Do you expect acetaminophen to be soluble in 1.0 M NaOH? why or why not?
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To determine whether acetaminophen (C8H9NO2) is soluble in 1.0 M NaOH (sodium hydroxide), we need to consider the chemical properties of both substances.
Acetaminophen is a polar organic compound, characterized by having both polar and nonpolar functional groups. It has hydrogen bonding capabilities due to the presence of hydroxyl (-OH) and amine (-NH) groups. Acetaminophen is generally soluble in polar solvents like water or ethanol.
On the other hand, sodium hydroxide (NaOH) is a strong base and a highly ionic compound. It dissociates completely in water to form sodium ions (Na+) and hydroxide ions (OH-). Sodium hydroxide is highly soluble in water but is not soluble in most organic solvents.
Based on their respective properties, we can predict that acetaminophen is not likely to be soluble in 1.0 M NaOH. This is because NaOH is an inorganic, highly ionic compound that does not possess the necessary molecular interactions (like hydrogen bonding) to dissolve acetaminophen.
To confirm this prediction, experimental testing or reference to solubility data for acetaminophen and NaOH could be helpful. Such data can indicate the extent of solubility or lack thereof and provide more precise information.