Acids and salts speed up the rate of rusting by increasing the concentration of ions, allowing more ion movement which causes iron to lose electrons faster and form iron oxide. Rusting can be prevented by applying a barrier like paint, oil, grease or electroplating between the metal and oxygen/water. Electroplating involves placing the plating metal as the anode and the metal to be plated as the cathode in an electrolyte solution. Common metals used for plating include tin, silver, nickel, chromium, zinc and gold.

5. Why does acids or salt speed up the
rate of rusting?
• With acids or salt, the concentration of ions
increases. This allows more ion movements
which will cause the iron to lose electrons
faster to form Iron(III) Oxide.
• This speeds up the rate of rusting

6. Prevention of rusting
• Rusting can be
prevented by
putting a barrier
around the metal
• Paint, oil, grease,
plastic coating and
electroplating can
be a barrier for the
metal

8. Process of electroplating
1. Put the plating metal
at the anode
2. Put the metal to be
plated at the cathode.
3. Both the plating
metal and the metal
would be placed into
the electrolyte

9. Common metals used for plating
objects
• Tin
• Silver
• Nickel
• Chromium
• Zinc
• Gold

10. • Tin is commonly used to coat food
containers
• Iron rusts faster when the tin metal coating
is damaged because iron is more reactive
than tin, therefore, the iron lose electrons
faster to form ions which cause rusting to
occur faster