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

Chemistry Practical Plan

Extracts from this document...


Chemistry Practical Plan. Aim: The aim of this experiment is to identify the chemicals below in the solutions A to F using suitable reactants, and also carry out a titration procedure to determine the concentration of aqueous nitric acid. *Aqueous calcium hydroxide *Ethanoic acid *Nitric acid *Aqueous Potassium Bromide *Aqueous Sodium Chloride Safety: Wear goggles to avoid chemicals getting into eyes. Immediately clean up spills that might occur. Use gloves if handling strong chemicals. Aqueous sodium hydroxide: Apparatus: Solutions A to E Calcium Carbonate Bunsen burner Stand and Clamp Test tube Conical Flask Stopper with tube. Diagram: Method: I will set up the apparatus as shown as above. When heating calcium carbonate carbon dioxide gas is released; this gas will go down the tube to the solutions. ...read more.


When Nitric acid is added to Magnesium, Magnesium nitrate and hydrogen if formed. We can test for hydrogen gas by lighting up a splinter, and putting it in the conical flask full of hydrogen gas really quickly (to stop hydrogen escaping), and see if it 'pops'. Equation: Mg(s) + 2HNO(aq) --> Mg(NO)(aq) + H(g) Word Count: 146 Aqueous potassium bromide: Apparatus: Solutions A to E Aqueous Chlorine solution Test tubes. Plastic Pasteur pipettes Diagram: Method: The apparatus will be set up the way it is shown above. Potassium bromide can be tested by adding aqueous chlorine solution, some of the bromide ions are oxidized to bromine. Some of the bromine molecules combine with the bromine ions to give tribromide ion. ...read more.


Add exactly 25cm of aqueous Sodium Carbonate into the pipette and into the conical flask. Add three drops of Methyl Orange indicator to the flask. Using the funnel pour the nitric acid solution into a burette, and take off the funnel. Titrate the nitric acid slowly into the conical flask until colour change appears. Do 1 rough titration, and 3 final titrations. Equation: NaOH(aq) + HNO3(aq) --> NaNO3(aq) + H2O(l) Calculations: Calculating the average titration volume: (Titration Volume 1 + Titration Volume l 2 + Titration Volume 3) / 3 Number of moles in Sodium Carbonate: Moles = concentration x volume / 1000 Moles = 0.500 x 25 / 1000 = 0.0125 mol From the equation we can see that the ratio is 1:1, therefore the number of moles in nitric acid = 0.0125 mol. Concentration = (Moles/Volume) x 1000. Concentration of nitric acid = (0. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our AS and A Level Organic 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 AS and A Level Organic Chemistry essays

  1. The aim of this experiment is to produce Aspirin. This is an estrification in ...

    x 180 = 0.3011g The mass of aspirin that didn't react was: 0.3086 - 0.3011 = 0.0075g Percentage by mass of aspirin (percent purity) = 0.3011 x 100 = 97.56% 0.3086 BACK TITRATION(12) Calculations Re-crysatalised aspirin Average titre = 8.50 + 8.50 = 8.50cm3 2 Mass of aspirin used =

  2. The aim of this experiment is to investigate the enthalpy change of combustion for ...

    Another complication was that it was hard to measure the temperature, start the stop clock and continue to stir the water simultaneously. This would have therefore increased the human error in the experiment along with the human error produced when measuring the temperature on the thermometer.

  1. investigating the amount of ascorbic acid present in fruit

    to the flask by using a 1ml graduated pipette. 6. Measure accurately 6.00ml of distilled water by using a 10ml measuring cylinder. 7. Add this to the 250cm3 conical flask too, then place a rubber bung onto the flask so that the solution doesn't get oxidised.

  2. Enzyme catalysed decomposition of hydrogen peroxide

    Plan: copper sulphate used ranged from 0.0m -0.2m in increments of 0.02 Variables: I will; Keep the volume of catalase (yeast) constant Keep the temperature constant at 40 oC by using a water bath. Keep the volume of Hydrogen peroxide constant Result: Conclusion Catalase is made of a central heme and four polypeptide chains.

  1. coursework plan for halogenalkanes

    + :Cl - (aq) AgNO3 & CH3CH2OH 2. CH3CH2CH2CH2Br (l) + :OH - (aq) CH3CH2CH2CH2OH (aq) + :Br - (aq) AgNO3 & CH3CH2OH 3. CH3CH2CH2CH2I (l) + :OH - (aq) CH3CH2CH2CH2OH (aq) + :I - (aq) Below shows three ionic equations for each hydrolysis reaction that I will carry out:- 1.

  2. Finding the concentration of an acid sample

    Flood eye with water for ten minutes. Seek medical attention. Sodium Carbonate Salts Irritant See sulphuric acid See sulphuric acid Scoop as much solid as possible up. Add mineral absorbent and scoop into bucket. Rinse area and mop thoroughly. See sulphuric acid Methyl Orange Minimal Hazard See sulphuric acid See sulphuric acid Scoop as much solid as possible up.

  1. Comprehensive and Detailed Chemistry notes

    - Nitrogen and Hydrogen are formed from ammonia ( reverse reaction ). - At the start rate of reaction is slow - Equilibrium is reached when forward reaction rate is equal to the reverse reaction rate - Conditions must be established to shift equilibrium to the right yielding more ammonia.

  2. Fuels Coursework Plan

    My second independent variable for the further investigation will be the position isomers of Propan-1-ol, Propan-2-ol, Butan-1-ol, and Butan-2-ol, and therefore again my dependant variable will be the enthalpy change of that particular fuel. There are also control variables, which are variables which will be kept constant and controlled throughout the full experiment.

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