Experiment: Acids and Metals
Aim: To determine the product of an acid and metal reaction.
Equipment:
- 1M Hydrochloric acid (in
dropper bottle)
- Vinegar
- 6 test tubes
- Test tube rack
-
Distilled water (in wash bottle)
Magnesium, Iron, Zinc
Stoppers
Matches
Safety glasses
Method:
1. Place six test-tubes in the test-tube rack.
2. Add a 2–3 cm depth of 0.1M hydrochloric acid to the first three tubes, and a
2–3 cm depth of vinegar to the remaining three tubes.
3. Add a small piece of a different metal to each of the tubes with hydrochloric
acid in them. Record which metal you add to each tube.
4. Put a stopper in these test tubes. Do not hold the stoppers down as the glass
could break.
5. Test that hydrogen has been produced in the test tubes with Hydrochloric
Acid. Test for hydrogen: The light of a flame will ‘pop’ and go out when it is
put over the gas.
6. Add a small piece of the same metals to each of the tubes with vinegar in
them. Record which metal you add to each tube.
7. When you are done list the order of reactivity by numbering the reactions
from highest to lowest (1 - highest reactivity).
Risk Assessment:
Table 1: Risk Assessment
Potential Hazards
Standard Handling Procedures
Results: Note your observations in the table below.
Metal
Zinc
Magnesium
Iron
Table 2: Results
Observations
Hydrochloric Acid
Vinegar
Reactivity
Questions and Discussion:
What gas did the reactions produce?
How did you test for this?
What do all acids contain?
When a metal and an acid react together they make
.
SALT - a SALT is formed when the Hydrogen of an Acid is
replaced by a metal
Naming SALTS
Remember metals (except copper and some others) push out (displace)
the hydrogen of acids to make SALTS.
ACID
TYPE of SALT made
Hydrochloric acid
HCl(aq)
CHLORIDES e.g. sodium chloride
NaCl(s)
Sulphuric acid
H2SO4(aq)
SULPHATES e.g. magnesium sulphate
MgSO4(s)
Nitric acid
HNO3(aq)
NITRATES e.g. potassium nitrate
KNO3(s)
Carbonic acid
H2CO3(aq)
CARBONATES e.g. zinc carbonate
ZnCO3(s)
Phosphoric acid
H3PO4(aq)
PHOSPHATES e.g. calcium phosphate
Ca3(PO4)2(s)
So, a SALT contains:
a CATION e.g. Na+ (usually from a METAL)
And
an ANION e.g. Clfrom an ACID e.g. hydrochloric acid HCl(aq)
1. Magnesium + hydrochloric acid  magnesium chloride + hydrogen
Mg
+
2HCl

MgCl2
+ H2
+ hydrochloric acid  ……………………….. + ……………………………
2. Iron
Fe
+
HCl
 ……………………….. + ……………………………
+ hydrochloric acid  ……………………….. + ……………………………
3. Zinc
Zn
+
HCl
 ……………………….. + ……………………………
4. Aluminium + hydrochloric acid  ……………………….. + ………………………
Al
5. Tin
Sn
+
HCl
 ……………………….. + ……………………………
+ hydrochloric acid  ……………………….. + ……………………………
+
HCl
 ……………………….. + ……………………………
Homework Activity 1
Using the information in the picture below or otherwise, answer the
following questions:
1.
2.
3.
4.
5.
What is acid rain?
What causes acid rain?
Why is acid rain harmful?
What is being done to prevent it?
What can you do to prevent it?
Experiment: Acids and Carbonates
Aim: To determine the products of an acid and carbonate reaction.
Equipment:
- 4 test tubes
- Test tube rack
- Stoppers
- Small beaker (100mL)
- Limewater
- Sodium carbonate
- Ammonium carbonate
-
Calcium Carbonate
Spatula
1M hydrochloric acid
Vinegar
Matches
Safety glasses
Method:
1. Add a small amount of each solid (about the tip of a spatula full) to two
different test tubes.
2. Add 2 cm of hydrochloric acid to the first tube and quickly stopper. Remove
the stopper and add a small amount of limewater.
3. Repeat steps 1–2 using vinegar instead of HCl
Risk Assessment:
Table 1: Risk Assessment
Potential Hazards
Standard Handling Procedures
Results: Note your observations in the table below.
Table 2: Results
Reactivity
Observations
Metal
Hydrochloric Acid
Sodium
Carbonate
Ammonium
Carbonate
Calcium
Carbonate
Vinegar
Questions
1. What products were formed during the reactions?
2. How did you test for these products?
3. Write out word equations to describe the chemical reactions you have
observed. If possible also write out formula equations.
4. What effects can Carbon Dioxide have on the environment?
5. Homework Activity 2
When Carbon dioxide is dissolved in water it forms a weak carbonic acid.
This is common in our waterways. What is the effect of carbonic acid on our
environment? You may use the internet to help you answer this question.
Experiment: Acids and Bases (Neutralisation)
Aim: To investigate the neutralization of an acid by a base.
Equipment:
- 50mL measuring cylinder
- 1M hydrochloric acid
- 1M sodium hydroxide
-
Universal indicator
Pasteur pipette
Safety glasses
Method:
1. Pour 25 ml of 1 M hydrochloric acid into the beaker.
2. Measure the pH using universal indicator.
3. Add 5 mL of 1 M sodium hydroxide.
4. Re-measure the pH of the solution in the beaker.
5. Repeat steps 3 and 4 until you have added 35 mL of the sodium hydroxide
solution.
Risk Assessment:
Table 1: Risk Assessment
Potential Hazards
Standard Handling Procedures
Results: Note your observations in the table below.
Volume of
Hydrochloric Acid
Table 2: Results
Volume of Sodium
Hydroxide
25mL
0mL
25mL
5mL
25mL
10mL
25mL
15mL
25mL
20mL
25mL
25mL
25mL
30mL
25mL
25mL
Colour
pH Range
Questions
1. At which point was the solution neutral. Why?
2. Construct the word equations to describe the reaction. Also complete a
formula equation if possible.
3. Does adding the same amount of base to an acid always neutralize the acid?
Explain why?