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Titration lab report. Aim: to determine the quantity and concentration of NaOH to completely neutralize one molar hydrochloric acid till the n point.

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Introduction

Practical Report-3 Titration ________________ Aim: to determine the quantity and concentration of NaOH to completely neutralize one molar hydrochloric acid till the n point. Requirements: hydrochloric acid 0.5 mole, sodium hydroxide , pipette, pipette pump, conical flask, burette, stand, clamp, plastic funnel, beaker, phenolphthalein Hypothesis: the indicator is used to display the pH of the solution. It will display different colour in different acid and different in base. In this case when the pH of the solution increases and as soon as is crosses 7 the colour will change this will allow us to know the approximate amount of base (NaOH) ...read more.

Middle

Using a pipette and a pipette pump take 20 ml of HCl in the conical flask 2. Add few drops of phenoptheline to acid 3. Add NaOH in the burette till the 0 level 4. Slowly add NaOH to HCl 5. Stir the solution after adding every drop till the solution changes the colour Observations: Experiment Quantity of NaOH required for colour change/ml ±0.6cm3 Quantity of HCl used in the experiment/ml ±0.6cm3 1 8.2 10 2 12.1 15 3 16.1 20 Remember: 1. were lab coats during the experiment 1. conduct all the experiment at same time and place to keep the temperature and light intensity constant 2. ...read more.

Conclusion

0.1 moles dm-3 Therefore concentration for exp with 15 cm-3 is: 0.6 ± 0.1 moles dm-3 And concentration for exp with 20 cm-3 is: 0.6 ± 0.1 moles dm-3 Conclusion: The colour of the indicator turns pink in basic solution and the drop before the colour change is supposed to be the n point. This means that it is the point at which the solution is neutral. Using which the number of moles can be calculated so can the concentration which came to the results of no of moles as 0.005 moles in first experiment and the concentration which is constant to all the experiment comes to 0.6 ± 0.1 moles dm -3 ...read more.

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