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

Determine the concentration of a limewater solution

Extracts from this document...


PLANNING AIM: To determine the concentration of a limewater solution. You have been provided with 250cm3 of limewater, which contains approximately 1g dm-3 of calcium hydroxide. Hydrochloric acid is also available, which has a concentration of exactly 2.00 mol dm-3. In order to determine the concentration of the limewater solution I will have to carry out a titration experiment between the acid being hydrochloric acid, HCl and the base being the limewater, Ca(OH) 2. However before continuing on with the titration you need to dilute the HCl acid since it is too concentrated to use. In order for you to do this you will need to work out the concentration of Ca(OH) 2. Balanced Equation of the titration: 2HCl + Ca(OH)2 --> CaCl2 + 2H2O 2 moles 1 mole 2 mol dm-3 ? Ca(OH)2 is 1g dm-3= 1 gram per 1dm3 No. of moles in Ca(OH)2 = Mass / Relative formula mass (RFM) = 1 / 74 = 0.0135 moles Concentration of Ca(OH)2 = No. of moles / Volume = 0.0135 / 1 = Ca(OH) 2 mol dm-3 Now that you have worked out the concentration of the lime water solution you can continue with the dilution process of HCl acid. ...read more.


* 250cm3 of HCl, 2.00 mol dm-3. * Distilled water. * 250cm3 volumetric flask and stopper. * Funnel. * Eye protection. METHOD: 1. Set up the burette stand and place the burette inside it. 2. Fill the burette with HCl acid, 2.00 mol dm-3 using a funnel to avoid spillage making sure the bottom of the meniscus touches the line. 3. Make sure the volumetric flask is clean and dry. 4. Place the volumetric flask underneath the tap of the burette. 5. Gently open the tap of the burette to allow the HCl acid to flow into the volumetric flask and close the tap when 2.5cm3 of HCl have been added. 6. Add distilled water to the volumetric flask containing the acid. *2 However you should not add water to HCl acid as the first drops of water will react completely, exothermically with the acid, boiling it and causing spillage. Nevertheless in this case you will add water but a little bit at a time and then put the stopper onto the volumetric flask and shake it to dilute the acid each time. ...read more.


11. The acid is then added to the Ca(OH)2 from the burette by opening the tap. A right handed person should use his left hand to open to open the burette tap and the right hand to hold the flask at the neck. 12. Release the solution of the HCl into the limewater solution slowly, observing the volumetric flask. When the solution changes from a light orange to a very light pink colour, this is an indication to stop and record the result. The white tile underneath the volumetric flask helps you with this because it gives you a better view of the colour change. 13. If the solution has turned pink then this is an indication that you have stepped over the end point and the titration is not valid. 14. Read off the side of the burette accurately how much volume is left and take this away from the initial volume to give you the volume of acid required to neutralise the base and record the titre. 15. Repeat the experiment 3 more times to give you more accurate results as anomalies do occur in this experiment. 16. Note all readings and work out the average of the volumes and work out the concentration of the limewater solution using the formula: concentration = no of moles / volume. ...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 Inorganic 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 Inorganic Chemistry essays

  1. Peer reviewed

    Determining the concentration of acid in a given solution

    5 star(s)

    Measuring the sodium carbonate solution 1 2 I need to make 250cm3 of a sodium hydroxide solution with the concentration of 0.1 mol dm-3. I will use solid hydrated sodium carbonate with the formula Na2CO3�10H2O.1 Mr (Na2CO3�10H2O) = (23+23+12+48+20+160) = 286 250cm3 of 0.1 mol dm-3 contains (0.1 x 250/1000)

  2. Peer reviewed

    Deducing the quantity of acid in a solution

    5 star(s)

    The most important part is to be very careful because it can cut and cause harmful wounds. First of all, if any glass equipment fall, we need to tell the teacher and ensure everybody is aware of the danger. Then, we need to sweep it thoroughly to ensure no shards remain and put it into the glass bin.

  1. effects Concentration and Temperature on the Rate of Reaction

    Although some of the acute hazards and symptoms associated with the concentrations I am using will not be as severe as those shown below, the risks are still very serious. For this reason I will still take appropriate precautions and will handle each substance with care.

  2. Bleaching experiment. Estimation of available chlorine in commercial bleaching solution.

    and the errors due to precision of apparatus (i.e. reading errors of burette.)there may still have been some possible sources of errors: The iodine solution should be used immediately because its molarity changes with time because: (i) Iodine is volatile which means that I2 can escape from the solution, causing the decrease of [I2]* with time.

  1. The Chemistry oh Phosphorous

    As the match is 'struck', friction heat causes some of this red phosphorus to convert to white phosphorus, which ignites instantly. The 3rd and final allotrope is black phosphorus. It is created by heating white phosphorus but also applying pressures of up to 12,000 atmospheres.

  2. Determination of the solubility of calcium hydroxide

    I will check to make sure no air bubbles have been drawn up. I then remove the pump slowly replacing it with my thumb. Keeping it on the top of the bulb pipette, I then move it to the conical flask.

  1. analysis of two commercial brands of bleaching solution

    Standard sodium thiosulphate solution was added to the burette. 8) The initial reading on the burette was recorded 9) Standard sodium thiosulphate solution was run out from the burette to the conical flask until the colour of the solution in the conical flask changed from reddish brown to pale yellow..

  2. The Effects of Strong and Weak Acids on the Order of a Reaction.

    Following the Rate of a Reaction If there is any significant change shown within the reaction, it can be measured by using one or more of the following methods: Dilatometry - When there is any significant changes made to the volumes of the liquids used in the reaction, this can be followed using a dilometer.

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