Consider the table shown here, which lists the solubilities of several alcohols
ID: 479974 • Letter: C
Question
Consider the table shown here, which lists the solubilities of several alcohols in water and in hexane. Explain the observed trend in terms of intermolecular forces.
Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer.
Part A Consider the table shown here, which lists the solubilities of several alcohols in water and in hexane. Explain the observed trend in terms of intermolecular forces. Solubility in H20 Solubility in Hexane (C6H14) Alcohol Space-Filling Model (mol alcohol 100 g H20) mol alcohol 100 g C6H14) Methanol (CH30H) Miscible 0.12 Ethanol (CH3CH2OH) Miscible Miscible Miscible Miscible Propanol (CH3CH2CH20H) Miscible Butanol (CH3CH2CH2CH20H) 0.11 0.030 Miscible Pentanol OHExplanation / Answer
PART A:
The first alcohol on the list is methanol which is highly polar and forms hydrogen bonds with water. It is miscible in water and has limited solubility in hexane which is non-polar. However as the carbon chain gets longer in the series of alcohol, the OH group becomes less important relative to the growing non-polar carbon chain. Therefore, the alcohols becomes progressively less soluble in water and more soluble in hexane. This table demonstrates the rule of thumb, like dissolves like. Methanol is like water and therefore dissolves in water. It is unlike hexane and therefore has limited solubility in hexane. As you move down the list, the alcohols become increasingly like hexane and increasingly unlike water and therefore become increasingly soluble in hexane and increasingly insoluble in water.