To determine which reaction mixture will produce a precipitate, we need to consider the solubility rules for common ionic compounds:
1. Aqueous Na2CO3 and aqueous CuSO4:
- When Na2CO3 reacts with CuSO4, the following double replacement reaction occurs:
Na2CO3 + CuSO4 → Na2SO4 + CuCO3
- Copper(II) carbonate (CuCO3) is insoluble in water and will precipitate out of the solution, indicating that this mixture will produce a precipitate.
2. Dilute H2SO4 and aqueous NaOH:
- When H2SO4 reacts with NaOH, the following neutralization reaction occurs:
H2SO4 + 2NaOH → Na2SO4 + 2H2O
- Sodium sulfate (Na2SO4) is soluble in water and will not form a precipitate, so this mixture will not produce a precipitate.
3. Dilute HNO3 and solid MgO:
- Nitric acid (HNO3) reacting with magnesium oxide (MgO) will undergo an acid-base reaction:
HNO3 + MgO → Mg(NO3)2 + H2O
- Magnesium nitrate (Mg(NO3)2) is soluble in water, so no precipitate will form in this case.
Therefore, the reaction mixture of aqueous Na2CO3 and aqueous CuSO4 will produce a precipitate (CuCO3), while the other two mixtures will not result in a precipitate formation.
