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Acids Reactions with Metal carbonates and Hydrogen Carbonates

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Reactions of Acids with Metal Carbonates and HCO3-

Acids react with metal carbonates and hydrogen carbonates to produce/evolve carbon(IV)oxide gas, water and a salt.
For a monovalent metal:
M2CO3(s)+ 2H+(aq) → 2M+(aq) + H2O (l)+ CO2(g)
MHCO3(s)+ H+(aq) → M+(aq) + H2O (l)+ CO2(g)
For a divalent metal:
MCO3(s)+ 2H+(aq) → M2+(aq) + H2O (l)+ CO2(g)
M(HCO3)2(aq)+2H+(aq) →M2+(aq)+2H2O(l)+2CO2(g)
Examples:
For a monovalent metal:
K2CO3(s)+ 2H+(aq) → 2K+(aq) + H2O (l)+ CO2(g)
NH4HCO3(s)+ H+(aq) → NH4+(aq) + H2O (l)+ CO2(g)
For a divalent metal:
ZnCO3(s)+ 2H+(aq) → Zn2+(aq) + H2O (l)+ CO2(g)
Mg(HCO3) 2(aq)+2H+(aq) →Mg2+(aq)+2H2O(l)+2CO2(g)

Acids neutralize metal oxides/hydroxides to salt and water only. i.e.
Ionically:
For a monovalent metal:
M2O(s) + 2H+(aq) → 2M+(aq) + H2O (l)
MOH(aq) + H+(aq) → M+(aq) + H2O (l)
For a divalent metal:
MO(s) + 2H+(aq) → M2+(aq) + H2O (l)
M(OH) 2(s) + 2H+(aq) → M2+(aq) + 2H2O(l)
For a trivalent metal:
M2O3(s) + 6H+(aq) → 2M3+(aq) + 3H2O (l)
M(OH) 3(s) + 3H+(aq) → M3+(aq) + 3H2O(l)

Examples:
For a monovalent metal: K2O(s) + 2H+(aq) → 2K+(aq) + H2O (l)
NH4OH(aq) + H+(aq) → NH4+(aq) + H2O (l)
For a divalent metal: ZnO (s) + 2H+(aq) → Zn2+(aq) + H2O (l)
Pb(OH) 2(s) + 2H+(aq) → Pb2+(aq) + 2H2O(l)

Chemical Properties of HCl gas and Ammonia Gas

Hydrogen chloride gas dissolves in methylbenzene /benzene but does not dissociate /ionize into free ions. It exists in molecular state showing none of the above properties.
Ammonia gas dissolves in water to form aqueous ammonia which dissociate/ionize to free NH4+ (aq) and OH-(aq) ions. This dissociation/ionization makes aqueous ammonia to:
  1. turn litmus paper/solution blue.
  2. have pH 8/9/10/11.
  3. be a good electrical conductor.
  4. react with acids to form ammonium salt and water only.
    5. NH4OH(aq) + HCl(aq) → NH4Cl(aq) + H2O(l)

Read on:

What are Acids?What are Bases?Polar and Non-Polar SolventsStrong and Weak Acids and BasesAmphoteric Oxides and HydroxidesMonobasic, Dibasic, and Tribasic AcidsHygroscopy, Deliquescence and EfflorescencePreparation of Soluble Salts in a LaboratoryCarbonates and Hydrogen Carbonates Reaction with AcidsNeutralization of a Soluble Base with Dilute AcidSalt Preparation by Direct Synthesis or CombinationPreparation of Insoluble SaltsEffect of Heat on Salts

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