1 / 15

Precipitation Reactions

Precipitation Reactions. Solubility.

awena
Download Presentation

Precipitation Reactions

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. Precipitation Reactions Solubility

  2. ·When two solutions containing dissolved ions (eg. ionic compounds) are mixed, the ions will come into contact. Oppositely charged particles attract and sometimes the attraction is strong enough to form new compounds. Sometimes these compounds cannot dissolve in water and a solid forms. The insoluble solid formed is called a precipitate. Reactions in which precipitates form are called precipitation reactions.

  3. ·How can the precipitate of a chemical reaction be determined? ·The solubility rules!

  4. Solubility Rules ·All compounds containing either the Na+, NH4+, K+, or NO3- ion will dissolve in water ·Compounds containing the Cl-, Br- and I- ions are soluble (except when they contain Ag+, Pb2+ or Hg2+ ions) ·Compounds containing the SO42- ions are soluble (except when they contain Ba2+, Pb2+ or Ca2+ ions) ·Compounds containing CO32- and PO43- are insoluble (except when they contain Na+, NH4+ or K+ ions) ·Compounds containing OH- are insoluble (except when they contain Na+, NH4+, or K+ ions) ·Some compounds are slightly soluble; Ca(OH)2, PbCl2, PbBr2, CaSO4 and Ag2SO4

  5. Precipitation Reactions ·Reaction in which a solid is formed --> Precipitate ·Reaction Classification: Double Displacement / Replacement AB + CD --> AD + CB

  6. Example KI(aq) + AgNO3(aq) --> KNO3 + AgI How do we know which one is the precipitate? Solubility rules (handout) Insoluble – forms a precipitate Soluble – remains dissociated (does not form a precipitate) KI(aq) + AgNO3(aq) --> KNO3(aq) + AgI(s)

  7. Predicting the Precipitate Determine Solubility of Each Product ·Solubility rules (handout) ·if product is insoluble or slightly soluble, it will precipitate

  8. Example Ba(NO3)2(aq) + CuSO4(aq) --> BaSO4 + Cu(NO3)2 Which product will be the precipitate??? ·Use your solubility rules handout SO42- always soluble except with Ba2+ Therefore BaSO4is insoluble --> Precipitate! Ba(NO3)2(aq) + CuSO4(aq) --> BaSO4(s) + Cu(NO3)2(aq)

  9. http://www.mhhe.com/physsci/chemistry/animations/chang_7e_esp/crm3s2_3.swfhttp://www.mhhe.com/physsci/chemistry/animations/chang_7e_esp/crm3s2_3.swf

  10. IONS Dissociation ·“To break apart” ·When an ionic solid dissolves in water, the ions separate and move independently Determine what ions each aqueous reactant has http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/molvie1.swf

  11. EXAMPLES NaCl(aq) + AgNO3(aq) --->

  12. K2SO4(aq) + NaOH(aq) --->

  13. CaCl2(aq) + Na2CO3(aq) --->

  14. Cu(NO3)2(aq) + NaOH(aq) --->

More Related