Solubility of Organic Compounds

The video tutorial explores the solubility of different molecules in water, focusing on the concept of polarity. It examines C2H6, butanol, hexanoic acid, and methanol, explaining why methanol is the most soluble due to its small size and polar nature. The tutorial emphasizes the principle that 'like dissolves like,' highlighting the role of hydrogen bonding and molecular structure in solubility.

What is the primary factor that determines the solubility of a molecule in water?

• Color

• Polarity

• Molecular weight

• Density

Why is C2H6 not soluble in water?

• It is too large

• It reacts with water

• It is non-polar

• It is too heavy

What type of intermolecular forces are present in non-polar compounds like C2H6?

• Covalent bonds

• London dispersion forces

• Ionic bonds

• Hydrogen bonds

What makes butanol potentially soluble in water?

• Its small size

• Its hydroxyl group

• Its density

• Its color

How does the length of the carbon chain affect the solubility of alcohols in water?

• Makes them non-polar

• Has no effect

• Decreases solubility

• Increases solubility

What is the effect of the hydroxyl group on the solubility of alcohols?

• Has no effect

• Decreases solubility

• Increases solubility

• Makes them non-polar

What is the main reason hexanoic acid might not be fully soluble in water?

• Its polar nature

• Its long carbon chain

• Its small size

• Its high density

Which compound is most soluble in water?

• C2H6

• Butanol

• Hexanoic acid

• Methanol

Why is methanol more soluble in water compared to butanol?

• It has a longer carbon chain

• It is heavier

• It has a shorter carbon chain

• It is non-polar

What type of bond is primarily responsible for the solubility of methanol in water?

• Covalent bond

• Ionic bond

• Metallic bond

• Hydrogen bond