Silver Chloride (AgCl) Is Insoluble In Water Ad Nitric Acid ... - Numerade

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Silver chloride (AgCl) is insoluble in water and nitric acid, but it is soluble in ammonia. Which statement is incorrect? Select one: O If present in sufficient concentration, ammonia will bind to Ag$^+$ ions to form a complex ion that is soluble in water. O AgCl is insoluble in water because the ionic bonds between the silver cation and the chlorine anion are stronger than the forces favouring formation of silver hydroxide (AgOH). O AgCl does not react with nitric acid, therefore AgCl is insoluble in nitric acid solution. O If an insufficient amount of ammonia is added, some AgCl precipitate will remain in solution. O In sufficiently concentrated ammonia, the concentration of silver ions in solution decrease to below the solubility product and a AgCl precipitate can no longer form. O The solubility constant $K_{sp}$ is very large therefore AgCl is insoluble in water and nitric acid. Silver chloride (AgCl) is insoluble in water and nitric acid, but it is soluble in ammonia. Which statement is incorrect? Select one: O If present in sufficient concentration, ammonia will bind to Ag$^+$ ions to form a complex ion that is soluble in water. O AgCl is insoluble in water because the ionic bonds between the silver cation and the chlorine anion are stronger than the forces favouring formation of silver hydroxide (AgOH). O AgCl does not react with nitric acid, therefore AgCl is insoluble in nitric acid solution. O If an insufficient amount of ammonia is added, some AgCl precipitate will remain in solution. O In sufficiently concentrated ammonia, the concentration of silver ions in solution decrease to below the solubility product and a AgCl precipitate can no longer form. O The solubility constant $K_{sp}$ is very large therefore AgCl is insoluble in water and nitric acid. Show more…

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Chemistry: Structure and Properties Nivaldo Tro 2nd Edition

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"If present in sufficient concentration; ammonia will bind to Ag+ ions to form a complex ion that is soluble in water." This statement is correct. Ammonia can indeed form a complex ion with silver ions, making AgCl soluble in ammonia. Show more…

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Submit Thanks for your feedback! Silver chloride (AgCl) is insoluble in water ad nitric acid, but it is soluble in ammonia Which statement is incorrect? Select one: If present in sufficient concentration; ammonia will bind t0 Agt ions t0 form a complex ion that is soluble in water AgCl is insoluble in water because the ionic bonds between the silver cation and the chlorine anion are stronger than the forces favouring formation of silver hydroxide (AgOH): AgCl does not react with nitric acid, therefore AgCl is insoluble in nitric acid solution; If an insufficient amount of ammonia is added, some AgCl precipitate will remain in solution: In sufficiently concentrated ammonia, the concentration of silver ions in solution decrease to below the solubility product and a AgCl precipitate can no longer form: The solubility constant Ksp is very large therefore AgCl is insoluble in water and nitric acid Play audio Feedback Powered by NumerAI

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If a saturated solution of silver chloride(AgCl) has a small amount of solid sodium chloride (NaCl) added which of the following is true AgCl(s)<--> Ag^+(aq) + Cl^-(aq) 1.The NaCl will dissolve and the equilibrium of AgCl will not change 2. The NaCl will dissolve and the Na+ ions will react with the AgCl(s) 3.The NaCl will dissolve and the equilibrium of AgCl will shift right more AgCl will dissolve 4.The NaCl will dissolve and the increased Cl will cause the equilibrium to shift left AgCl(s) will precipitate from solutions 5. The NaCl will form a solid in place of the AgCl(s)

Rashmi S.

Silver chloride, $\mathrm{AgCl}(s)$, is an "insoluble" strong electrolyte. (a) Write the equation for the dissolution of $\mathrm{AgCl}(s)$ in $\mathrm{H}_{2} \mathrm{O}(l)$ (b) Write the expression for $K_{c}$ for the reaction in part (a). (c) Based on the thermochemical data in Appendix $\mathrm{C}$ and Le Châtelier's principle, predict whether the solubility of $\mathrm{AgCl}$ in $\mathrm{H}_{2} \mathrm{O}$ increases or decreases with increasing temperature. (d) The equilibrium constant for the dissolution of $\mathrm{AgCl}$ in water is $1.6 \times 10^{-10}$ at $25^{\circ} \mathrm{C}$. In addition, $\mathrm{Ag}^{+}(a q)$ can react with $\mathrm{Cl}^{-}(a q)$ according to the reaction $$\mathrm{Ag}^{+}(a q)+2 \mathrm{Cl}^{-}(a q) \longrightarrow \mathrm{AgCl}_{2}^{-}(a q)$$ where $K_{c}=1.8 \times 10^{5}$ at $25^{\circ} \mathrm{C}$. Although $\mathrm{AgCl}$ is "not soluble" in water, the complex $\mathrm{AgCl}_{2}^{-}$ is soluble. At $25^{\circ} \mathrm{C},$ is the solubility of AgCl in a $0.100 M$ NaCl solution greater than the solubility of AgCl in pure water, due to the formation of soluble $\mathrm{AgCl}_{2}^{-}$ ions? Or is the $\mathrm{AgCl}$ solubility in $0.100 \mathrm{M} \mathrm{NaCl}$ less than in pure water because of a Le Châtelier-type argument? Justify your answer with calculations.

As a sodium chloride solution is added to a solution of silver nitrate, a white precipitate forms. Ammonia is added to the mixture and the precipitate dissolves. When potassium bromide solution is then added, a pale yellow precipitate appears. When a solution of sodium thiosulfate is added, the yellow precipitate dissolves. Finally, potassium iodide is added to the solution and a yellow precipitate forms. Write reactions for all the changes mentioned above. What conclusions can you draw concerning the sizes of the $K_{\mathrm{sp}}$ values for $\mathrm{AgCl}, \mathrm{AgBr},$ and AgI? What can you say about the relative values of the formation constants of $\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}+$ and $\mathrm{Ag}\left(\mathrm{S}_{2} \mathrm{O}_{3}\right)_{2}^{3-} ?$

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Transcript

00:01 The reason why silver chloride is soluble in ammonia is because the ammonia forms the complex ion with the silver by kicking off the chloride. 00:18 So we end up producing silver with two ammonia's and the chloride is removed. 00:30 And then silver chloride itself is so insoluble that really the reaction is favored this way because water is unable. 00:41 To pull the ions apart. 00:45 So of the statements, if present in sufficient concentration, ammonia will bind with silver ions to form complex ion that is soluble in solution. 00:55 That one's true. 01:00 B, silver chloride is insoluble in water because the ionic bonds between the silver cation and the chlorine anion are stronger than the forces favoring the formation of silver hydroxide. 01:13 Yeah, i guess i guess you could say that this silver ends up forming silver hydroxide. 01:24 So i would say that one's true. 01:26 And then for the third one, c, it says silver chloride does not react with nitric acid, therefore silver chloride is insoluble in nitric acid. 01:38 Yeah, i guess would say that. 01:40 I mean, it's soluble to a degree, but it's a very small extent, as mentioned up here. 01:45 The nitric acid doesn't influence this equilibrium like the ammonia does... Need help? Use Ace Ace is your personal tutor. It breaks down any question with clear steps so you can learn. Start Using Ace Ace is your personal tutor for learning Step-by-step explanations Instant summaries Summarize YouTube videos Understand textbook images or PDFs Study tools like quizzes and flashcards Listen to your notes as a podcast

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