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Questions and Answers
What is the reaction between hydrogen and chlorine gas and what acid is produced?
What is the reaction between hydrogen and chlorine gas and what acid is produced?
The reaction is H2 + Cl2 -> 2HCl, producing hydrochloric acid.
Describe the process through which acidic oxides can form an acid when combined with water.
Describe the process through which acidic oxides can form an acid when combined with water.
Acidic oxides react with water to form an acid, such as CO2 + H2O -> H2CO3, resulting in carbonic acid.
What happens when a non-volatile acid is heated with a salt of a more volatile acid?
What happens when a non-volatile acid is heated with a salt of a more volatile acid?
The non-volatile acid displaces the volatile acid, resulting in the formation of a new acid and salt.
What is produced when sulfur is oxidized by concentrated nitric acid?
What is produced when sulfur is oxidized by concentrated nitric acid?
How are basic oxides formed from metals through their reaction with oxygen?
How are basic oxides formed from metals through their reaction with oxygen?
Explain how basic oxides produce alkalis when dissolved in water.
Explain how basic oxides produce alkalis when dissolved in water.
What occurs in a reaction between a salt solution and a strong base?
What occurs in a reaction between a salt solution and a strong base?
What kind of reactions result in the formation of basic oxides via salt decomposition?
What kind of reactions result in the formation of basic oxides via salt decomposition?
What is the role of active metals in the formation of bases when they react with water?
What is the role of active metals in the formation of bases when they react with water?
Can neutral oxides like CO and NO produce acids when reacting with water? Why or why not?
Can neutral oxides like CO and NO produce acids when reacting with water? Why or why not?
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Study Notes
Acids
Acids from Non-metals
- Non-metal and hydrogen reaction produces an acid.
- Example reactions:
- Hydrogen + Chlorine → Hydrochloric acid (H2 + Cl2 → 2HCl)
- Hydrogen + Iodine → Hydroiodic acid (H2 + I2 → 2HI)
Acids from Acidic Oxides
- Acidic oxides react with water to form acids.
- Example reactions:
- Carbon dioxide + Water → Carbonic acid (CO2 + H2O → H2CO3)
- Sulfur dioxide + Water → Sulfurous acid (SO2 + H2O → H2SO3)
- Sulfur trioxide + Water → Sulfuric acid (SO3 + H2O → H2SO4)
- Diphosphorus pentoxide + Water → Phosphoric acid (P2O5 + 3H2O → 2H3PO4)
- Neutral oxides such as carbon monoxide (CO) and nitric oxide (NO) do not form acids when reacted with water.
Acids from Salts
- Heating non-volatile acids with salts of more volatile acids releases a volatile acid.
- Example reactions:
- Potassium nitrate + Concentrated sulfuric acid → Potassium hydrogen sulfate + Nitric acid (KNO3 + H2SO4 < 200°C → KHSO4 + HNO3)
- Sodium chloride + Concentrated sulfuric acid → Sodium hydrogen sulfate + Hydrochloric acid (NaCl + H2SO4 < 200°C → NaHSO4 + HCl)
Acids by Oxidation of Non-metals
- Non-metals can be oxidized to form acids.
- Example reaction:
- Sulfur + Nitric acid → Sulfuric acid + Water + Nitrogen dioxide (S + 6HNO3 → H2SO4 + 2H2O + 6NO2)
Bases [Oxides/Hydroxides]
Bases from Metals
- Metals react with oxygen to form basic oxides.
- Example reactions:
- Sodium + Oxygen → Sodium oxide (4Na + O2 → 2Na2O)
- Magnesium + Oxygen → Magnesium oxide (2Mg + O2 → 2MgO)
Bases from Basic Oxides
-
Soluble basic oxides react with water to form alkalies.
-
Example reactions:
- Potassium oxide + Water → Potassium hydroxide (K2O + H2O → 2KOH)
- Sodium oxide + Water → Sodium hydroxide (Na2O + H2O → 2NaOH)
-
Highly reactive metals can also react with water:
- Potassium + Water → Potassium hydroxide + Hydrogen (2K + 2H2O → 2KOH + H2)
- Sodium + Water → Sodium hydroxide + Hydrogen (2Na + 2H2O → 2NaOH + H2)
Bases from Salts
- Mixing salts with strong bases results in the precipitation of hydroxides.
- Example reactions:
- Aluminum chloride + Sodium hydroxide → Sodium chloride + Aluminum hydroxide precipitate (AlCl3 + 3NaOH → 3NaCl + Al(OH)3↓)
- Iron(II) sulfate + Sodium hydroxide → Sodium sulfate + Iron(II) hydroxide precipitate (FeSO4 + 2NaOH → Na2SO4 + Fe(OH)2↓)
Bases by Decomposition of Salts
- Heating certain carbonates or nitrates produces basic oxides.
- Example reaction:
- Lead(II) nitrate decomposes to lead oxide, nitrogen dioxide, and oxygen (2Pb(NO3)2 → 2PbO + 4NO2 + O2)
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