# Problem: The pH of a 1.00 M solution of urea, a weak organic base, is 7.050.Calculate the Ka of protonated urea.

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###### FREE Expert Solution

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.

###### Problem Details

The pH of a 1.00 M solution of urea, a weak organic base, is 7.050.

Calculate the Ka of protonated urea.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Ka and Kb concept. You can view video lessons to learn Ka and Kb. Or if you need more Ka and Kb practice, you can also practice Ka and Kb practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Murray's class at UF.