Which of the following pairs of compounds will give a precipitate in a diluted solution?
Question 4 options:
A) Cu(NO3)2 and Na2CO3
B) KNO3 and NaCl
C) MgCl2 and Ba(NO3)2
D) NH4Cl and Al2(SO4)3
ALL OF THEM ARE SOLUBLE? WHAT DO I DO?
To determine if a precipitation reaction will occur and which pair of compounds will give a precipitate in a diluted solution, we need to refer to the solubility rules.
1. Start by writing out the chemical formulas for the compounds in each option:
A) Cu(NO3)2 and Na2CO3
B) KNO3 and NaCl
C) MgCl2 and Ba(NO3)2
D) NH4Cl and Al2(SO4)3
2. Next, we need to consult the solubility rules. The rules state that most nitrate (NO3-) salts are soluble, as are most alkali metal (Group 1) salts such as sodium (Na+).
3. For compound A, Cu(NO3)2 and Na2CO3, both compounds are soluble according to the solubility rules. Therefore, there won't be a precipitate formed in a diluted solution.
4. For compound B, KNO3 and NaCl, both compounds are also soluble according to the solubility rules. Hence, there won't be a precipitate formed in a diluted solution.
5. For compound C, MgCl2 and Ba(NO3)2, the solubility rules state that most chloride (Cl-) salts are soluble except for those of silver (Ag+), lead (Pb2+), and mercury (Hg2+). Both magnesium (Mg2+) chloride (Cl-) and barium (Ba2+) nitrate (NO3-) salts are soluble according to the rules. Therefore, there won't be a precipitate formed in a diluted solution.
6. For compound D, NH4Cl and Al2(SO4)3, the solubility rules tell us that most sulfate (SO4^2-) salts are soluble except for those of calcium (Ca2+), strontium (Sr2+), barium (Ba2+), lead (Pb2+), and silver (Ag+). Ammonium (NH4+) chloride (Cl-) is soluble, while aluminum (Al3+) sulfate (SO4^2-) is also soluble according to the rules. Hence, there won't be a precipitate formed in a diluted solution.
Therefore, after considering the solubility rules, none of the compound pairs in the given options will form a precipitate in a diluted solution.
If all of the compounds are soluble, it means that they will not form a precipitate in a diluted solution. In this case, none of the provided options would give a precipitate in a diluted solution.
Not quiet. The all are soluble, then dissociate, and form ions, which float, and mix. If the mix forms a compound which is insoluble...
Take a look at the solubility rules for carbonate compounds, I cant think of a group II carbonate that is soluble. http://mrnorton.com/Chemistry/Tables/Solubility%20Rules.pdf