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The Estimation Of Ethandioic Acid And Sodium Ethandioate In A Mixture Containing Both

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Introduction

The Estimation Of Ethandioic Acid And Sodium Ethandioate In A Mixture Containing Both To determine the percentage of ethandioic acid and sodium ethandioate in the mixture will require two titrations, one in which the reactant will react with both the sodium ethandioate and the ethandioate and a second which will react with only one of them. From previous As investigational work we know that Sodium Hydroxide will react with ethandioate acid. Ethandioic acid reacts with calcium, iron, sodium, magnesium and potassium to form salts called oxalates. This reaction produces sodium ethandioate. This reaction will therefore only react with the ethandioic acid and not the sodium ethandioate. For this titration an indicator is required, phenolphthalein. Phenolphthalein is a colourless weak acid, which dissociates to form pink anions. When in alkaline conditions, the equilibrium of the reaction shifts to the right and the concentration of the anions is enough for a pink solution to be observed. Phenolphthalein works as an indicator in this reaction as it is between a week acid and a strong base to form a solution with an alkaline pH. From preliminary work we also know that potassium manganate will react with ethandioic acid and sodium ethandioate. ...read more.

Middle

By decreasing the pressure the level of the solution will fall. Carefully allow some of the solution out so that the bottom of the meniscus is in level with the like marked on the pipette. Transfer the solution in the pipette into a conical flask. Touch the end of the pipette against the inside of the conical flask to release the remaining mixture from the pipette. Add three to four drops of the phenolphthalein indicator to the mixture. Place the conical flask on the white tile underneath the jet of the burette. Open the tap of the burette and allow about 2cm3 of the sodium hydroxide out into the conical flask, then swirl the solution. Repeat this until the solution in the conical flask is almost pink. Slow the flow of the sodium hydroxide so that it is coming out drop at a time swirling the solution all the time. As soon as the solution becomes pink it has reached the end point of the reaction. Stop the flow of sodium hydroxide and record the volume of sodium hydroxide left in the burette, then work out the volume of sodium hydroxide used. ...read more.

Conclusion

Analysis Titration of Ethandioic acid and Sodium Hydroxide * Number of moles of Sodium Hydroxide: 0.06 x Volume 1000 = A * Number of moles of Ethandioic acid: (Using equation for mole ratio) Moles of Sodium Hydroxide, A 2 = B Titration of Ethandioic acid and Sodium Ethandioate with Potassium Manganate * Number of Moles of Potassium Manganate 0.02 x Volume 1000 = X * Number of Moles of Ethandioate acid: (Using equation for mole ratio) Moles of Potassium Manganate, X x 5 2 = Y Percentage Composition of Ethandioic acid and Sodium Ethandioate * Mass of Ethandioic acid present in 25 cm3 in titration with Sodium Hydroxide: (Mr of Ethandioic acid = 126) Moles, B x 126 = C * Mass of Ethandioic acid present in 200 cm3 in titration with Sodium Hydroxide Mass, C x 8 =D * Mass of Ethandioic acid present in cm3 in titration with Potassium Manganate: (Mr of Ethandioic acid = 126) Moles, Y x 126 = Z * Mass of Ethandioate acid present in 200 cm3 in titration with Potassium Manganate: Mass Z x 8 = T * Percentage of Ethandioic acid present in mixture: Mass, D 2 = _____ % * Percentage of Sodium Ethandioate: (Mass, T - Mass, D) 2 = _____ % ...read more.

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