Hexanoic acid is only slightly soluble in water but is readily soluble (with stirring and shaking) in both 0.6 M NaHCO3 and 2.5 M NaOH.

give a brief explanation of the reaction for each
please help...thanksssss

An acid + base = salt + water.

NaOH forms the Na salt as does NaHCO3.
RCOOH + HONa ==> RCOONa + HOH.

Hexanoic acid, also known as caproic acid, is a fatty acid with the molecular formula C6H12O2. It is a weak acid and has limited solubility in water. However, it can be dissolved in both sodium bicarbonate (NaHCO3) and sodium hydroxide (NaOH) solutions.

1. Solubility in 0.6 M NaHCO3:
When hexanoic acid is added to a solution of sodium bicarbonate, which is a basic solution, a reaction occurs. In this reaction, the acidic nature of hexanoic acid is neutralized by the basic sodium bicarbonate. The reaction can be represented as follows:

C6H12O2 (hexanoic acid) + NaHCO3 (sodium bicarbonate) → C6H11O2Na (sodium caproate) + H2O (water) + CO2 (carbon dioxide)

The product of this reaction, sodium caproate, is a salt that is soluble in water, which explains why hexanoic acid becomes readily soluble in 0.6 M NaHCO3 solution.

2. Solubility in 2.5 M NaOH:
Hexanoic acid is also soluble in sodium hydroxide solution due to a similar reaction that takes place. Sodium hydroxide is a strong base that can fully ionize in water and readily react with hexanoic acid. The reaction can be represented as follows:

C6H12O2 (hexanoic acid) + NaOH (sodium hydroxide) → C6H11O2Na (sodium caproate) + H2O (water)

Again, the product of this reaction is sodium caproate, which is a salt and hence soluble in water. This explains why hexanoic acid is soluble in 2.5 M NaOH solution.

By understanding the basic chemical reactions between hexanoic acid and sodium bicarbonate or sodium hydroxide solutions, we can explain why hexanoic acid is only slightly soluble in water but readily soluble in these particular alkaline solutions.