The solid (insoluble) products of a double replacement reaction between aqueous sodium carbonate and aqueous strontium nitrate is
Na2CO3(aq) + Sr(NO3)2(aq) ==> SrCO3(s) + 2NaNO3(aq)
strontium carbonate is the solid.
To determine the solid (insoluble) products of a double replacement reaction between aqueous sodium carbonate (Na2CO3) and aqueous strontium nitrate (Sr(NO3)2), we need to consider the solubility rules.
Step 1: Write the balanced chemical equation for the double replacement reaction.
Na2CO3 + Sr(NO3)2 → ?
Step 2: Identify the ions present in the reactants.
Na2CO3 dissociates into two sodium ions (Na+) and one carbonate ion (CO3^2-).
Sr(NO3)2 dissociates into one strontium ion (Sr^2+) and two nitrate ions (NO3^-).
Step 3: Determine the possible solid products by combining the cations and anions from the reactants.
Since both sodium and strontium are group 2 metals, they can form insoluble carbonates when combined with carbonate ions.
Strontium carbonate (SrCO3) is insoluble, while sodium nitrate (NaNO3) is soluble.
Step 4: Write the balanced chemical equation with the solid product(s).
Na2CO3 + Sr(NO3)2 → NaNO3 + SrCO3
Therefore, the solid (insoluble) product of the reaction between aqueous sodium carbonate and aqueous strontium nitrate is strontium carbonate (SrCO3).
To determine the solid (insoluble) products of a double replacement reaction, you need to consider the solubility rules. These rules can guide you in predicting whether a compound will remain soluble or precipitate as a solid.
In this case, we have the reactants: aqueous sodium carbonate (Na2CO3) and aqueous strontium nitrate (Sr(NO3)2).
To find the products, you need to swap the cations (positive ions) of the reactants. The sodium ion (Na+) will combine with the nitrate ion (NO3-) to form sodium nitrate (NaNO3). The strontium ion (Sr2+) will combine with the carbonate ion (CO3^2-) to form strontium carbonate (SrCO3).
Now, we need to determine the solubility of these compounds. According to the solubility rules:
1. Most nitrate (NO3-) salts are soluble, so NaNO3 remains in the aqueous state.
2. Carbonates (CO3^2-) with alkali metal cations (such as Na+) are soluble, so Na2CO3 remains in the aqueous state.
However, strontium carbonate (SrCO3) is an exception to the rule. It is insoluble in water and will precipitate as a solid.
Therefore, the solid (insoluble) product of the reaction between aqueous sodium carbonate and aqueous strontium nitrate is strontium carbonate (SrCO3). The other product, sodium nitrate (NaNO3), remains in the aqueous state.