I thought that the end point was always pink when using phenolphthalein
You are adding acid to base.
The indicator in base is red and the end point is considered when the equivalence point is reached between pH8-10, which is when the phenolphthalein turns colourless.
The indicator in base is red and the end point is considered when the equivalence point is reached between pH8-10, which is when the phenolphthalien turns colourless.
but is this not a neutralization reaction therefore meaning that the end point is neutral? How am I meant to know it's A?
The indicator in base is red and the end point is considered when the equivalence point is reached between pH8-10, which is when the phenolphthalein turns colourless.
Sorry to bother you again Charco, but why is CH3COCH3(l) a better solvent for cyclohexanol than CH3CH2CH2CH2CH2CH3 (l)?
but is this not a neutralization reaction therefore meaning that the end point is neutral? How am I meant to know it's A?
The actual end point of this titration (equivalence point) is at pH 7, but 1 more drop then turns the mixture to pH10 so you see the red colour turn colourless.
The actual end point of this titration (equivalence point) is at pH 7, but 1 more drop then turns the mixture to pH10 so you see the red colour turn colourless.
Are they not asking for the end point? In my text book it clearly says that it would be pink..
I am not saying you're wrong I am just really unsure why this is...seems really odd..
Endpoint=neutral
Colour of neutral solution in phenolphthalein= pink
Sorry to bother you again Charco, but why is CH3COCH3(l) a better solvent for cyclohexanol than CH3CH2CH2CH2CH2CH3 (l)?
Thank you very much for your help.
The efficiency of solvents is a balance between the solvent intermolecular forces acting (solvent-solvent), the solute intermolecular forces (solute-solute) and the solvation forces (solvent - solute).
All particles exhibit van der Waals induced dipole attractions, the strength of which is dependent on the available surface area, which is turn is a function of the relative mass and shape.
The hydrocarbon is relatively large and has appreciable induced dipole attractions with itself.
The ketone has also permanent dipole -dipole interactions with itself, but relatively weak solvation forces.
However, cyclohexanol can interact with itself via both induced dipole, permanent dipole and hydrogen bonding.
The hydrocarbon cannot disrupt these forces using only induced dipole, but the ketone can interact via dipole -dipole with the cyclohexanol and also it can form hydrogen bonds between the lone pairs on the oxygen and the hydrogen of the cyclohexanol. This extra bonding tips the balance in favour of propanone as a solvent.
The actual end point of this titration (equivalence point) is at pH 7, but 1 more drop then turns the mixture to pH10 so you see the red colour turn colourless.
The efficiency of solvents is a balance between the solvent intermolecular forces acting (solvent-solvent), the solute intermolecular forces (solute-solute) and the solvation forces (solvent - solute).
All particles exhibit van der Waals induced dipole attractions, the strength of which is dependent on the available surface area, which is turn is a function of the relative mass and shape.
The hydrocarbon is relatively large and has appreciable induced dipole attractions with itself.
The ketone has also permanent dipole -dipole interactions with itself, but relatively weak solvation forces.
However, cyclohexanol can interact with itself via both induced dipole, permanent dipole and hydrogen bonding.
The hydrocarbon cannot disrupt these forces using only induced dipole, but the ketone can interact via dipole -dipole with the cyclohexanol and also it can form hydrogen bonds between the lone pairs on the oxygen and the hydrogen of the cyclohexanol. This extra bonding tips the balance in favour of propanone as a solvent.
That is a fantastic explanation; however I am finding it difficult to understand due to my lack of knowledge (I am only at ASLevel)
Is it basically because the ketone can form stronger bonds with the cyclohexanol?