Answer:
1. Zn(OH)₂ (s)
2. Ag₂CO₃ (s)
3. Ni₃(PO₄)₂(s)
4. No reaction
5. (NH₄)₂CO₃(s)
Explanation:
Let's state the equations and we analyse some solubility and precipitation information:
ZnCl₂(aq) + 2KOH(aq) → Zn(OH)₂ (s) + 2KCl (aq)
All the salts from the halogens with group 1, are soluble.
The OH⁻ reacts to Zn cation in order to produce a precipitate. This is ok, but if the base is in excess, the Zn(OH)₂ will be soluble
K₂CO₃(aq) + 2AgNO₃(aq) → Ag₂CO₃ (s) ↓ + 2KNO₃(aq)
All salts from nitrate are soluble
All salts from carbonates are insoluble
2(NH₄)₃PO₄(aq) + 3Ni(NO₃)₂(aq) → Ni₃(PO₄)₂(s) ↓ + 6NH₄NO₃(aq)
Salts from phosphates are insoluble
All salts from nitrate are soluble
NaCl(aq) + KNO3(aq) → NO REACTION
All salts from nitrate are soluble
All the salts from the halogens with group 1, are soluble
Na₂CO₃(aq) + 2NH₄Cl(aq) → 2NaCl(aq) + (NH₄)₂CO₃(s) ↓
All salts from carbonates are insoluble
All the salts from the halogens with group 1, are soluble
