1 / 25

AgNO 3 ( aq ) + NaCl( aq ) AgCl( s ) + NaNO 3 ( aq )

AgNO 3 ( aq ) + NaCl( aq ) AgCl( s ) + NaNO 3 ( aq ). What happens when you put AgNO 3 and NaCl in water?. AgNO 3 ( aq ) + NaCl( aq ) AgCl( s ) + NaNO 3 ( aq ). What really happens when you put AgNO 3 and NaCl in water?. KEY POINT: NaCl ( aq )

mauli
Download Presentation

AgNO 3 ( aq ) + NaCl( aq ) AgCl( s ) + NaNO 3 ( aq )

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq) What happens when you put AgNO3 and NaCl in water?

  2. AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq) What really happens when you put AgNO3 and NaCl in water?

  3. KEY POINT: NaCl (aq) really means: Na +1(aq) + Cl -1(aq) “dissociated ions” or “ions in solution”

  4. What is Dissolving ? When an ionic compound (eg salt) dissolves in water, the compound disassociates. (breaks apart into cations and anions) Ex: Ca(NO3)2(s)Ca2+(aq) + 2NO3-(aq) When a covalent compound (eg sugar) dissolves in water, the molecules simply disperse; they do not disassociate. Molecules of the covalent compounds simply disperse due to attraction with polar water molecules.

  5. An Ionic Compound Dissolves: A Covalent Compound Dissolves:

  6. KEY POINT: Mg(NO3)2(aq) really means: Mg +2(aq) + (NO3) -1(aq) 2 “dissociated ions” or “ions in solution”

  7. KEY POINT: AgCl (s) really means: AgCl (s) Solid Silver (I) Chloride.

  8. AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq) What happens when you put AgNO3 and NaCl in water?

  9. AgNO3 NaCl

  10. NO3- Na+ Ag+ Cl-

  11. Na+ NO3- Ag+ Cl-

  12. Na+ NO3- AgCl

  13. Na+ NO3- AgCl(s) precipitate AgCl

  14. NO3- Na+ NO3- NO3- Na+ Na+ Na+ NO3- NO3- Na+ Na+ Na+ NO3- NO3- Na+ NO3- Na+ AgCl(s)

  15. AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq) complete ionic equation

  16. AgCl Na+ NO3- Reaction

  17. No Reaction Na+ NO3- AgCl

  18. These ions do not participate in the reaction. They are called SPECTATOR IONS Na+ NO3- AgCl

  19. The net ionic equation is constructed from the complete ionic equation:

  20. NO3- and Na+ are not participating in the reaction

  21. net ionic equation

  22. net ionic equation

  23. Complete molecular equation- • describes double replacement reaction • Complete ionic equation- • more accurately shows the reacting species as ions and the products either as ions or a precipitate • Net ionic equation- • focuses only on the ions REACTING • Spectator ions are those ions that do NOT participate in the reaction

  24. PREDICTING THE FORMATION OF A PRECIPITATE • Consider the possibility that a precipitate may form. • Must use the solubility table on page 227 to decide. • Possible outcomes • No visible reaction (nvr) • Formation of one ppt. • Formation of two ppt. (rare occurrence)

  25. Basic Chemical equation AgNO3(aq) + KCl(aq)AgCl(s) + KNO3(aq) Complete ionic equation shows ions in solution Ag+ (aq)+NO3(aq) + K+ (aq)+Cl-(aq)AgCl(s) + K+ (aq) + NO3-(aq) Net ionic equation shows ions in rxn Ag+ (aq)+Cl-(aq)AgCl(s) (leave out spectator ions) link

More Related