Class B) When a 25cm� is pipette is used correctly it will have an error of 0.06cm� or 0.24% Error � 100 Percentage Error = Actual Reading * In this experiment I will be using 2.65g of Sodium Carbonate. It has an experimental error of �0.005g 0.005 � 100 Percentage Error = 2.65 Percentage Error = 0.189% * Here is the calculation which shows the number of moles of Sodium Carbonate Na2CO3 Na = 23 Ar � (2) = 46 C = 12 Ar = 12 O = 16 Ar � (3) = 48 46 + 12 + 48 = 106 Mr Moles (mol) = Mass (g) � Molar Mass (Mr) = 2.65 � 106 = 0.025 mol * All of the apparatus which are involved in this experiment must be checked that they are not damaged, furthermore they will be thoroughly cleaned and rinsed with the distilled water to get rid of any dirt or unknown liquids. This will reduce the possibilities of experimental errors and will help in giving more accurate set of results. * When making the solution of Sodium Carbonate it is important to add small quantities from the spatula as it will prevent the risk of exceeding over the required value. This method will be quite effective and reliable. * When the Sodium Carbonate crystals have been thoroughly dissolved in the beaker, it is important to rinse out the glass rod in the beaker with some distilled water to wash away any leftover Sodium Carbonate. * When transferring the Sodium Carbonate solution from the beaker into the volumetric flask, it is important to use a funnel and the particular pouring technique; this is when the glass rod is held against the beaker for the solution to flow straight into the burette. ...read more.

Conclusion

* Harmful-Substances which are similar to toxic but are less dangerous. Potential Health Issues * Inhalation May cause irritation in the respiratory system. Some of the symptoms include coughing, sore throat, laboured breathing and chest pains. * Ingestion May cause irritation in the Gastro-Internal Track. Symptoms include nausea, vomiting and diarrhoea. * Skin Contact May cause mild irritation and slight redness. * Eye Contact May cause mild irritation and slight redness. Handling and Storage * Methyl Orange Indicator must be stored in a tightly stored container. * It must be kept in a cool, dry and ventilated area. * It must be protected from any physical damage, direct sunlight and freezing. * The containers of this certain solutions may still be hazardous when empty as the chemical residue still remains. * All warnings and precautions stated for this product must carefully be observed and followed. In the event of an accident... * The area of leak or spill must be ventilated. * Sensible protective equipment must be used to clean up the spills. * The liquid must be recovered to prevent any further damage. * Collect liquid in an appropriate container or absorb with an insert materials. E.g. Vermiculite or Dry Sand. * Do not use combustible materials such as saw dust. Exposure Controls and Personal Protection * Ventilation System A dilution ventilation is a satisfactory health hazard for this solution. In the case of discomfort to the worker a local exhaust system should be considered. * Skin Protection Protective gloves must be worn at all times when handling this chemical. * Eye Protection Safety goggles must be worn at all times. First Aid * Eye or Skin Contact In the case of contact, immediately wash eyes or skin with plenty of water for at least 15 minutes. Remove contaminated clothing. Seek medical attention immediately. * Ingestion If swallowed do not induce vomiting. Have large amounts of water and seek immediate medical attention. * Inhalation If inhaled, go out in fresh air. Immediately seek medical attention if having trouble in breathing. ...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?

    9) Attach crocodile clips to the two strips of metal and using wire connect them both to a high-resistance voltmeter. 10) Record the voltage of the Iron-Copper cell, and note which side is positive and which is negative. 11) Repeat the experiment using varying concentrations of Iron (II) Ammonium Sulphate (aq)

  2. The Use of Volumetric Flask, Burette and Pipette in Determining the Concentration of NaOH ...

    NaOH + HCl -> NaCl + H2O Materials and Apparatus 50cm Burette Phenolphthalein Solution HCI Solution (1.000 x 10-2M) Watch Glass H2SO4 Solution (1.000x10-2M) Ring Stand 500ml Beaker NaOH Solution 25ml Volumetric Flask Pipette Bulb Funnel 250cm Erlenmeyer flask 20cm or 25cm Pipette Distilled water Suction Experimental Procedures 1.

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

    A strong acid is an acid, which is completely ionized in an aqueous solution; in other words an acid, which is capable of producing 1 or more protons for every acid molecule originally present. Basically I have to find out the unknown concentration of sulphuric acid.

  2. construction science and materials

    anything from 3 to 11 years, can measure over 25mm in length. The adult emerges through a flight hole 6 - 8mm in diameter BRICKS: Sulphate attack: When water soaks into brickwork, the soluble salts will dissolve in the water.

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

    * Pipette filler and pipette (to transfer sodium carbonate solution to a conical flask) * 3 drops of Methyl orange (to show colour change-end point of titration) * White tile (to show colour change clearly for more accuracy so we can determine the exact point the titration ends.

  2. The Use of Volumetric Flask, Burette and Pipette in Determining the Concentration of NaOH ...

    The NaOH solution is topped up to 250cm� with distilled water, the cap is closed and the flask is rotated several times to get a homogenous solution. 4. This solution is poured into a clean and dry beaker, labeled, covered with with a watch glass and putted aside.

  1. Planning of Titration

    Distilled Water Weighing Bottle Calculation of Sodium Carbonate According to equation 1 mol of Na2CO3 = 1 mol of H2SO4 Mr of Na2CO3 = (23)2 + 12 + (16)3 = 106 g mol-1 1 dm3 = 1000 cm3 Below are the calculations of finding the mass of Na2CO3 required to

  2. Investigation of the carbonate - bicarbonate system

    When stability is achieved, alkalinity is said to buffer the solution. Buffering of an aqueous system is the equilibrium between the acid and base reaction, this is done when the hydrogen [H+] ion is either used up or donated so that the pH of the solution remains normal, that is, remains as the original pH of the system.

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