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

Determination of the solubility of calcium hydroxide.

Extracts from this document...


Determination of the solubility of calcium hydroxide Aim I am aiming to determine the solubility of calcium hydroxide. Calcium hydroxide is an alkali and limewater is a saturated solution of it, therefore I can titrate it against an acid of whose concentration I know. Using this information I will be able to accurately estimate the concentration of the calcium hydroxide solution. I will be provided with limewater, which has an approximate concentration of 0.015 mol dm-3 and a solution of hydrochloric acid which has a known concentration of 0.3 mol dm-3. The concentration of the acid is too high so it will need to be diluted. Material Quantities Concentration of the acid Hydrochloric Acid + Limewater --> Calcium Chloride + Water Ca(OH)2 + 2HCl --> 2CaCl + 2H2O By observing the above equation I know that the calcium hydroxide reacts with the HCl in the ration 1:2, with the concentrations of the solutions at 0.015 and 0.3 mol dm-3 the ratio is 1:20 which means the reaction will take place far too fast to find an accurate end point. ...read more.


> Wash out burette with distilled water and then with the HCl solution. Fill the burette with the HCl using a funnel and rush the jet through making sure no air bubbles are trapped. > Then use a pipette and pipette filler to transfer 25cm of limewater into a washed conical flask and add 3 drops of methyl orange indicator. > Place the conical on a white tile underneath the burette and record the reading on the burette ready to titrate. > Whilst swirling the conical flask add the HCl from the burette to the Ca(OH)2 . > Look for the end point, which will be a slight colour change to orange and then add drop by drop to ensure you do not go over the end point. > When the end point is reached record the volume in the burette and subtract it from the initial volume to find the titre. Record this as a rough titration and repeat the experiment adding a few drops at a time as you become near to the endpoint. ...read more.


> Repeating the titration until all results are within 0.1cm3 of each other makes sure that the endpoint found is correct and accurate. > The burette readings are to 2 decimal places because this gives precise readings for the amount of titre so when calculating the concentration of the acid it will be accurate. Percentage errors Burette = 0.20% Pipette = 0.24% Flask = 0.08% Total Percentage Error = 0.52% Risk Assessment Hydrochloric Acid Corrosive and irritant. Wear eye protection and gloves. If substance gets in to eyes, mouth or on skin wash with water and seek medical attention. Calcium Hydroxide Corrosive and irritating to eyes. Wear eye protection and gloves. If hands are contaminated and the substance gets in to eyes or mouth, flood with excess water and seek medical attention. Calcium Chloride Irritant to eyes, skin and respiratory system. Is dangerous with water as it is an anhydrous salt and can cause water to boil. Wear eye protection and gloves. Use in a well ventilated area. If substance gets in to eyes, mouth or on skin then wash with water and seek medical attention. ...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)

    mL 10.00 mL = 0.0562M Solution IV [H+] = [OH-] M1 = [H+] = 0.05M V1 = Volume of HCl = 8.65 mL V2 = Volume of saturated solution = 10.00 mL M1 x V1 = M2 x V2 M2 = = 0.05M x 8.65 mL 10.00 mL = 0.0432M 2)

  2. Determine Solubility of KClO3 Salt.

    than the required temperature because there is temperature gradient between the test tube and the water inside the beaker. Besides this, there is no 100% transfer of heat from water bath to the KClO3 solution inside the test tube. Some heat will be transferred to the environment.

  1. Determination of the Solubility of Calcium Hydroxide.

    Calculate the quantity of sulphuric acid solution which has been used by reading the burette. Record this reading. 9. repeat steps 4-8 until there 3 results with a concurrent difference of 0.1cm3 of calcium hydroxide solution used Risk Assessment Calcium hydroxide is caustic and can cause blindness.

  2. Aim To calculate the solubility of Calcium Hydroxide (Ca(OH)2) by titration with Hydrochloric Acid ...

    If irritation continues seek medical help. Skin Contact: Wash off with soapy water. If Swallowed: If the person is conscious wash out their mouth with water. Call for medical help immediately. Hydrochloric Acid (HCl) * Hazards - Contact with eyes or skin can cause serious permanent damage.

  1. I have to plan an experiment to find the solubility of calcium hydroxide, Ca(OH)2, ...

    Once filled to the line, put a rubber bung on the flask, and mix the solution. Then allow it to settle down, so that the excess calcium hydroxide that was added, may be able to go down to the bottom, as shown in the diagram below.

  2. Determine the solubility of calcium Hydroxide solution with the aid of the titration process

    Depending upon the strength of an alkali and acid the right indicator is chosen: * A Titration between a strong acid and a weak alkali requires a methyl orange indicator. * A Titration between a weak acid and a strong alkali requires a phenolphtalein indicator * In a Titration between

  1. Determination of the solubility of calcium hydroxide.

    Place the pipette over the conical flask and by removing index finger from the open end of the pipette the calcium hydroxide solution will run into the conical flask. When nearly all of the solution has gone out of the pipette gently tap the pipette on the bottom of the conical flask to get another drop out.

  2. Determining the Solubility of Calcium Hydroxide.

    The concentration of the calcium hydroxide is 0.015mol dm-3. Therefore the hydrochloric acid needs to be a concentration of 0.03mol dm-3. Originally the concentration is 0.3mol dm-3 so I need to dilute this by a factor of 10. As the volumetric flask holds 250cm3 I require 1/10 of this to be hydrochloric acid.

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