Which of the following pair of aqueous solutions when mixed will not form a precipitate?
A. FeCl2 (aq) and NaOH (aq)
B. Ni(NO3)2 (aq) and Li2(CO3) (aq)
C. KBr (aq) and AgNO3 (aq)
D. (NH4)2 CO3 (aq) and KBr (aq)
E. All of them
Well, let me take a closer look at these options to determine which pair won't have a "precipitate" performance.
A. FeCl2 (aq) and NaOH (aq) - Now, we all know that iron can be quite stubborn, always forming some sort of mess, so I wouldn't trust it not to leave any unwanted precipitates.
B. Ni(NO3)2 (aq) and Li2(CO3) (aq) - Nickel and carbonate? Sounds like a recipe for a funky chemistry experiment. Yeah, I doubt this pair will stay dissolved when combined.
C. KBr (aq) and AgNO3 (aq) - Potassium bromide and silver nitrate? Well, we all know silver loves to hang out with bromide ions, so I suspect some precipitate party will happen here.
D. (NH4)2 CO3 (aq) and KBr (aq) - Ammonium carbonate and potassium bromide? Honestly, I can't quite "nit"pick any reason why a precipitate wouldn't form when these two get together.
So, considering all these options, I'd go with:
E. All of them - because it's always better to be on the safe side and expect some precipitation in these situations. Being prepared for a little mess never hurts!
Remember, chemistry can be quite unpredictable, just like my humor!
To determine which of the following pairs of aqueous solutions when mixed will not form a precipitate, we need to use solubility rules.
Let's analyze each pair of solutions:
A. FeCl2 (aq) and NaOH (aq)
According to the solubility rules, FeCl2 is soluble in water, and NaOH is also soluble in water. When these two solutions are mixed, they will react to form Fe(OH)2, which is insoluble. Therefore, a precipitate will form.
B. Ni(NO3)2 (aq) and Li2(CO3) (aq)
Ni(NO3)2 is soluble in water, and Li2(CO3) is also soluble in water. Therefore, when these two solutions are mixed, they will not form a precipitate.
C. KBr (aq) and AgNO3 (aq)
KBr is soluble in water, and AgNO3 is also soluble in water. However, according to the solubility rules, silver bromide (AgBr) is insoluble. Therefore, a precipitate of AgBr will form when these two solutions are mixed.
D. (NH4)2 CO3 (aq) and KBr (aq)
(NH4)2CO3 is soluble in water, and KBr is also soluble in water. Therefore, when these two solutions are mixed, they will not form a precipitate.
Based on our analysis, the pair of aqueous solutions that will not form a precipitate when mixed is:
B. Ni(NO3)2 (aq) and Li2(CO3) (aq)
Therefore, the answer is B.
To determine if a precipitate will form when two aqueous solutions are mixed, we need to consider the solubility rules for various compounds.
A. FeCl2 (aq) and NaOH (aq):
To determine if a precipitate will form, we need to check if the possible combination of ions will form an insoluble compound. According to the solubility rules, hydroxides are generally insoluble except for those of alkali metals (Group 1) and ammonium (NH4+). Therefore, Fe(OH)2 will form a precipitate. So, the answer is NOT A.
B. Ni(NO3)2 (aq) and Li2(CO3) (aq):
When we examine the possible combination of ions, we find that Ni2+ and CO3^2- do not form an insoluble compound based on the solubility rules. In fact, the carbonate ion (CO3^2-) is generally insoluble except for those of alkali metals (Group 1) and ammonium (NH4+). Therefore, no precipitate will form in this case. So, the answer is B.
C. KBr (aq) and AgNO3 (aq):
When we look at the possible combination of ions, Br- and Ag+ form an insoluble compound (AgBr) based on the solubility rules. Therefore, a precipitate will form. So, the answer is NOT C.
D. (NH4)2CO3 (aq) and KBr (aq):
Looking at the possible combination of ions, NH4+ and Br- do not form an insoluble compound based on the solubility rules. Therefore, no precipitate will form. So, the answer is D.
Considering our analysis, the correct answer is B. Only the pair of aqueous solutions Ni(NO3)2 (aq) and Li2(CO3) (aq) will not form a precipitate. Therefore, the answer is NOT E.