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

Trimethylamine, (CH_{3})_{3}N, is a weak base (Kb = 6.4 × 10^{–5}) that hydrolyzes by the following

equilibrium: (CH_{3})_{3}N + H_{2}O → (CH_{3})_{3}NH^{+} + OH^{–}

What is the pH of a 0.1 M solution of (CH _{3})_{3}NH^{+}? (Enter pH to 2 decimal places; hundredth's.)

For this problem, we know that **Trimethylamine, (CH _{3})_{3}N**, is a

**(CH _{3})_{3}N + H_{2}O → (CH_{3})_{3}NH^{+} + OH^{–}**

We need to do these steps to **solve for the pH** of a 0.1 M solution of (CH_{3})_{3}NH^{+}

1. Write the equilibrium expression for **(CH _{3})_{3}NH^{+} in H_{2}O**

2. Make an ICE chart to **solve for [H _{3}O^{+}]** (in M or moles/L) at equilibrium

- Find K
_{a}given K_{b} - Recall that: $\overline{){{K}}_{{a}}{}{\times}{}{{K}}_{{b}}{}{=}{}{{K}}_{{w}}}$

3. Solve for pH

Recall that pH is given by the equation:

$\overline{){\mathbf{pH}}{\mathbf{}}{\mathbf{=}}{\mathbf{-}}{\mathbf{log}}\left[{\mathbf{H}}_{\mathbf{3}}{\mathbf{O}}^{\mathbf{+}}\right]}$

pH and pOH