# Problem: What is the pH of 0.25 M ethanolamine, HOCH2CH2NH2, (Kb=3.2x10-5)?

###### FREE Expert Solution

HOCH2CH2NH2(aq) + H2O(l)  HOCH2CH2NH3+(aq) + OH(aq); Kb = 3.2 × 10–5

Step 1Construct an ICE table.

The Kb expression for HOCH2CH2NH2 is:

$\overline{){{\mathbf{K}}}_{{\mathbf{b}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactant}}{\mathbf{=}}\frac{\mathbf{\left[}{\mathbf{HOCH}}_{\mathbf{2}}{\mathbf{CH}}_{\mathbf{2}}{{\mathbf{NH}}_{\mathbf{3}}}^{\mathbf{+}}\mathbf{\right]}\mathbf{\left[}{\mathbf{OH}}^{\mathbf{-}}\mathbf{\right]}}{\left[{\mathrm{HOCH}}_{2}{\mathrm{CH}}_{2}{\mathrm{NH}}_{2}\right]}}$

###### Problem Details

What is the pH of 0.25 M ethanolamine, HOCH2CH2NH2, (Kb=3.2x10-5)?

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 Weak Bases concept. If you need more Weak Bases practice, you can also practice Weak Bases practice problems.

What professor is this problem relevant for?

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

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.