I NEED HELP PLEASE, THANKS! Ammonia (NH3) is an example of a Brønsted-Lowry Base.
-Define the Brønsted-Lowry acid-base theory.
-What is the pH of an ammonia solution that has a concentration of 0.335 M? The Kb of ammonia is 1.8 × 10^–5.

Here's what I get.

Explanation:

1. Brønsted-Lowry theory

An acid is a substance that can donate a proton to another substance.

A  base is a substance that can accept a proton from another substance.

2. pH of ammonia

The chemical equation is

For simplicity, let's re-write this as

(a) Set up an ICE table.

                     B + H₂O ⇌ BH⁺ + OH⁻

I/mol·L⁻¹:     0.335             0        0

C/mol·L⁻¹:       -x                +x       +x

E/mol·L⁻¹:  0.335 + x          x         x

Check for negligibility:

(b) Solve for [OH⁻]

(c) Calculate the pOH

(d) Calculate the pH

pH = 14.00 - pOH = 14.00 - 2.61 = 11.39

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