Four isomeric alcohols are possible for molecular formula C4H10O.
Which of the following statement is true for given compounds?
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Boiling point depends on molecular weight and intermolecular hydrogen bonding. All four isomers have same molecular weight (C4H10O), so hydrogen bonding capability becomes the key factor.
Primary alcohols (a, b, c) have stronger hydrogen bonding than secondary alcohol (d). Among primary alcohols, branching reduces surface area and weakens intermolecular forces. Compound c (1-butanol) is linear and has the strongest intermolecular forces, followed by slightly branched b (2-methyl-1-propanol), then more branched a (2-methyl-2-propanol).
Therefore, boiling point order is c > b > a > d. Solubility decreases with increasing carbon chain length, so d (secondary butanol) is more soluble than c (primary butanol).
Final answer: Boiling point of b > a is true.