Decide whether each of the following is water-soluble. If soluble tell what ions are produced.
A. Na2CO3
B. CuSO4
C.NiS
D.BaBr2
I put soluble for A, B, and D. But i can not figure out the ions that are produced??
JuCt ionize them.
Na2CO3 ==> 2Na^+ + CO3^-2
CuSO4 ==> Cu^+2 + SO4^-2
BaBr2 ==> ?? + ??
Ba^+2 + 2 Br^-
Let's go through each compound and determine if it is water-soluble and what ions are produced when it dissolves:
A. Na2CO3 (Sodium carbonate):
- Sodium carbonate is soluble in water.
- When it dissolves, it dissociates into sodium (Na+) and carbonate (CO3 2-) ions.
B. CuSO4 (Copper sulfate):
- Copper sulfate is soluble in water.
- When it dissolves, it dissociates into copper (Cu2+) and sulfate (SO4 2-) ions.
C. NiS (Nickel sulfide):
- Nickel sulfide is not soluble in water. Therefore, it does not produce any ions when dissolved.
D. BaBr2 (Barium bromide):
- Barium bromide is soluble in water.
- When it dissolves, it dissociates into barium (Ba2+) and bromide (Br-) ions.
To summarize, the correct answers are:
A. Na2CO3 - Soluble, produces Na+ and CO3 2- ions.
B. CuSO4 - Soluble, produces Cu2+ and SO4 2- ions.
C. NiS - Insoluble, does not produce any ions.
D. BaBr2 - Soluble, produces Ba2+ and Br- ions.
To determine whether a compound is water-soluble, you need to consider the solubility rules. These rules detail the conditions under which compounds dissociate and dissolve in water.
Let's go through each compound and determine its solubility and the ions produced when it dissolves:
A. Na2CO3 (Sodium Carbonate):
According to the solubility rules, carbonate (CO3^2-) compounds, except for those containing alkali metal cations (Group 1 elements like sodium), are typically insoluble. Therefore, Na2CO3 is soluble.
When Na2CO3 dissolves in water, it dissociates into Na+ and CO3^2- ions:
Na2CO3 -> 2Na+ + CO3^2-
B. CuSO4 (Copper (II) Sulfate):
Copper (II) sulfate is typically soluble in water according to the solubility rules.
When CuSO4 dissolves in water, it ionizes into Cu2+ and SO4^2- ions:
CuSO4 -> Cu^2+ + SO4^2-
C. NiS (Nickel (II) Sulfide):
Nickel (II) sulfide is considered insoluble in water based on the solubility rules. Although there are exceptions for some sulfide compounds, nickel (II) sulfide is generally not water-soluble.
D. BaBr2 (Barium Bromide):
Like most bromides, barium bromide is soluble in water based on the solubility rules.
When BaBr2 dissolves in water, it dissociates into Ba^2+ and 2Br- ions:
BaBr2 -> Ba^2+ + 2Br-
In summary, the solubilities and ions produced are as follows:
A. Na2CO3 is soluble, and it produces Na+ and CO3^2- ions.
B. CuSO4 is soluble, and it produces Cu^2+ and SO4^2- ions.
C. NiS is insoluble.
D. BaBr2 is soluble, and it produces Ba^2+ and 2Br- ions.