Use the solubility interactive to complete the solubility table. co; SO? – s2 Pb2+ Ni2+ Ba? + Answer Bank soluble insoluble For the chemical reaction Na,Co, + Ca(NO3)2 +CaCO3 +2 NaNO, how many moles of calcium carbonate (CaCO3) are produced from 8.0 mol of sodium carbonat
The Correct Answer and Explanation is:
Answer:
For the reaction:
Na₂CO₃ + Ca(NO₃)₂ → CaCO₃ + 2 NaNO₃
From the balanced chemical equation, 1 mole of sodium carbonate (Na₂CO₃) reacts with 1 mole of calcium nitrate (Ca(NO₃)₂) to produce 1 mole of calcium carbonate (CaCO₃).
So, 8.0 moles of Na₂CO₃ will produce 8.0 moles of CaCO₃, provided there is at least 8.0 moles of Ca(NO₃)₂ available.
✅ Answer: 8.0 moles of CaCO₃ are produced.
Explanation
This problem involves a double displacement reaction between sodium carbonate (Na₂CO₃) and calcium nitrate (Ca(NO₃)₂). The balanced chemical reaction is:
Na₂CO₃ + Ca(NO₃)₂ → CaCO₃ ↓ + 2 NaNO₃
This equation shows a 1:1 molar ratio between sodium carbonate and calcium carbonate. That means for every 1 mole of Na₂CO₃ that reacts, 1 mole of CaCO₃ is produced, assuming calcium nitrate is present in excess or in an equimolar amount.
In this case, if we are given 8.0 moles of sodium carbonate and no limiting information about calcium nitrate, we assume it is in sufficient quantity. Therefore, using the molar ratio:
- 1 mol Na₂CO₃ : 1 mol CaCO₃
- 8.0 mol Na₂CO₃ : 8.0 mol CaCO₃
This reaction is also used in qualitative analysis to test for calcium ions. Calcium carbonate is insoluble in water, and it precipitates out as a solid. That’s why it appears as a white precipitate in lab settings.
Solubility rules tell us:
- Most carbonate salts (CO₃²⁻) are insoluble, except those with Group 1 cations (e.g., Na⁺, K⁺) and ammonium (NH₄⁺).
- Calcium carbonate (CaCO₃) is insoluble, so it forms a precipitate.
- Sodium nitrate (NaNO₃) is soluble and remains dissolved in the solution.
This simple stoichiometry calculation highlights key chemical concepts: molar ratios, limiting reactants, and solubility rules, which are fundamental in predicting the outcomes of chemical reactions.
