Which of the following compounds would result in an exchange reaction if mixed in an aqueous solution with (NH4)2S?

Question

Which of the following compounds would result in an exchange reaction if mixed in an aqueous solution with (NH4)2S?

a. SrCl2
b. Li2C2O4
c. CH3CO2Ag
d. MnSO4

I don't know what to look for.

Answer 1

Look for the following:

1. formation of an insoluble substance (a precipitate). Do you know the solubility rules?
2. formation of a gas.
3. formation of a weak electrolyte.
4. possibility of an oxidation-reduction reaction.

Here are the solubility rules.
http://www.files.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html

Answer 2

To determine which of the compounds would result in an exchange reaction with (NH4)2S, we need to identify compounds that contain cations that would be replaced by ammonium ions, NH4+.

Let's analyze each option:

a. SrCl2 - This compound contains strontium ions (Sr2+). Since (NH4)2S would not replace the strontium ions, there would be no exchange reaction.

b. Li2C2O4 - This compound contains lithium ions (Li+). Like strontium ions, lithium ions would not be replaced by ammonium ions, so there would be no exchange reaction.

c. CH3CO2Ag - This compound contains silver ions (Ag+). (NH4)2S would replace silver ions, leading to the formation of a precipitate of silver sulfide (Ag2S). Therefore, an exchange reaction would occur.

d. MnSO4 - This compound contains manganese ions (Mn2+). (NH4)2S would not replace manganese ions, so there would be no exchange reaction.

Therefore, the correct answer is:

c. CH3CO2Ag

Answer 3

To determine which of the given compounds would result in an exchange reaction when mixed with (NH4)2S in an aqueous solution, we need to understand what an exchange reaction is.

An exchange reaction, also known as a double displacement or metathesis reaction, occurs when two compounds in solution exchange positive ions (cation) or negative ions (anion) to form two new compounds. In simpler terms, the positive ions from one compound switch places with the positive ions of the other compound.

In the case of (NH4)2S, it is an aqueous solution of ammonium sulfide. It dissociates into ammonium ions (NH4+) and sulfide ions (S2-) in water. In an exchange reaction, the ammonium ions and sulfide ions will react with the positive ions (cations) in the other compound.

Now, let's analyze each compound from the options and determine if they would undergo an exchange reaction with (NH4)2S:

a. SrCl2:
When SrCl2 is dissolved in water, it dissociates into Sr2+ and Cl- ions. Since there are no ammonium (NH4+) or sulfide (S2-) ions in SrCl2, it will not undergo an exchange reaction with (NH4)2S. Therefore, option a is not the correct answer.

b. Li2C2O4:
When Li2C2O4 is dissolved in water, it dissociates into Li+ and C2O42- ions. Again, there are no ammonium (NH4+) or sulfide (S2-) ions in Li2C2O4, so it will not undergo an exchange reaction with (NH4)2S. Thus, option b is not the correct answer.

c. CH3CO2Ag:
When CH3CO2Ag (silver acetate) is dissolved in water, it dissociates into CH3CO2- and Ag+ ions. Since Ag+ is a cation, it can potentially exchange with NH4+ in (NH4)2S to form a new compound, NH4Ag. Therefore, option c is a possible answer.

d. MnSO4:
When MnSO4 is dissolved in water, it dissociates into Mn2+ and SO42- ions. Similarly, there are no ammonium (NH4+) or sulfide (S2-) ions in MnSO4, so it will not undergo an exchange reaction with (NH4)2S. Option d is not the correct answer.

Therefore, the compound from the given options that would result in an exchange reaction with (NH4)2S is option c: CH3CO2Ag.