# silver nitrate and aluminum chloride net ionic equation

It can be called double displacement reaction or salt metathesis reaction, depending on who you're talking with. Lattice energy for AgCl ($\ce{Ag_{(g)}^+ + Cl_{(g)}^- -> AgCl_{(s)}}$) is more negative than for NaCl and KCl. Does a reaction occur when aqueous solutions of aluminum chloride and silver(I) nitrate are combined? The other answers make an error, I think. We have access to experiment, which clearly informs us that AgCl is insoluble in water. First of all, it's actually kind of an overdue homework question: It is well established in the pedagogical literature that AgCl is insoluble in water while NaCl and Why is that? Similar to the $\ce{NaCl}$ case above, $\ce{NO3-}$ and $\ce{Al^{3+}}$ are present as ions on both sides--so nothing to worry about there. 27461 views Of course, I sort of "assumed" that $\ce{AgCl}$ precipitates in the beginning--this was so that I wouldn't have to complicate stuff. indeed this is no redox problem, oxidation states do not change. This reaction is a type of metathesis reaction. rev 2020.11.24.38066, The best answers are voted up and rise to the top, Chemistry Stack Exchange works best with JavaScript enabled, Start here for a quick overview of the site, Detailed answers to any questions you might have, Discuss the workings and policies of this site, Learn more about Stack Overflow the company, Learn more about hiring developers or posting ads with us, I talked to my teacher today and she said it exactly as @CHM did. What is the ionic compound formula of magnesium nitrate? This means Aluminum Nitrate would have the formula Al(NO3)3. #Ag^(+)(aq) +NO_3^(-)(aq)+K^(+)(aq)+Cl^(-)(aq)->AgCl(s)+K^(+)(aq)+NO_3^(-)(aq)#. The easiest way to decide is by looking at thermodynamic stability--solid silver chloride is more stable. Maybe you can do your own research from the answers provided here and come back with a more "elaborate" answer. Why should I expect that black moves Rxd2 after I move Bxe3 in this puzzle? In this case, we have something slightly different. See all questions in Ionic Bond Formation. To analyse such situations, you first must realize that nearly everything is present as ions. How does the Dissonant Whispers spell interact with advantage from the halfling's Brave trait? The net ionic equation however, would be: Notice, the spectator ions - which are the common ions in both sides - are removed from the net ionic equation. $$\ce{Ag+ + Cl- <=> AgCl v}$$. Can lead(II) oxidize tin metal in aqueous solution? What is the ionic compound formula of ammonium sulfate? Edit the question and put the oxidation numbers to confirm that it is not a redox reaction. As you can see, I cannot provide you with a thorough answer, it would be extremely time consuming (for me) and I'd have to conduct many many calculations. Here are some ideas: Crystal growth in saturated solutions. I googled a bit about what $\ce{AgNO3 + AlCl3}$ will yield and found out the following: $\ce{3AgNO3 + AlCl3 -> Al(NO3)3 + 3AgCl}$. Stack Exchange network consists of 176 Q&A communities including Stack Overflow, the largest, most trusted online community for developers to learn, share their knowledge, and build their careers. MathJax reference. AgCl(s) is favored due to it is has a more covalent fashion than NO3. This reduces the reaction to: Now, we have reduced the question to "why does $\ce{AgCl}$ precipitate?". I just think it's obvious that the enthalpy of formation of AgCl is favorable, since it has to counter an unfavorable entropy loss in the formation of an ordered crystal lattice. Why does Lovecraft write that Mount Nansen (approx. What is the ionic compound formula of sodium sulfate? How do I legally resign in Germany when no one is at the office? AgCl is insoluble in water, therefore its solubility product is low. Here are some interesting points for the question: Liebman concludes from thermodynamic data (and contrary to HSAB expectations) that $\ce{Ag+}$ is better solvated than $\ce{Na+}$ or $\ce{K+}$. For example, if you took the reaction $\ce{NaCl +KBr->NaBr +KCl}$, the "direction" it goes in has no real meaning since $\ce{Na+}$, $\ce{Cl-}$, $\ce{K+}$, $\ce{Br-}$ are present as ions. What is the ionic compound formula of sodium hydroxide? If a piece of software does not specify whether it is licenced under GPL 3.0 "only" or "or-later", which variant does it "default to"? There is no actual reaction going on here, just a mixing of ions. Together with the total initial concentration of $\ce{Ag+}$ and $\ce{Cl-}$, you can then calculate the equilibrium concentrations. oxidize the Cl-, so that $\ce{Cl2 ^}$ is removed out of the system. The reaction between silver nitrate #AgNO_3# and potassium chloride #KCl# is the following:. There are some nice arguments why $\ce{AgCl}$ is less soluble than $\ce{AgNO3}$ in this post. My personal conclusions: It's a really though question. Why does potassium react more violently with water than lithium? Both suggest that the solubility product of AgCl is of importance in determining why the reaction takes place. instead it is a phase transition equilibrium I really hope someone can clarify the why. Is it because $\ce{Cl}$ is just one when $\ce{NO3}$ is multiple? Is the reaction of silver nitrate and copper endothermic or exothermic? Identify the oxidation and reduction half-reactions. How to find individual probabilities of all numbers from a list? Ag is higher up in the Reactivity serie than Al but that do not make sense to me in this problem. $\ce{AgCl}$ precipitates here: $$\ce{3AgNO3_{(aq)} + AlCl3_{(aq)} -> Al(NO3)3_{(aq)} + 3AgCl v}$$. Should recorded lectures be provided for students when teaching a math course online? I think the reaction proceeds because the formation of AgCl(s) is enthalpically favored.