Nick DiPreta
Jonny Masci
4/27/10
Pre-Lab- Acids ionize in aqueous solution and produce hydrogen ions. The strength of the acid is directly
related to how much the acid dissolved. The more ions are produced in dissolution, the stronger the
acid. Acidic and Alkalinic properties are related to the amount of hydronium and hydroxide ions
produced.
Purpose- The purpose of this lab is to observe and study typical properties and reactions of acids and
bases.
Equipment- page 183 of the lab. Exception: no glass tubing
Materials- Refer to page 184 on the lab.
Safety:
• Handle acid and base solutions with care and avoid spills
• Flush or wash any spills with water immediately
• Always wear safety goggles and lab apron while working in the lab
Procedure: Part A
Add 5 drops of 6M HCl, 6M HC₂H₃O₂ and .5 NaOH in the spot plate
Test the blue litmus, red litmus, ph paper and phenolphthalein with each depression
Clean spot plate and dry
Part B
Add Zinc, magnesium, iron copper to a depression in the spot plate
Add 6M HCl and observe the reactions
Repeat the first two steps using 6M HC₂H₃O₂
Clean and dry spot plate
Place zinc in a test tube and add 6M HCl
Invert a test tube and collect the gas and add a burning splint
Part C
Add limewater solution to a test tube
Add CaCO₃ and 6M HCl into another test tube
Use the glass tubing to insert the gas into the limewater solution and observe
Part D
Add 10 drops of 1M HCl and one drop of phenolphthalein to a test tube and test with pH paper
Count the number of drops .5 M NaOH to the acid until it changes color
Test with pH paper
Part E
Add vinegar, lemon juice, tomato juice, milk, household ammonia into each depression in a spot plate
Test each one with red litmus, blue litmus, pH paper, and phenolphthalein
Observations and DataPart A-
6M HCL
6M HC2H3O2
0.5 M NaOH
Red litmus
Turns pink
A little darker
blue
Blue Litmus
Stronger
Weaker than HCL
blue
pH paper
2
3
10
Phenolphthalein
More cloudy
Nothing
pink
Part B
Reactivity in decreasing order
The reactivity from fastest to slowest is Fe, Mg, Zn, Cu.
2. Comparative Reactivities with HCl and HC2H3O2
Zinc
Magnesium
Iron
copper
With HCL
slow
fast
Very fast
No change
With HC2H302
No change
Fast
Very slow
No change
3. Results of Burning Splint TestThe gases ignited and caused a loud popping noise as a result of the burning flame test.
Part DNumber of drops of .5 NaOH to neutralize 10 drops of 1 M HCl: 1 drop
pH of neutral solution: 7
Part E: Data Table
Red litmus
Vinegar
Turns Red
Lemon juice Turns Red
Tomato juice Turns Red
Milk
Turns Red
Ammonia
Turns Blue
Blue litmus
Turns red
Turns red
Turns red
No change
Turns Blue
pH paper
2
3
5
7
10
Phenolphthalein
No change
Turns cloudy
No change
No change
turns Dark Red
Equations
1. Write The Balanced molecular equations for the reaction of each metal with 6 M HCL
Mossy Zinc: Zn + 2 HCl  H2 + ZnCl2
Magnesium Ribbon: Mg + 2 HCl  H2 + MgCl2
Iron Filings: Fe + 2 HCl  H2 + FeCl2
Copper wire: Cu + 2 HCl  H2 + CuCl
2. Write the Balanced molecular equations for the reaction of each metal with 6 M HC2H3O2
Mossy Zinc: Zn + 2 (HC2H3O2)  Zn(C2H3O2)2 + H2
Magnesium Ribbon: Mg + 2 HC2H3O2 Mg(C2H3O2)2 + H2
Iron Filings: Fe + 2 HC2H3O2  Fe(C2H3O2)2 + H2
Copper Wire: Cu + 2 HC2H3O2  Cu(C2H3O2)2 + H2
3. CaCO3 with HCl
CaCO3 + 2 HCl  CaCl2 + H2O + CO2
4. HCl with NaOH
HCl + NaOH  H2O + NaCl
Questions1. A single replacement reaction occurs between a metal and an acid. A general equation for this type of
reaction is:
Metal+ Acid Metal ion + Water+ Hydrogen (g)
2. The rates of reaction between a metal and the different acids has to do with reactivity between the
metal and nonmetal in the acid. If the metal is more reactive than the non metal, due to the fact that
the reaction is a single replacement, it will occur faster. On the other hand, if the metal is not
significantly greater in reactivity than the other metal in the acid, than the reaction will not occur at a
fast rate.
3. The balanced reaction between CO2 gas and limewater, Ca(OH)2, is:
CO2 + Ca(OH)2  Ca(CO3) + H2O
Calcium carbonate is the name of the milky precipitate that forms.
4. For some reason, it only took one drop in our experimental data for a neutral solution in part D to be
found. However, due to the fact that the concentration of the NaOH is 0.5 M and the HCL is 1.0M one
would expect to find under standard conditions, around two times the amount of drops of NaOH to
neutralize the 10 drops of HCL.
5. Vinegar, lemon juice, and tomato juice were all acidic. Milk was close to neutral but was more acidic.
Ammonia was basic.
Conclusion: In this experiment, the properties of acids and bases were investigated. We learned about
neutralization reactions as well as learned how to tell if something was an acid or a base using
indicators.