el34
09-16-2013, 10:47 PM
Like many others I've used muriatic acid (hydrochloric acid) to test for zinc. You hear "if the acid makes it bubble, you got zinc!".
But zinc isn't the only metal that reacts. Actually lead does too, but not much. From http://au.answers.yahoo.com/question/index?qid=20100311034531AAxxxwG -
For a metal to react with an acid to form a salt and hydrogen gas, it has to be above hydrogen in the electrochemical series (ECS).
The Electrochemical Series is a list of elements in order of their reactivity (high to low).
The list is as follows: Potassium(most reactive), Sodium, Calcium, Magnesium, Aluminium, Zinc, Carbon, Iron, Tin, Hydrogen, Lead, Copper, Silver, gold(least reactive)In your experiment, the Magnesium reacted most vigorously hence producing a lot of Hydrogen gas, which when lit with a glowing splint burned with a pop.
Mg + 2HCl ------------------->MgCl2 + H2
Zinc should also have produced hydrogen gas quickly, however not as quickly or vigorously as Magnesium. Maybe a smaller amount of zinc was used in the experiment - hence the proportion of Hydrogen gas produced would be less.
Zn + 2HCl --------------------> ZnCl2 + H2
Aluminium should also produce hydrogen gas when reacted with HCl acid, however the aluminium may have been coated in Aluminium Oxide (due to corrosion with oxygen in the air).
This coating has to be dissolved by the Hydrochloric Acid before the main reaction proceeds.
So the reaction takes longer to start but when it does it will produce Hydrogen gas.
To dissolve the Al2O3 (aluminium oxide coating the aluminium metal)
Al2O3 + 6HCl---------------------------> 2AlCl3 + 3H2O
The main reaction then is:
2Al + 6HCl -----------------------> 2AlCl3 + 3H2
Finally Copper will not react with Hydrochloric Acid to produce Hydrogen gas as it is below Hydrogen in the Electrochemical Series.
But zinc isn't the only metal that reacts. Actually lead does too, but not much. From http://au.answers.yahoo.com/question/index?qid=20100311034531AAxxxwG -
For a metal to react with an acid to form a salt and hydrogen gas, it has to be above hydrogen in the electrochemical series (ECS).
The Electrochemical Series is a list of elements in order of their reactivity (high to low).
The list is as follows: Potassium(most reactive), Sodium, Calcium, Magnesium, Aluminium, Zinc, Carbon, Iron, Tin, Hydrogen, Lead, Copper, Silver, gold(least reactive)In your experiment, the Magnesium reacted most vigorously hence producing a lot of Hydrogen gas, which when lit with a glowing splint burned with a pop.
Mg + 2HCl ------------------->MgCl2 + H2
Zinc should also have produced hydrogen gas quickly, however not as quickly or vigorously as Magnesium. Maybe a smaller amount of zinc was used in the experiment - hence the proportion of Hydrogen gas produced would be less.
Zn + 2HCl --------------------> ZnCl2 + H2
Aluminium should also produce hydrogen gas when reacted with HCl acid, however the aluminium may have been coated in Aluminium Oxide (due to corrosion with oxygen in the air).
This coating has to be dissolved by the Hydrochloric Acid before the main reaction proceeds.
So the reaction takes longer to start but when it does it will produce Hydrogen gas.
To dissolve the Al2O3 (aluminium oxide coating the aluminium metal)
Al2O3 + 6HCl---------------------------> 2AlCl3 + 3H2O
The main reaction then is:
2Al + 6HCl -----------------------> 2AlCl3 + 3H2
Finally Copper will not react with Hydrochloric Acid to produce Hydrogen gas as it is below Hydrogen in the Electrochemical Series.