🤓 Based on our data, we think this question is relevant for Professor Klausmeyer's class at BAYLOR.

The pH of 0.1 M C _{4}H_{9}NH_{2}(aq) (butylamine) aqueous solution was measured to be 12.04. What is the value of p*K*_{b} of butylamine?

1. 1.96

2. 2.93

3. 2.57

4. 0.25

5. 3.50

6. 2.87

We are being asked to calculate the pK_{b} for a 0.1 M solution of C_{4}H_{9}NH_{2} (butylamine).** **

**C _{4}H_{9}NH_{2} (butylamine)** is a

We can calculate the pK_{b} of butylamine from its **K _{b}** using the following equation:

$\overline{){{\mathbf{pK}}}_{{\mathbf{b}}}{\mathbf{=}}{\mathbf{-}}{\mathbf{log}}{\mathbf{}}{{\mathbf{K}}}_{{\mathbf{b}}}}$

Since we’re dealing with a weak base and **K _{b} is an equilibrium expression **we will have to

• **C _{4}H_{9}NH_{2}** →

•

**Equilibrium reaction:** **C _{4}H_{9}NH_{2(aq)} + H_{2}O_{(l)} **

Weak Bases