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

I have to plan an experiment to find the solubility of calcium hydroxide, Ca(OH)2, in water. I have to make up a solution of calcium hydroxide and carry out a titration using hydrochloric acid solution of the chosen concentration

Extracts from this document...

Introduction

Determination of the solubility of calcium hydroxide I have to plan an experiment to find the solubility of calcium hydroxide, Ca(OH)2, in water. I have to make up a solution of calcium hydroxide and carry out a titration using hydrochloric acid solution of the chosen concentration. The equipment need is as below: * Solid calcium hydroxide * Methyl orange indicator * Volumetric flask (250cm3) * Clamp and boss * Clamp stand * Burette (50cm3) * Conical flask * Pipette (25cm3) * Pipette filler * Distilled water * White spotting tile * Hydrochloric acid of chosen concentration * Beaker x2 * Rubber bung * Funnel x2 * Electronic scale 'The maximum mass of calcium hydroxide needed to produce 1dm3 of saturated solution at room temperature is 1.5g.' I only want 250cm3 as I am using a 250cm3 volumetric flask. Therefore: 1dm3 / 4 = 250cm3 1.5g / 4 = 0.375g The number of moles in volumetric flask: 0.375 / 74 = 0.005 moles I need an excess of 0.5g to make sure that all the calcium hydroxide has been fully dissolved: 0.375g + 0.5g = 0.875g I have to now work out the concentration of hydrochloric acid I will be using. The molar mass of calcium hydroxide is: C = 40 O = 16 (x2) H = 1 (x2) R.A.M = 74 The concentration of calcium hydroxide at the beginning will be: 1.5 / 74 = 0.02 So, the concentration is 0.02 mol/dm3 In ...read more.

Middle

After being rinsed, take out 25cm3 of calcium hydroxide from the volumetric flask, using the pipette. 25cm3 is easily measured on the pipette, as there is a mark line. Be careful when doing this, as if you suck up the solution too quickly with the pipette, then air gaps form in the pipette, and this means you will not have a full 25cm3 of solution, making the experiment unreliable. After, release the solution of calcium hydroxide into the conical flask. Add four drops of methyl orange indicator to the conical flask, and the solution will now turn orange. Titration The burette will be rinsed out with 0.04 mol/dm3 hydrochloric acid, so during the experiment, the hydrochloric is not contaminated with solutions previously used in the burette. Before rising out the burette, make sure that the tap is closed in the horizontal position. Bring the burette down to a level where you can be pouring into it at your height level, so you do not have to reach up, otherwise this could be a hazard. Place a funnel inside the top of the burette, and carefully pour the hydrochloric acid into the burette via the funnel. Once full to the top, open the tap, and let the dirty hydrochloric drain into a beaker. Once the burette has been thoroughly rinsed, close the tap again, and pour in fresh 0.04 mol/dm3 of hydrochloric acid. Fill the burette to the top, where the reading will be 0cm3. ...read more.

Conclusion

Then follow the method used for the first titration. The results will be recorded in a table which has rows, with the initial volume reading of the burette, final volume on burette, and the volume of acid used. The columns will be the titration number, and the end column will be the mean volume used. Calculation of the solubility of calcium hydroxide * Moles of Hydrochloric acid: = concentration x volume = 0.04 mol/dm3 x mean volume * There is for every one moles of calcium hydroxide, two moles of hydrochloric acid, therefore we need to divide the amount of moles of hydrochloric acid by two, to get the number of moles of calcium hydroxide. The number of moles of Ca(OH)2 = mean x 0.04 in one solution of volume 25cm3 2 * We want the number of moles of calcium hydroxide in 1dm3 of water, therefore we need to work out its concentration. Moles of Ca(OH)2 in dm3 = mean (dm3) x 0.04 x 1000 2 x 25 * The molar mass of calcium hydroxide is 74. If we multiply the concentration of calcium hydroxide by the molar mass, then this will tell us the amount of solid calcium hydroxide which will dissolve in 1dm3 of water. 20 Solubility of Ca(OH)2 in g/dm3 = mean x 0.04 x 1000 x 74 2 x 25 = mean x 0.04 x 20 x 24 = mean x 59.2 g/dm3 ?? ?? ?? ?? Dipen Patel Chemistry Planning Page 1 ...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. Marked by a teacher

    Determine the solubility product of calcium hydroxide

    3 star(s)

    Solution II : A saturated solution of Calcium Hydroxide in 0.1M Sodium Hydroxide. Solution III : A saturated solution of Calcium Hydroxide in 0.05M Sodium Hydroxide. Solution IV : A saturated solution of Calcium Hydroxide in 0.025M Sodium Hydroxide. 1.

  2. Marked by a teacher

    Enthalpy of Neutralisation.

    3 star(s)

    When this number is scaled to a molar quantity, it is called the enthalpy change of the reaction, ?H. Reactions between liquids and solids are easily carried out in such a device or a reaction may be carried out externally (as in the experiment)

  1. Titrating Sodium hydroxide with an unknown molarity, against hydrochloric acid to find its' molarity.

    This would mean that the molarity of the solution would not be the same throughout the graduated flask. * All of the equipment used was washed with distilled water and the chemical that would be placed in it or dried before the titration took place.

  2. Determine Solubility of KClO3 Salt.

    distilled water means that you have obtain solution that considered as a saturated solution and the solubility of the salt is maximum. Later on, the measuring cylinder is placed in a beaker that contain of hot water. At the beginning of the experiment, we use 40 oC as the temperature of the hot water in the beaker.

  1. To run the synthesis of calcium oxalate via the precipitate from solution containing calcium ...

    After that, 1.5ml of saturated ammonium oxalate solution and 1.5 gram of solid urea was added into the solution. - With stirring, the solution was gently boiled until the colour changes from red to yellow. Some water was added during the heating process to compensate for loss of water due to evaporation.

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

    Burette cleaned with distilled water and rinse with 5cm� NaOH solution a few times. Burette filled with NaOH solution using a funnel. The pipette is cleaned and rinse a few times with the acid to be used in the titration.

  1. Determining the Solubility of Calcium Hydroxide.

    Quantities of Materials to use 2HCl(l) + Ca(OH)2(l) CaCl2(l) + 2H2O(l) From the above equation it is clear that I require 2 moles of hydrochloric acid to react with 1 mole of calcium hydroxide. Therefore I will use a hydrochloric acid solution that is twice as concentrated as the calcium hydroxide.

  2. Determination of the Solubility of Calcium Hydroxide.

    Use the pipette pump to fill the clean pipette with hydrochloric acid. The bottom of the meniscus of the hydrochloric acid must be on the 25cm3 line. This ensures that there is exactly 25cm3 of the hydrochloric acid in the pipette, and that an accurate concentration of 0.03moldm-3 will be produced.

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