🤓 Based on our data, we think this question is relevant for Professor Murray's class at UF.
We’re being asked to calculate the Ka of protonated urea (The pH of 1.00 M urea, a weak organic base is 7.050).
Urea ((NH2)2CO) is a weak base.
Remember that weak bases partially dissociate in water and that bases accept H+ from the acid (water in this case).
The dissociation of Urea is as follows:
(NH2)2CO (aq) + H2O(l) ⇌ (NH2)2COH+ (aq) + OH-(aq)
From this, we can construct an ICE table.
Remember that liquids are ignored in the ICE table.
Kb expression for (NH2)2CO is:
Liquids are ignored in the Kb expression.
Note that each concentration is raised by the stoichiometric coefficient: [(NH2)2CO], [OH–] and [(NH2)2COH+] are raised to 1.
The pH of a 1.00 M solution of urea, a weak organic base, is 7.050.
Calculate the Ka of protonated urea.