Rinse the burette with the standard oxalic acid solution. It is the point where no more titrant is required and the reaction is complete. Fix the burette in the burette stand and place the white tile below the burette in order to find the end point correctly. Wash the burette with water after titration is over. The strength of KMnO4 is calculated by using the molarity. Equivalent weight of oxalic acid = Molecular weight/No of electrons lost by one molecule, Equivalent weight of oxalic acid = 126/2 = 63, For the preparation of 1 litre of N/10 oxalic acid solution amount of oxalic acid required = 6.3 g. (b) Titration of potassium permanganate solution against standard oxalic acid solution: To calculate the strength of given KMnO4 in terms of molarity the following formula is used. The formula for oxalic acid is (COOH)2.2H2O. Since sodium hydroxide is not a primary standard a standard solution of oxalic acid is prepared and used for standardisation of sodium hydroxide. Where a 1 and a 2 are stoichiometric coefficient of oxalic acid and KMnO 4 in a balanced chemical equation. Let’s see… MnO4(-) is reacting under acidic conditions, so it goes to Mn(2+). Any solution whose strength is known is called a standard solution. The balanced equation for the reaction between oxalic acid and permanganate ion is as below. Turn the flask of measurement until the oxalic acid dissolves. 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Weigh the exact amount of clean and dried watch glass and record its weight in the notebook. What Bob is talking about is the dehydration of oxalic acid by hot concentrated (undiluted) H2SO4. The basicity of oxalic acid is 2 means it is a dibasic acid. Note down the upper meniscus on the burette readings.

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