Hi thank you so much!!!!
What is a net ionic equation for the reaction of H+ with Cu(NH3)4 ^2+
ALSO
what is the net ionic equation for the reaction of H+ with Hg2Cl2
Does the H+ addition increase, decrease, or has no impact on the solubility of the salt.?
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Cu(NH3)4^+2 + 4H^+ ==> 4NH4^+ + Cu^+2
The solubility of Hg2Cl2 in acid depends upon the acid used. My sources say Hg2Cl3 is soluble in HNO3.
To find the net ionic equation for the reaction between H+ and Cu(NH3)4^2+, we first need to know the chemical equation for the reaction between these two species.
The chemical equation for this reaction can be given as follows:
H+ + Cu(NH3)4^2+ → Cu^2+ + 4NH3
To find the net ionic equation, we need to eliminate the spectator ions. In this case, NH3 is a weak base and does not significantly contribute to the reaction. Thus, NH3 can be considered as a spectator ion.
The net ionic equation can, therefore, be written as:
H+ + Cu(NH3)4^2+ → Cu^2+ + H+
Moving on to the second part of your question, to determine the net ionic equation for the reaction between H+ and Hg2Cl2, we need to know the chemical equation for this reaction.
The chemical equation for this reaction is:
H+ + Hg2Cl2 → 2H+ + HgCl2
Here, the chloride ions (Cl^-) are the spectator ions, and they do not undergo any significant change during the reaction.
Therefore, the net ionic equation can be written as:
H+ + Hg2Cl2 → HgCl2
As for your final question about the impact of H+ addition on the solubility of the salt, it depends on the specific salt in question. In general, the addition of H+ ions can increase the solubility of salts if they contain anions (negative ions) that can form soluble acids or complexes in acidic conditions. On the other hand, if the salt contains anions that form insoluble compounds in the presence of H+ ions, the solubility may decrease.
In the case of the two reactions mentioned above, the solubility of Cu(NH3)4^2+ and Hg2Cl2 are not significantly affected by the addition of H+ ions. The solubilities of these salts mainly depend on other factors such as the stability of the complex ions or the solubility product constant of the compound.