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1.) A water sample contains Pb^2+, NO3^-, Ba^2+, ClO4^- part a. use the solubility rules to...

1.) A water sample contains Pb^2+, NO3^-, Ba^2+, ClO4^- part a. use the solubility rules to help you (i) select an ion that will only precipitate Pb^2+ from the mixture. (ii) Write the formula for the solid. (iii) Name the coumpund. part b. Use the solubility rules to help you (i) select an ion that can precipitate Ba^2+ from the remaining ions in that mixture ( there is no Pb^2+ left). (ii) Write the formula for the solid. (iii) Name the coumpound.

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Answer #1

Rule 3: All nitrate (NO3-), chlorate (ClO3-), perchlorate (ClO4-), and acetate salts are soluble.

For this reason Pb2+ and Ba2+ mixed with nitrate or perchlorate will be soluble salts.

Looking for the solubility of both salts, we can notice that perchlorate ion is more soluble than nitrate ion, and also lead salts are more soluble than barium salts at same temperature.

In conclusion, both ions will precipitate Pb2+ and Ba2+.

Knowing it:

a. Nitrate (NO3-) will precipitate more Pb2+. The compound formed is Pb(NO3)2, it is called lead nitrate.

b . Perchlorate (ClO4-) will precipitate the remaining Ba2+. The product formed is Ba(ClO4)2 and it's called barium perchlorate.

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