Name: _____________________________
Properties of Acids and Bases
Introduction: In an aqueous solution, an acid yields an H+ ion. Bases yield an OH- ion. But what other
properties do they have? Acids react with metals in a single replacement reaction:
M(s) + 2H3O+  M2+ + H2(g) + 2H2O(l)
Also acids react with a carbonate:
CO32- + 2H3O+  CO2(g) + 3H2O(l)
A neutralization reaction can occur between an acid and a base to form salt and water. In this lab we will
observe those reactions as well as test their acidity and pH.
Purpose: To determine the properties of acids and bases.
Pre-Lab:
1. Create a data table for results found in step one and two.
2. Identify HCl, HC2H3O2, and NaOH as an acid or base and explain.
3. When is phenolphthalein colorless? When is it pink?
4. Write a balanced double replacement equation for the reaction of HCl and CaCO3.
5. Write a balance reaction for the reaction of HCl and NaOH.
6. What type of reaction occurs between HCl and NaOH?
Materials: test tubes and rack, pipettes, spatula, spot plate, splint, 6M HCl, 6M HC2H3O2, 0.5M NaOH, 1M
NaOH, phenolphthalein, litmus paper, pH paper, zinc, magnesium, copper, CaCO3.
Procedure:
1. Test each solution at this lab station with red and blue litmus paper and pH paper. Then decide if they
are acids or bases. Record the substance name and results.
Substance
Red litmus
Blue litmus
pH paper
Acid or Base?
2. Repeat procedure one with a new set of substances.
Substance
Red litmus
Blue litmus
pH paper
Acid or Base?
3. Add about five drops of each of the following to separate depressions on a spot plate: 0.5M NaOH, 6M
HCl, and 6M HC2H3O2. Test them all with litmus paper, pH paper and finally phenolphthalein. Record
your observations. Clean and dry your spot plate.
Substances
0.5M NaOH
6M HCl
6M HC2H3O2
Red litmus
Blue litmus
pH paper
phenolphthalein
4. Add small pieces of Zn, Mg, Cu and Fe to separate depressions on your plate. Add a few drops of 6M
HCl to each depression. Observe and record their reactivity. Scale their reactivity 0 (not reactive) to 4
(most reactive). Clean and dry your spot plate.
Metals
Zn
Mg
Cu
Fe
Observations
Reactivity
5. Repeat procedure four with 6M HC2H3O2 in place of HCl. Record the reactivity and compare to HCl.
Clean and dry your spot plate.
Metals
Zn
Mg
Cu
Fe
Observations
Reactivity
6. Place a small amount of CaCO3 to a test tube. Then add a few drops of HCl. Record your observations.
Clean and dry your test tube.
Observations: ______________________________________________________________________
7. Add about 10 drops of 6M HCL to a clean, dry test tube. Also add one drop of phenolphthalein. To the
same test tube, add 0.5 M NaOH slowly, drop by drop, while swirling until the solution turns pink.
Count how many drops you needed to add. Test it with pH paper and record.
Drops needed: ________
pH: _______
Observations: _______________________________________________________________________
Questions:
1. What properties do all household acids have in common?
2. What properties do all household bases have in common?
3. Write a balanced reaction for HCl reacting with each metal that reacted.
4. Explain why the HCl reacted more vigorously than the HC2H3O2.
5. Using the full reaction for HCl reacting with CaCO3 in prelab 4, explain your observations for this
reaction.
6. Explain why more drops of NaOH were needed than drops of HCl in steps 7 and 8.
7. Explain why the reaction between the acid and the base is called a neutralization reaction in terms of pH
values.