if I did? $%edit$. oxidize the Cl-, so that $\ce{Cl2 ^}$ is removed out of the system. I know that $\ce{Ag}$ is higher up in the reactivity series than $\ce{Al}$ but that does not make sense to me in this problem. We can experimentally prove this, or use standard enthalpies. By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy. site design / logo © 2020 Stack Exchange Inc; user contributions licensed under cc by-sa. Is it because $\ce{Cl}$ is just one when $\ce{NO3}$ is multiple? This reduces the reaction to: Now, we have reduced the question to "why does $\ce{AgCl}$ precipitate?". There are some nice arguments why $\ce{AgCl}$ is less soluble than $\ce{AgNO3}$ in this post. around the world. Why do silver nitrate and sodium hydroxide react to produce silver(I) oxide? Why does Lovecraft write that Mount Nansen (approx. How can I find the area of an overlayer structure? It only takes a minute to sign up. Maybe you can do your own research from the answers provided here and come back with a more "elaborate" answer. 3 AgNO3(aq) + AlCl3(aq) 3 AgCl(s) + Al(NO3)3(aq) Write the balanced net ionic equation for the reaction. My argument goes down the ladder. My personal conclusions: It's a really though question. We can experimentally prove this, or use standard enthalpies. Nevertheless, we can, in a similar way, experimentally prove that the others are found in ionized form and generally do not precipitate. Well, it seems AgCl is less ionic than AgNO3 since it is insoluble in water. 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. A bond with a greater covalent character is more stable, since the electrons are shared and not transfered. Looking for a function that approximates a parabola. Do all threads share the same instance of a heap variable, or have different instances of a heap variable? $$\ce{Ag+ + Cl- <=> AgCl v}$$. As it is behind a paywall, I'll try to summarize a few points out of it. indeed this is no redox problem, oxidation states do not change. But I find the particular situation far away from any textbook kind of reasoning that should introduce general chemical concepts to students. To analyse such situations, you first must realize that nearly everything is present as ions. 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. #AgNO_3(aq)+KCl(aq)->AgCl(s)+KNO_3(aq)# During this reaction, a precipitate will form which is the silver chloride #AgCl#.. Asking for help, clarification, or responding to other answers. I'll stick to the experiment with measurable properies such as equilibrium constants. AgCl(s) is favored due to it is has a more covalent fashion than NO3. by $\ce{NH3}$ or $\ce{CN-}$. This reduces the reaction to: $$\ce{3Ag+ + 3Cl- -> 3AgCl v}$$ Now, we have reduced the question to "why does $\ce{AgCl}$ precipitate?". 9000 ft.) is 15,000 feet high? You'll see that the precipitation moves the reaction towards equilibrium (unless the concentrations in the aqeous solution are not extremely low). Both suggest that the solubility product of AgCl is of importance in determining why the reaction takes place. If you can answer why AgCl is insoluble in water, then you can definitely predict that Ag+ and Cl- ions from different sources (i.e. AgCl is insoluble in water, therefore its solubility product is low. What is the ionic compound formula of sodium sulfate? @cbeleites: The second part of your answer would work as an answer here as well, you may want to try answering: Reaction between silver nitrate and aluminum chloride, Paradigms and Paradoxes: The Solubility of AgCl in Water, chemistry.stackexchange.com/questions/410/…, MAINTENANCE WARNING: Possible downtime early morning Dec 2/4/9 UTC (8:30PM…, “Question closed” notifications experiment results and graduation. I think the reaction proceeds because the formation of AgCl(s) is enthalpically favored. The other answers make an error, I think. What is the ionic compound formula of magnesium nitrate? Use MathJax to format equations. Why is ionic bonding stronger than covalent? Why is silver chloride less soluble than silver nitrate? 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. It can be called double displacement reaction or salt metathesis reaction, depending on who you're talking with. that the AgCl bond is less ionic than the AgNO3 bond, since it practically does not dissociate/has a low Ksp in water. Why does potassium react more violently with water than lithium? How does the Dissonant Whispers spell interact with advantage from the halfling's Brave trait? Aluminum has a +3 charge. Meaning of the Term "Heavy Metals" in CofA? What exactly are cap_style and join_style in shapely buffer function? If someone can predict and quantify the solubility product of AgCl in water from first principles, then that's another story, but the explanations offered only rely on observation (experiment) to quantify the Ksp. This means Aluminum Nitrate would have the formula Al(NO3)3. Lattice energy for AgCl ($\ce{Ag_{(g)}^+ + Cl_{(g)}^- -> AgCl_{(s)}}$) is more negative than for NaCl and KCl. Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds. Total ionic equation: I googled a bit about what $\ce{AgNO3 + AlCl3}$ will yield and found out the following: $\ce{3AgNO3 + AlCl3 -> Al(NO3)3 + 3AgCl}$. MathJax reference. instead it is a phase transition equilibrium Why is ionic bonding stronger than hydrogen bonding? The reaction between silver nitrate #AgNO_3# and potassium chloride #KCl# is the following:. What is the ionic compound formula of ammonium sulfate? Thus, silver nitrate has the formula AgNO3. Here are two experiments that you can do to check that it is really a dynamic equilibrium (though much on the side of the precipitate) The total ionic equation would be: So the point that is different is that the formation of diatomic AgCl is much more favorable than formation of diatomic NaCl or KCl. We can safely remove them from the equation. Here are some ideas: Crystal growth in saturated solutions. Is There (or Can There Be) a General Algorithm to Solve Rubik's Cubes of Any Dimension? How should this half-diminished seventh chord from "Christmas Time Is Here" be analyzed in terms of its harmonic function? Molecular cohesion (enthalpy) is greater in AgCl than in AgNO3, thus promoting its formation. Now you maybe thinking this argument is also circular, but it's not. Do I have to say Yes to "have you ever used any other name?" yes no If a reaction does occur, write the net ionic equation. What is the ionic compound formula of sodium phosphate? We can safely remove them from the equation. Can you have a Clarketech artifact that you can replicate but cannot comprehend? 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 $\ce{K+}$. Together with the total initial concentration of $\ce{Ag+}$ and $\ce{Cl-}$, you can then calculate the equilibrium concentrations. There is no actual reaction going on here, just a mixing of ions. 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. Krishna visiting Sudra's home or touching a Sudra, How to make my own professional book step-by-step( there is a course or a book that I didn't find?). Thanks for contributing an answer to Chemistry Stack Exchange! The paper estimates that the enthalpy of $\ce{AgCl_{(g)} -> AgCl_{(s)}}$ is comparable to that for the alkali chlorides. Reactions proceed in the direction of more stability, so the above reaction goes forward.