ChemistryWiki | RecentChanges | Preferences
1. Compare the pH of the weak acid solution and the acid buffer solution. Explain why the pH has changed between the two solutions.
2. Draw a picture of beaker including what the different species that are in the acid buffer solution. Make sure to show water molecule. Use the size of your symbols of the species to indicate its concentration (Molarity) in the solution.
3. How did the pH change after you added the first two drops of sodium hydroxide into the acid buffer solution? Explain what happens.
4. Write the chemical reaction that happened when you added the sodium hydroxide into your acid buffer.
5a. How many drops did it take so that the pH changed significantly. What was the pH before you added this drop and after.
5b. Explain why the pH changed so much when you added that drop into your solution.
6. Does the Equivalence point of the solution have anything to or was "passed through" as you were dropping the sodium hydroxide into your acid buffer solution. Explain.
7a. If you added HCl into your original acid buffer solution, how would the pH change?
7b. Write the chemical reaction that occurred when you added in the HCl.
8a. If you have ammonia (NH3) that is a weak base, give me the chemical formula of a salt with its conjugate base in it. Make sure that you write the chemical formula of a salt that will create a basic buffer if you added the salt to the ammonia solution.
8b. Answer the same questions as in Question 2 for an acid buffer but how do it for a base buffer (using information from Question 8a).