This series demonstrates a progression as 0.5 M solution of sodium carbonate (?? ?? ) as it is added drop-by-drop to a test tube containing 0.2 M solution of lead (II) nitrate (??(?? ) ) 1. What observations indicate that a chemical reaction has occurred? 2. Break up the reactants into ions. Switch the cations. Use the “criss-cross” method to get the balanced formulas for the products. Write the balanced molecular equation for this reaction, including phase labels. 3. Write the complete ionic equation for this reaction. 4. Write the net ionic equation for this reaction. 5. What is the precipitate?
This series demonstrates a progression as 0.5 M solution of sodium carbonate (?? ?? ) as it is added drop-by-drop to a test tube containing 0.2 M solution of lead (II) nitrate (??(?? ) )
1. What observations indicate that a
2. Break up the reactants into ions. Switch the cations. Use the “criss-cross” method to get the balanced formulas for the products. Write the balanced molecular equation for this reaction, including phase labels.
3. Write the complete ionic equation for this reaction.
4. Write the net ionic equation for this reaction.
5. What is the precipitate?
1. Formation of white precipitate indicates that a chemical reaction has occurred
2. The balanced chemical equation:
Na2CO3(aq) + Pb(NO3)2(aq) ---> 2NaNO3(aq) + PbCO3(s)
3. The ionic equation:
2Na+(aq) + CO32-(aq) + Pb2+(aq) + 2NO3-(aq) ---> 2Na+(aq) +2NO3-(aq) + PbCO3(s)
Step by step
Solved in 2 steps
