Na2SO4 solution is slowly added to a solution which contains .10 M Ba (2+) and .1 M Pb(2+). which of the following statements descrives the result of the addition of Na2SO4
The addition of Na2SO4 to a solution containing Ba(2+) and Pb(2+) ions will result in the formation of precipitates. The following reactions will take place:
1. Na2SO4 dissociates into Na+ and SO4(2-) ions:
Na2SO4 → 2Na+ + SO4(2-)
2. Ba(2+) ions react with SO4(2-) ions to form BaSO4 precipitate:
Ba(2+) + SO4(2-) → BaSO4
3. Pb(2+) ions react with SO4(2-) ions to form PbSO4 precipitate:
Pb(2+) + SO4(2-) → PbSO4
Both BaSO4 and PbSO4 are insoluble salts, so they will precipitate out of the solution as solid particles. This precipitation reaction is due to the low solubility product constants (Ksp) of BaSO4 and PbSO4.
In summary, the addition of Na2SO4 to the solution will result in the formation of white precipitates of BaSO4 and PbSO4.
To determine the result of adding Na2SO4 to a solution containing Ba(2+) and Pb(2+), we need to understand the reaction between these ions and the sulfate ion (SO4(2-)).
Ba(2+) reacts with sulfate ion to form an insoluble compound called barium sulfate (BaSO4). This compound is white and can precipitate out of the solution.
Pb(2+) also reacts with sulfate ion to form an insoluble compound called lead sulfate (PbSO4), which is also a white precipitate.
Based on this information, we can make the following statements to describe the result of adding Na2SO4 to the solution:
1. When Na2SO4 is added, Ba(2+) ions react with SO4(2-) ions to form BaSO4. Therefore, we expect a white precipitate (BaSO4) to form.
2. Pb(2+) ions also react with SO4(2-) ions to form PbSO4. Therefore, a second white precipitate (PbSO4) should form.
In summary, adding Na2SO4 to the solution will result in the formation of white precipitates of both barium sulfate (BaSO4) and lead sulfate (PbSO4).