Acid Base Titration

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Acid and Base Titration Aim: To determine the concentration of a dilute solution of sodium hydroxide which is approximately 0.1 mol dm-3 Introduction: Titration is an example of redox reaction and is a process of chemical analysis in which the quantity of some constituent of a sample is determined by adding to the measured sample an exactly known quantity of another substance with which the desired constituent reacts in a definite, known proportion. The process involves the gradual adding of standard solution of titrating reagent from a burette. The addition is stopped when the equivalence point is reached. From this point an exact equivalent of titrant will be added to the earlier solution. The completion of the reaction is marked by some signal; this signifies the end point. The signal can be a colour change of an indicator (Encyclopaedia Britannica, 2013). The experiment is repeated to obtain consistent results and will be later on calculated to achieve the averaged mean value of the titre. In acid-base titration the indicator is a substance that can exist in two forms, an acid form and a basic form, which differ in colour. A wide choice of acid-base indicators is available, varying not only in the colours of the two forms but also in their sensitivity toward acid or base (Encyclopaedia Britannica, 2013). In relation to this practical the Sodium Hydroxide (NaOH) is the strong base which dissolves in water to form an alkaline solution. The concentration of this solution can be determined by titrating it with a standard solution of a strong acid such as Hydrochloric Acid (HCl). The indicator to be used is Methyl Orange. Apparatus: * * Pipette (10cm3) and Filler * Burette (50cm3) * Conical Flask * Funnel * Glass beaker * Stand and Clamp (for burette) * White paper * Chemicals (NaOH, HCl, Methyl Orange for indicator)
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