Final answer:
In acid-base extraction, acids and bases are separated based on solubility differences. For decreasing acid strength, arrange HClO3 > H3PO4 > CH3PO3H2; for increasing base strength, arrange CF3S¯ < CH3S¯ < OH¯. Acidic and basic hydrolysis of an ester yield different products.
Step-by-step explanation:
In the context of extraction protocols in chemistry, acid-base extraction is a method to separate acids and bases present in a mixture based on their differential solubility in aqueous or organic solvents. After removal of impurities by filtration, when working with an aluminate, for example, the addition of acid can lead to the reprecipitation of aluminum hydroxide. This technique relies on the partition coefficient of a solute between two immiscible liquids, usually water, and an organic solvent.
Regarding the order of extraction in the context of Exercise 15.8.1 and Exercise 17.4.1, for decreasing acid strength, one would arrange ‘HClO3 > H3PO4 > CH3PO3H2’ as chloric acid (HClO3) is typically a stronger acid than phosphoric acid (H3PO4), which in turn is stronger compared to the phosphorous acid (CH3PO3H2). For increasing base strength, the arrangement would be ‘CF3S¯ < CH3S¯ < OH¯’, with hydroxide (OH¯) being the strongest base listed.
Hydrolysis reactions of esters under acidic or basic conditions will produce different products: acidic hydrolysis results in the formation of a carboxylic acid and an alcohol, while basic hydrolysis (also known as saponification) results in a carboxylate salt and an alcohol. Liquid-liquid extractions are pivotal in the isolation and purification of these reaction products.