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Experiment: Titration Aim My aim is to find the volume of hydrochloric acid needed to neutralise sodium hydroxide.

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Introduction

Experiment: Titration Aim My aim is to find the volume of hydrochloric acid needed to neutralise sodium hydroxide. Theory Titration is a laboratory method used to analyse a chemicals concentration. In this experiment 10cm3 of sodium hydroxide should be neutralised by 10cm3 of hydrochloric acid. Phenolphthalein is used in this experiment as an indictor where the base is a pink colour and acid as a cloudy white colour. When they are use to neutralise each other the mixture goes clear at the endpoint. The endpoint is where the number of moles in both solutions is equal. Different types of titration: * Acid based titration - neutralisation between an acid and a base * Redox titration - form of oxidation reduction * Complexometric titration - used to find certain ions Equipment The equipment I am going to use in this experiment; * Funnel * Hydrochloric acid * Sodium hydroxide * Bosshead / clamp * Stand * Conical flask * Burette * White tile * Goggles * Measuring cylinder * Phenolphthalein Funnel Diagram Bosshead / clamp Burette stand Sodium hydroxide Phenolphthalein White tile measuring cylinder hydrochloric acid Conical flask Method 1. ...read more.

Middle

The chemicals can be very dangerous if it is at a high concentration. Sodium hydroxide: It is a very harmful corrosive; it can cause burns as well as permanent damage to eye if contact with it. The E.U classification for sodium hydroxide is corrosive. To prevent potential risk I am going to wear goggles in this experiment. Hydrochloric acid: Hydrochloric acid is very corrosive and can damage eyes if it comes into contact. It's also lethal to fish from 25 mg/l up also toxic for aquatic organisms due to pH shift. To prevent potential risk I am going to wear goggles in this experiment. Phenolphthalein: Phenolphthalein is safe to use and it doesn't appear to have any safety risks. Result table Number of times the Cm3 of hydrochloric Experiment was repeated acid needed 1 10 2 9.7 3 10.2 4 9.8 5 10.4 Average 10.02 Calculations Hcl = hydrochloric acid Naoh = sodium hydroxide Mr - NaoH Na + O + H 40g Mr - Hcl cl + H 36.5g No. of moles of Naoh Volume x molarity 0.02L x 0.5M = 0.01 moles (20ml) ...read more.

Conclusion

What would i do to the limewater in the experiment. This is only the planning part of the coursework so i only need to show my method, apparatus, safety precautions etc. you dilute the acid.. any low concentration will do.. i would go for 0.1M/0.25M... better not have it tooo concentrated for safety reasons. fill the burette with the Acid and using a pippete, put 25cm3 of the limewater into a conical flask with a few drops of indicator (phenophthalin(howeva u spell it)) and titrate till eqivalence point (till the drop that turns the solution pink permanently) read the volume of acid used from the burette. the concentration of acid is known so find the number of moles now using write out the equation and use stochiometry to find mumber of moles of Ca(OH)2 present. your volume was 25cm3 (with the pippete) so calculate concentration by c=n/v yea basically its the same thing coz the number of moles of acid needed will never change... so if its more concentrated, less acid will be needed, but n=CV .... you will always get the same number of moles in the end, no matter what concentration you use.. but dont have it too concentrated or else youll have a highly exothermic vigourous reaction... keep away from that! ...read more.

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