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

Determining the equilibrium constant for the hydrolysis of Ethyl Ethanoate Definition

Extracts from this document...


HYPOTHESIS Determining the equilibrium constant for the hydrolysis of Ethyl Ethanoate DEFINITION Chemical equilibrium is when, in a the rate of the forward reaction is equal to the rate of the reverse reaction. When a chemical reaction has reached equilibrium, collisions are still occurring: the reaction is now happening in each direction at the same rate. This means that reactants are being formed at the same rate as products are being formed, and this is indicated by double arrows,. At equilibrium, the reaction can lie far to the right, meaning that there are more products in existence at equilibrium, or far to the left, meaning that at equilibrium there are more reactants. The concentration of the reactants and products in a reaction at equilibrium can be expressed by an equilibrium constant, symbolised Kc Kc = [ethanoic acid][ethanol] [ethyl Ethanoate][water] CH3COOC2H5 + H2O CH3COOH + C2H5OH ETHYL ETHANOATE + WATER ETHNOIC ACID + ETHANOL CH3COOC2H5 Ester group The functional group -COOR, R here is a ethyl group C2H5. ...read more.


They are soluble in water and in organic solvents and are neutral to litmus tests. Esters are used as artificial perfumes or scents as they emit a sweet smell. Also they can be used in making artificial food flavours that are added in many edible items like ice creams, soft drinks, sweets, etc. Esters are also used as industrial solvents for making cellulose, fats, paints and varnishes and also as solvents in pharmaceutical industries. Some esters are used as softeners in plastic industries and moulding industries. Many esters have distinctive odours, which has led to their widespread use as artificial flavourings and fragrances. For example methyl butyrate smells of pineapple or apple, isopentyl acetate smells of pear or banana (it is used as the flavouring in the manufacturing of old fashioned Pear Drops) and methyl benzoate smells of fruity-ylang ylang. Ethyl formate smells of rum. Ester are also used in the biosynthesis of fats and fatty acids, and in the making of soaps. General formula of an ester. ...read more.


These included wearing of an over coat to protect clothes from spillages, placing a mate on work surfaces to protect it from heat as well as wearing of goggles to protect ones eyes from irritation. Also when handling hot test tubes, forceps and gloves need to be used to prevent one from burning their hands. Hands also need to washed after every experiment to wash off any excess chemicals. CONCLUSION I was able to perform the hydrolysis of Ethyl Ethanoate as well as to determine the equilibrium constant. The standard value is 0.23 and due to my results my experiment was very successful. My average Kc value was 0.22 and this was even better. The experiment was very successful. ANALYSIS AND EVALUATION For the calculations of the titrations, when determining the end point I had to be very careful not to pass the end point. Also we had to leave the reagents for a week so that they could reach equilibrium. My experiment was highly successful with all the results proving the success and accuracy of the experiment. ...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 equilibrium constant - Kc; of ethanoic acid reacting with ethanol producing an ...

    Reactants / Products CH3COOH C2H5OH CH3COOC2H5 H2O Volume (cm3) 0 75 75 100 Mass (g) 0.00 59.25 69.00 100.00 Moles in Total 0 1.29 0.78 5.56 Moles Initially 0.00000 0.00516 0.00312 0.02224 Moles at Eqm. 0.00145 0.00661 0.00167 0.02079 Molecular masses are such: CH3COOH = 60 C2H5OH = 46 CH3COOC2H5

  2. The aim of this experiment is to answer the following question: What is the ...

    A 10ml measuring cylinder will be used so that the reactants can be measured accurately. A thermometer will be used so that the temperature of the water bath can be verified. Risk assessment The chemicals I will be using are: * Hydrochloric acid (known concentration of 0.1moldm-3-150ml approx.

  1. Determination of the equilibrium constant for esterification of ethanoic acid and propan-1-ol by using ...

    19.50 19.75 6.85 6.75 Calculations : 1. Equation for the esterification reaction between ethanoic acid and propan-1-ol: CH3COOH (l) + CH3CH2CH2OH (l) CH3COOCH2CH2CH3 (l) + H2O (l) 2. Equation for the neutralization reaction between ethanoic acid and NaOH: CH3COOH (l) + NaOH (aq) � CH3COONa (aq) + H2O (l) 3.

  2. Obtain pure samples of Ethanol (CH3CH2OH) and Ethanoic Acid (CH3COOH) from fermented Yeast (Saccharomyces ...

    and Sodium dichromate (VI) mixture will be refluxed for approximately 20 minutes. With the reflux apparatus, as the reaction mixture boils, vapour passes into the condenser where it cools (see diagram), changes into a liquid and falls back into the flask. No vapour is able to escape into the atmosphere.

  1. Identification of an Organic Unknown.

    The reliability of the results is entirely dependant on observations therefore must take into account differences between different people. Also it would be more reliable to use a colorimeter to test the colour of certain results however it was

  2. Determination of the Equilibrium Constant for Esterification - Ethanoic Acid and Propan-1-ol

    How many moles of unreacted CH3COOH remain at the end of the refluxing? (iii) Calculate the concentrations of the other species present at equilibrium. (iv) Give the equilibrium expression for the reaction. (v) Calculate the equilibrium constant for the reaction.

  1. Determining an equilibrium constant

    added Mass of water added/g 5.105 � 0.002 2.946 � 0.002 PART B: Tube number Final burette reading/ cm3 Initial burette reading/ cm3 Titre/ cm3 1a 0 � 0.05 9.61 � 0.05 9.61 � 0.05 1b 0 � 0.05 9.62 � 0.05 9.62 � 0.05 2 9.61 � 0.05 35.10

  2. Test the hypothesis that lipids have special properties inrelation to solvents.

    The top layer turned red in the test-tube containing the water and oil as the oil rose to the surface since oil is less dense than water. Finally the test-tubes containing the ethanol and the oil showed a faint red colour at the top and this was because some of

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