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

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

Extracts from this document...

Introduction

Titration assignement: Aim: The aim of my investigation is to determine the solubility of calcium Hydroxide solution with the aid of the titration process. Titration can be defined as the method of determining the concentration of a substance in solution by adding to it a standard reagent of known concentration in carefully measured amounts until a reaction of definite and known proportion is completed, as shown by a color change or by electrical measurement, and then calculating the unknown concentration. An example could be, a given volume of a solution of unknown acidity may be titrated with a base of known concentration until complete neutralization has occurred. This point is called the equivalence point and is generally determined by observing a color change in an added indicator such as phenolphthalein. From the volume and concentration of added base and the volume of acid solution, the unknown concentration of the solution before titration can be determined. Titrations can also be used to determine the number of acidic or basic groups in an unknown compound. A specific weight of the compound is titrated with a known concentration of acid or base until the equivalence point has been reached. ...read more.

Middle

Will function as the alkali. The target of our experiment is to evaluate the solubility of this compound. Limewater (0.015 mol dm -3) Will be placed into the beaker containing the solid calcium hydroxide. It will function as an indicator and will give us visible proof of when the neutralisation will have reached completion. Graduated Burette Will be containing the hydrochloric acid, and also controlling the amounts of acid falling into the beaker. It is specially built to enable to control the amounts of its content, which exit the burette. This will allow us to measure the amount of hydrochloric acid needed to completely neutralise the calcium hydroxide. 10 cm3 volumetric pipette Will be used to fill up the graduated burette with hydrochloric acid. It is important to transfer the hydrochloric acid from the conical flask to the graduated burette in a safe manner, trying to avoid spllages and most importantly any contact with the body. It also allowes us to accurately and precisely measure the amount of acid that we place into the graduated burette. 100 cm3 conical flask Will be containing the hydrochloric acid before I extract it with the aid of the volumetric pipette. ...read more.

Conclusion

* If spilt in laboratory: wear eye protection, scoop up as much as possible. Add water to the area, followed by mineral absorbent. * If dust inhaled: remove victim to fresh to rest. Seek medical attention if breathing is even slightly affected. * If spilt on skin or clothes: brush off as much solid as possible. Remove contaminated clothing. Flood affected area with large quantities of water. If a large area is affected or blistering occurs, seek medical attention. Non-chemical hazards and precautions to be taken: It is important to arrange the equipment in a way in which there is minimum chance of the equipment being knocked over. Therefore placing the equipment towards the centre of the table is preferable rather than towards the edges. It is important to wear safety spectacles and labcoats throughout the course of the experiment. It is aslo advisable to wear gloves when handling calcium hydroxide. Disposal of residues: Hydrochloric acid - Wear eye protection and gloves. Solutions are best neutralised with sodium carbonate before being disposed of in the fouk water drain with further dilution. Very dilute solutions used in volumetric analysis may be washed away without neutralisation. Calcium hydroxide - Wear eye protection and gloves. Add solid little by little to a large excess of water in a bucket. Leave for one hour before pouring the solution down the foul-water drain. 1 Chemistry coursework 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

    Investigate the effect of changing the concentration of sodium hydroxide (alkali) on the volume ...

    4 star(s)

    Temperature of reaction mixture (�C) Colour of indicator 2. Using the measuring cylinder, 20cm� of sodium hydroxide was added to the polystyrene cup. A few drops of phenolphthalein indicator were then added to the acid. The colour of the changed from colourless to pink solution changed to pink. 3.

  2. Marked by a teacher

    Determine the solubility product of calcium hydroxide

    3 star(s)

    = M2 x V2 M2 = = 0.05M x 6.50 mL 10.00 mL = 0.0325M Solution II [H+] = [OH-] M1 = [H+] = 0.05M V1 = Volume of HCl = 18.25 mL V2 = Volume of saturated solution = 10.00 mL M1 x V1 = M2 x V2 M2

  1. Marked by a teacher

    Enthalpy of Neutralisation.

    3 star(s)

    35 40 45 50 The factors that might affect the results of this experiment are: 1. Volume. 2. Concentration. 3. Type of substance used. 4. Catalyst. 5. Pressure. Volume can affect the experiment because if it is not kept constant them results will be varied and there would be no

  2. Investigate a neutralisation reaction between hydrochloric acid and sodium hydroxide.

    I drew a line of best fit, which was appropriate. From this I found out that my results show a strong relationship because some points on the graph were exactly on the line of best fit and some were just off.

  1. A titration to determine the ratio of moles of Sulfamic acid to Sodium Hydroxide ...

    >Drain this into a conical flask and rinse neck of flask with distilled water. >Place the flask under the burette, set up as shown. Diagram >First roughly titrate the solution with the Burette of NaOH measuring the start and end points.

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

    were as precise as possible: * Ensuring that the temperature was constant throughout the titrations; as temperature affects the rates of reactions. The higher the temperature, the faster the rate of reaction, so if the temperature increased towards the end of the experiment, the end points would have been reached faster than before.

  1. To carry out a titration between a strong acid and a weak alkali, to ...

    This may have been because I did not add 3 drops exactly. This means the green colour of the indicator (methyl orange) was less concentrated and required less acid to make it become clear. For my rough titration and my fourth titration, I used three drops.

  2. Explain how the enthalpy change of neutralisation can be used to determine the relative ...

    = 135 x 1.00 = 135g Grams (50cm3) = 135 ? 20 = 6.75g Next a measuring cylinder will be filled with an accurate 50cm3 of distilled water. The unknown acid solute will then be poured into a clean 100cm3 beaker (labelled U).

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