Solutions of sodium carbonate and silver nitrate react to form solid silver carbonate and a solution of sodium nitrate. A solution containing 3.50 g of sodium carbonate is mixed with one containing 5.00 g of silver nitrate. How many grams of sodium carbonate are present after the reaction is complete? How many grams of sodium nitrate are present after the reaction is complete?

Verified step by step guidance

1. Write the balanced chemical equation for the reaction: \[ \text{Na}_2\text{CO}_3 (aq) + 2\text{AgNO}_3 (aq) \rightarrow \text{Ag}_2\text{CO}_3 (s) + 2\text{NaNO}_3 (aq) \]
2. Calculate the molar mass of sodium carbonate (Na\_2CO\_3) and silver nitrate (AgNO\_3).
3. Determine the number of moles of sodium carbonate and silver nitrate using their respective masses and molar masses.
4. Identify the limiting reactant by comparing the mole ratio from the balanced equation with the moles available.
5. Calculate the amount of sodium carbonate remaining after the reaction by considering the stoichiometry and the limiting reactant.

Key Concepts

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the amounts of substances consumed and produced in a reaction, using mole ratios derived from the coefficients of the balanced equation.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for calculating the remaining quantities of reactants after the reaction has occurred.

Precipitation Reactions

Precipitation reactions occur when two soluble salts react in solution to form an insoluble solid, known as a precipitate. In this case, silver carbonate precipitates out of the solution when sodium carbonate and silver nitrate are mixed, which is essential for understanding the reaction's outcome and the quantities of reactants left.