1. Outline a procedure to prepare an ammonia/ammonium buffer solution.
I'm confused how to start it off.
This is an outline of how the steps should be:
Step One - Calculate the concentration of hydronium ions in the solution that requires buffering. You can determine this concentration from the pH of the solution.
Use the formula: [H3O+(aq)]=10−pH
Step Two - Using the Table of Relative Strengths of Acids and Bases, choose the weak acid that has a Ka closest to the hydronium ion concentration of the solution that requires buffering.
Step Three - Mix equal quantities of the weak acid and its conjugate base (salt). Buffers work best if the ratio of weak acid to conjugate base is 1:1. An ideal buffer contains these two entities in equal concentration.
How would I write the steps using the ammonia/ammonium buffer solution given above?
Choices: True,False. Select all that are True. The pH at the equivalence point of a weak base with a strong acid is expected to be less than 7 because of the presentce of the conjugated acid in the water. One cannot prepare a
TRUE OR FALSE? 1) A solution that is made out of 1.00mol/L ammonia and 0.50mol/L of ammonium chloride is a basic buffer. 2) The pH at the equivalence point of a weak base with a strong acid is expected to be less than 7 because
1.)An ammonia/ammonium buffer solution contains 0.35 M NH3 and 0.72 M NH4+. The Kb value of ammonia is 1.8×10−5. Calculate the pH of this buffer. 2.) Nitrous acid has a Ka of 4.5×10−4. What is the pH of a buffer solution