1)Which cations should form soluble sulfate compounds from (Sodium, calcium, silver, copper 2)?
2) which anions should form precipitates with barium ions from (sulfate, carbonate and iodide?)
3) which anions should form precipitates with silver ions? Write net ionic equations for the reactions.
http://www.files.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html
To determine which cations form soluble sulfate compounds or which anions form precipitates with specific ions, we can refer to solubility rules and use the concept of ionic equations.
1) Solubility of Sulfate Compounds:
According to solubility rules, most sulfates are soluble; however, there are exceptions. The common solubility rule for sulfates is that salts containing Group 1 cations (such as sodium, Na+) and ammonium (NH4+) are always soluble.
So, in this case, sodium (Na+) would form a soluble sulfate compound.
Calcium (Ca2+) is a Group 2 cation. Group 2 sulfates are generally soluble; however, it's important to note that there are exceptions. Calcium sulfate (CaSO4) is sparingly soluble. It is considered slightly soluble, so it forms a precipitate under certain conditions, but it depends on the concentration and other factors.
Silver (Ag+) is not a Group 1 or Group 2 cation, and therefore, it does not follow the solubility rules for sulfates. Silver sulfate (Ag2SO4) is insoluble and forms a precipitate.
Copper (Cu2+) is not a Group 1 or Group 2 cation, but unlike silver, it does not form an insoluble sulfate compound. Copper sulfate (CuSO4) is soluble and does not form a precipitate.
2) Precipitates with Barium Ions:
To determine which anions form precipitates with barium ions (Ba2+), we refer to solubility rules again.
The solubility rule for sulfates states that most sulfates are soluble, except for sulfates of certain cations. BaSO4, barium sulfate, is one such sulfate that is mostly insoluble and forms a precipitate.
The solubility rule for carbonates states that most carbonates are insoluble, except for carbonates of certain cations. BaCO3, barium carbonate, is a carbonate that is mostly insoluble and forms a precipitate.
The solubility rule for iodides states that most iodides are soluble, including iodides containing barium. BaI2 and other barium iodides are soluble and do not form a precipitate.
Therefore, the anions that form precipitates with barium ions are sulfate (SO4^2-) and carbonate (CO3^2-), while iodide (I-) does not form a precipitate.
3) Precipitates with Silver Ions:
To determine which anions form precipitates with silver ions (Ag+), we refer to solubility rules again.
The solubility rule for chlorides states that most chlorides are soluble, including silver chloride (AgCl). However, it is important to note that silver chloride is only sparingly soluble; thus, it forms a precipitate under certain conditions.
The solubility rule for bromides states that most bromides are soluble, including silver bromide (AgBr). Similar to silver chloride, silver bromide is only sparingly soluble and forms a precipitate.
The solubility rule for iodides states that most iodides are soluble, including silver iodide (AgI). Similar to silver chloride and silver bromide, silver iodide is also only sparingly soluble.
The net ionic equations for the precipitations with silver ions would be as follows:
- Formation of silver chloride precipitate:
Ag+(aq) + Cl-(aq) → AgCl(s)
- Formation of silver bromide precipitate:
Ag+(aq) + Br-(aq) → AgBr(s)
- Formation of silver iodide precipitate:
Ag+(aq) + I-(aq) → AgI(s)
Remember that these net ionic equations represent the formation of precipitates and occur when the silver ion reacts with the respective anions.