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Wiki User
∙ 11y ago
Benzene (C6H6) is minimally soluble in water due to its nonpolar nature, whereas water is polar. This makes it difficult for benzene molecules to interact with water molecules, limiting its solubility in water.
Wiki User
∙ 11y agoNo. because it is non polar
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Do KCl and C6H6 dissolve in each other?
No, KCl (potassium chloride) and C6H6 (benzene) would not readily dissolve in each other because they are not soluble in each other due to differences in their polarities. KCl is an ionic compound that is soluble in water, while benzene is a nonpolar solvent that is not miscible with water or ionic compounds like KCl.
C6H6 C2H5OH CH3CH2CH2OH CH3-O-CH3 Which compound has more repulsion with water and why?
C6H6 will be repelled the most. C2H5OH and CH3CH2CH2OH are both alcohols, both are polar molecules and will easily dissolve in water.CH3OCH3 is dimethyl ether and will repel water, though it is slightly polar.C6H6 or benzene will be repelled by water the most, as benzene is non polar and water is polar.
Why are NaI and CH2O more soluble in water than benzene (C6H6)?
NaI is soluble in water due to ion-dipole interactions, where the ionic Na+ and I- interact with the polar water molecules. CH2O is soluble in water due to hydrogen bonding with water molecules. On the other hand, benzene is nonpolar and does not interact favorably with polar water molecules, leading to poor solubility in water.
Has the molecular formula C6H6?
Benzene has the molecular formula C6H6.
Will sand dissolve in boiling water?
No, sand will not dissolve in boiling water as it is insoluble in water. Sand is made of large particles of silicon dioxide which do not break down or dissolve in water at any temperature.
Do KCl and C6H6 dissolve in each other?
No, KCl (potassium chloride) and C6H6 (benzene) would not readily dissolve in each other because they are not soluble in each other due to differences in their polarities. KCl is an ionic compound that is soluble in water, while benzene is a nonpolar solvent that is not miscible with water or ionic compounds like KCl.
What compounds each as a liquid would be expected to be the best solvent for carbon disulfide nh3 ch3oh h2o c6h6 or hbr?
Carbon disulfide (CS2) would be best dissolved by carbon tetrachloride (CCl4) due to its nonpolar nature similar to CS2, NH3 would dissolve in water (H2O) due to their ability to form hydrogen bonds, CH3OH would dissolve in water due to their similar polar nature and ability to form hydrogen bonds, C6H6 (benzene) would dissolve in HBr due to their ability to form temporary dipoles and induce dipole-dipole interactions.
Why are NaI and CH2O more soluble in water than benzene (C6H6)?
NaI is soluble in water due to ion-dipole interactions, where the ionic Na+ and I- interact with the polar water molecules. CH2O is soluble in water due to hydrogen bonding with water molecules. On the other hand, benzene is nonpolar and does not interact favorably with polar water molecules, leading to poor solubility in water.
C6H6 C2H5OH CH3CH2CH2OH CH3-O-CH3 Which compound has more repulsion with water and why?
C6H6 will be repelled the most. C2H5OH and CH3CH2CH2OH are both alcohols, both are polar molecules and will easily dissolve in water.CH3OCH3 is dimethyl ether and will repel water, though it is slightly polar.C6H6 or benzene will be repelled by water the most, as benzene is non polar and water is polar.
Is c6h6 a hydrocarbon?
C6H6 is this a hydrocarbon
What is the chemical formula for benzen?
Formula: C6H6
A substance that does not dissolve in a solvent is said to be what in that solvent?
- Sand does not dissolve in water- Plastic does not dissolve in water- metals do not dissolve in water
Does water and salt dissolve?
No, but salt does dissolve in water.
Do lipids dissolve water?
No. Lipids do not dissolve in water.
Has the molecular formula C6H6?
Benzene has the molecular formula C6H6.
Does salt dissolve in tap water?
Yes it does dissolve in tap water. It can really dissolve in any water.
What are substances that dissolve in water?
Nutilite's vitamins dissolve in water.
