Solubility
Hi guys my teacher said for a Solute to dissolve in a solvent the forces of attraction between the solute and solvent particles must be strong enough to overcome the solvent-solvent forces and the solute-solute forces.
the thing im confused about is that for example when ethanol dissolves in water they form a hydrogen bond. so according the rule I stated earlier this forces has to be greater the intermolecular forces in both ethanol and water but doesn't ethanol have a hydrogen bond and London forces. so wouldn't the forces in ethanol be stronger than than the hydrogen bond between the water and the ethanol
thank you
the thing im confused about is that for example when ethanol dissolves in water they form a hydrogen bond. so according the rule I stated earlier this forces has to be greater the intermolecular forces in both ethanol and water but doesn't ethanol have a hydrogen bond and London forces. so wouldn't the forces in ethanol be stronger than than the hydrogen bond between the water and the ethanol
thank you
Reply 1
Original post
by aghast-groundHi guys my teacher said for a Solute to dissolve in a solvent the forces of attraction between the solute and solvent particles must be strong enough to overcome the solvent-solvent forces and the solute-solute forces.
the thing im confused about is that for example when ethanol dissolves in water they form a hydrogen bond. so according the rule I stated earlier this forces has to be greater the intermolecular forces in both ethanol and water but doesn't ethanol have a hydrogen bond and London forces. so wouldn't the forces in ethanol be stronger than than the hydrogen bond between the water and the ethanol
thank you
the thing im confused about is that for example when ethanol dissolves in water they form a hydrogen bond. so according the rule I stated earlier this forces has to be greater the intermolecular forces in both ethanol and water but doesn't ethanol have a hydrogen bond and London forces. so wouldn't the forces in ethanol be stronger than than the hydrogen bond between the water and the ethanol
thank you
yes but a water molecule has polar bonds as oxygen is the second most electronegativity element meaning its covalent + intermolecular bonds are really strong ! hope this helps !
Reply 2
but isn't the bonding between ethanol and water hydrogen bonding. so doesn't that bond need to be greater than that the intermolecular forces in water
Reply 3
Original post
by aghast-groundHi guys my teacher said for a Solute to dissolve in a solvent the forces of attraction between the solute and solvent particles must be strong enough to overcome the solvent-solvent forces and the solute-solute forces.
the thing im confused about is that for example when ethanol dissolves in water they form a hydrogen bond. so according the rule I stated earlier this forces has to be greater the intermolecular forces in both ethanol and water but doesn't ethanol have a hydrogen bond and London forces. so wouldn't the forces in ethanol be stronger than than the hydrogen bond between the water and the ethanol
thank you
the thing im confused about is that for example when ethanol dissolves in water they form a hydrogen bond. so according the rule I stated earlier this forces has to be greater the intermolecular forces in both ethanol and water but doesn't ethanol have a hydrogen bond and London forces. so wouldn't the forces in ethanol be stronger than than the hydrogen bond between the water and the ethanol
thank you
Ethanol dissolves in water mainly due to the formation of hydrogen bonds between the hydroxyl group of ethanol and water molecules. The strong OH group of ethanol forms hydrogen bonds with the O atom in water molecules, while water molecules also form hydrogen bonds with each other. London dispersion forces, a weaker intermolecular force, exist in all molecules, including ethanol. Hydrogen bonds and London dispersion forces hold ethanol molecules together, whereas the high polarity of water results in stronger hydrogen bonds holding water molecules together.
This difference is due to the much higher polarity of water compared to ethanol. For ethanol to dissolve in water, the hydrogen bonds formed between ethanol and water must be strong enough to outweigh the hydrogen bonds between water molecules. This interaction allows the mixture to become homogeneous.
Bye,
Sandro
Reply 4
Original post
by NitrotolueneEthanol dissolves in water mainly due to the formation of hydrogen bonds between the hydroxyl group of ethanol and water molecules. The strong OH group of ethanol forms hydrogen bonds with the O atom in water molecules, while water molecules also form hydrogen bonds with each other. London dispersion forces, a weaker intermolecular force, exist in all molecules, including ethanol. Hydrogen bonds and London dispersion forces hold ethanol molecules together, whereas the high polarity of water results in stronger hydrogen bonds holding water molecules together.
This difference is due to the much higher polarity of water compared to ethanol. For ethanol to dissolve in water, the hydrogen bonds formed between ethanol and water must be strong enough to outweigh the hydrogen bonds between water molecules. This interaction allows the mixture to become homogeneous.
Bye,
Sandro
This difference is due to the much higher polarity of water compared to ethanol. For ethanol to dissolve in water, the hydrogen bonds formed between ethanol and water must be strong enough to outweigh the hydrogen bonds between water molecules. This interaction allows the mixture to become homogeneous.
Bye,
Sandro
bro def pulled this straight out of chatgpt, but says the same thing i said water molecules have polar bonds which are stronger
Reply 5
20
Original post
by aghast-groundHi guys my teacher said for a Solute to dissolve in a solvent the forces of attraction between the solute and solvent particles must be strong enough to overcome the solvent-solvent forces and the solute-solute forces.
the thing im confused about is that for example when ethanol dissolves in water they form a hydrogen bond. so according the rule I stated earlier this forces has to be greater the intermolecular forces in both ethanol and water but doesn't ethanol have a hydrogen bond and London forces. so wouldn't the forces in ethanol be stronger than than the hydrogen bond between the water and the ethanol
thank you
the thing im confused about is that for example when ethanol dissolves in water they form a hydrogen bond. so according the rule I stated earlier this forces has to be greater the intermolecular forces in both ethanol and water but doesn't ethanol have a hydrogen bond and London forces. so wouldn't the forces in ethanol be stronger than than the hydrogen bond between the water and the ethanol
thank you
The strength of the forces broken and forces that replace them are roughly the same.
Entropy increases, hence it happens.
Quick Reply
Related discussions
- chem question Kc
- OCR A A level biology question
- chem question help please
- University Project Inquiry: SR9009 Bioavailability and Formulation Optimizat
- OCR A level Geology Help
- OCR A A Level Biology
- Ccea chemistry triple award gcse
- A2 Organic Question
- please help! oxidation of alcohols practical mishap
- A level biology MCQ
- A-level Biology Essay Question
- chemistry question help please Kpc
- Wjec AS chemistry unit 1
- A level revision songs
- Edexcel GCSE Chemistry Paper 1 (Higher) - 19th May 2025 [Exam Chat]
- Entry requirements for Geology courses
- Chemistry Qs
- SQA National 5 Chemistry -1st May 2025 [Exam Chat]
- using tollens reagent on an alcohol
- Titration titre volume question
Latest
Trending
Last reply 3 weeks ago
AQA A level chemistry synthetic routes map - what is the best one to memorise?Last reply 4 months ago
AQA Chemistry Electrode Potentials Conventional Representation QuestionLast reply 6 months ago
OCR B Salters A Level Chemistry 2025 Advanced ArticleLast reply 7 months ago
Help with this chemistry question? (A2, acid-base equilibria)How The Student Room is moderated
To keep The Student Room safe for everyone, we moderate posts that are added to the site.
