A titration reaction is carried out between potassium hydroxide of 1.00 mol dm^-3 and ethanoic acid of unknown concentration. Ethanoic acid is a weak acid. To perform better using Burnett’s, the acid is normally poured into the burette. It is known that the concentration of the ethanoic acid lies between 0.8 mol dm^-3 and 0.9 mol dm^-3.

You are given:
1. 150 cm^3 of each of the reactants.
2. Several 200 cm^3 flasks.
3. A 50.0 cm^3 burette.
4. A 25.0 cm^3 pipette.
5. A 25 cm^3 measuring cylinder.
6. Methyl orange and phenolphthalein indicators.

Your task is to give a detailed procedure of the experiment to be conducted in order to achieve best results. You need to provide a chemical equation, a table of observation with possible value of the titration, and an expected calculation with your suggested values of the titration. State also the indicator you are using with a reason.