To determine the solubility of calcium hydroxide.

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Aim: To determine the solubility of calcium hydroxide

Introduction and definitions

Titration is an analytical method in which a standard solution is used to determine the concentration of another solution. Because titration is an analytical technique, the proper method must be used if you are going to get meaningful quantitative results. A titration is a process in which a measured volume of a solution is added to a reaction mixture until some observable property has changed. An acid/base titration uses the fact that one can be "neutralized" with the other. In this neutralization reaction, the acid and base will combine to produce a salt plus water. When done correctly, the resulting solution will be "neutral" neither acid nor base. In a titration, this is known as the end point. The change in pH of the solution can be monitored using an indicator. It is extremely important that the exact amounts of each solution used be known at the end point.

A neutralisation reaction is the process in which the acidity or alkalinity of a substance is destroyed. Destroying acidity means removing the H+ (aq) ions by reaction with a base. Destroying alkalinity means removing the OH- (aq) ions by reaction with an acid. The acid and alkali particles must be in exactly equal amounts to get a perfectly neutral solution.

Neutralisation

Acid + Alkali = Salt + Water

H+(aq) + OH- (aq) = H20 (l)

Aim:

In this experiment I am going to determine the solubility of calcium hydroxide in water by titrating against a known concentration of hydrochloric acid. I will collect the data that from titration in order to calculate the solubility of Ca(OH)2.

Materials:

  • Volumetric flask of 250cm3
  • Conical flask 250cm3 
  • Burette for titration that contain Ca(OH)2 solution
  • Pipette 25cm3
  • Pipette filler
  • Methyl orange indicator to show the end point of the reaction i.e. when the orange is achieved
  • White tile to be able to see clearly the end point of the reaction.
  • Clamp stand to hold the burette
  • 0.3 M hydrochloric acid solution
  • 2*50cm3Beaker
  • 0.015M Calcium hydroxide

Safety

Risk assessment

During the experiment long hair should be tied back to prevent distraction. Stools should be placed under the tables to avoid accidents. Surface area show to be clear, to avoid spillage and breakages.

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Safety

  • Lab coat
  • Goggles
  • Hair tied back

Hazards

Chemical risk

Hydrochloric acid it very corrosive, wear eye protection and gloves. Use a fume cupboard because its vapour is very irritating to the respiration system. It also causes severe skin burn. If the solution is swallowed seek medical attention immediately, and if spilt on skin and clothes remove clothing and wipe liquid off skin with a cloth also seek medical attention. It is dangerous to add water to acids, (hydrochloric acid) but since a low concentration is used, it is relatively safe.

Calcium hydroxide (limewater) is mildly corrosive, ...

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