1 / 8

Ions in Aqueous Solution

NO 3 1–. NO 3 1–. NO 3 1–. NO 3 1–. Pb 2+. Pb 2+. Na 1+. Na 1+. I 1–. I 1–. Ions in Aqueous Solution. Print Copy of Lab. Pb(NO 3 ) 2 (s). + H 2 O(l). Pb(NO 3 ) 2 (aq). Pb 2+ (aq) + 2 NO 3 1– (aq). add water. in solution. dissociation :. NaI(s) . + H 2 O(l). NaI(aq).

rashida-turan
Download Presentation

Ions in Aqueous Solution

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. NO31– NO31– NO31– NO31– Pb2+ Pb2+ Na1+ Na1+ I1– I1– Ions in Aqueous Solution Print Copy of Lab Pb(NO3)2(s) + H2O(l) Pb(NO3)2(aq) Pb2+(aq) + 2 NO31–(aq) add water in solution dissociation: NaI(s) + H2O(l) NaI(aq) Na1+(aq) + I1–(aq) Mix them and get… Balance to get overall ionic equation… Cancel spectator ions to get net ionic equation…

  2. Pb(NO3)2(aq) + 2 NaI(aq) + 2 Na1+(aq) PbI2(s) + 2 NO31–(aq) NO31– NO31– NO31– NO31– Pb2+ Pb2+ Na1+ Na1+ Na1+ Na1+ I1– I1– I1– I1– + 2 Na1+(aq) + 2 I1–(aq) Pb2+(aq) + 2 NO31–(aq) + 2 Na1+(aq) PbI2(s) + 2 NO31–(aq) Pb2+(aq) + 2 I1–(aq) PbI2(s) Solubility Chart Mix them and get… solid in solution Balance to get overall ionic equation… Cancel spectator ions to get net ionic equation…

  3. Zn(NO3)2(aq) + Ba(OH)2(aq) + Ba2+(aq) Zn(OH)2(s) + 2 NO31–(aq) OH1– NO31– Ba2+ Zn2+ NO31– OH1– + Ba2+(aq) + 2OH1–(aq) Zn2+(aq) + 2 NO31–(aq) + Ba2+(aq) Zn(OH)2(s) + 2 NO31–(aq) Zn2+(aq) + 2 OH1–(aq) Zn(OH)2(s) Solubility Chart Mix together Zn(NO3)2(aq) and Ba(OH)2(aq): Mix them and get… Zn(NO3)2(aq) Ba(OH)2(aq) Zn2+(aq) + 2 NO31–(aq) Ba2+(aq) + 2 OH1–(aq) Balance to get overall ionic equation… Cancel spectator ions to get net ionic equation…

  4. Pre-lab: • 1. What ions are present in the following solutions? • NaCl(aq) ____________________ AgNO3(aq) ____________________ • When these solutions are mixed together, a precipitate is seen. What are the new combinations of ions that could have formed the precipitate? • ____________________ and ____________________ • Using the solubility table, which new combination will form a precipitate? • ____________________  • Which new combination will remain in solution? • ____________________ • 5. Write the overall reaction equation for this reaction. Be sure to indicate the correct phase (reaction condition) for each reactant and each product. • 6. Write the net ionic equation for this reaction. Again, include the phases (reaction conditions). • 7. Explain why you would expect no reaction between solutions of KOH(aq) and NaOH(aq). Na1+(aq) Cl1-(aq) Ag1+(aq) NO31-(aq) Ag1+(aq) Na1+(aq) NO31-(aq) Cl1-(aq) Ag1+(aq) AgCl(s) Cl1-(aq) Na1+(aq) NO31-(aq) Na1+(aq) + Na1+(aq) + NO31-(aq) + Cl1-(aq) + Ag1+(aq) + NO31-(aq) AgCl(s) Ag1+(aq) + Cl1-(aq) AgCl(s) When the cations switch places they end with a hydroxide (no new combination is formed)

  5. Co2+(aq) + 2 OH1-(aq) Co(OH)2(s) 3. Co2+(aq) + 2 NO31-(aq) + 2 Na1+(aq) + 2 OH1-(aq) Co(OH)2(s) + 2 Na1+(aq) + 2 NO31-(aq) Co2+(aq) + 2 OH1-(aq) Co(OH)2(s) 9. Pb2+(aq) + 2 NO31-(aq) + 2 K1+(aq) + 2 OH1- (aq) Pb(OH)2(s) + 2 K1+(aq) + 2 NO31-(aq) Pb2+(aq) + 2 OH1-(aq) Pb(OH)2(s) 10. Pb2+(aq) + 2 NO31-(aq) + 2 Na1+(aq) + 2 OH1-(aq) Pb(OH)2(s) + 2 Na1+(aq) + 2 NO31-(aq) Pb2+(aq) + 2 OH1-(aq) Pb(OH)2(s) 11. Pb2+(aq) + 2 NO31-(aq) + Co2+(aq) + 2Cl1-(aq) PbCl2(s) + Co2+(aq) + 2 NO31-(aq) Pb2+(aq) + 2 Cl1-(aq) PbCl2(s) 12. 3 Pb2+(aq) + 6 NO31-(aq) + 2 Fe3+(aq) + 6 Cl1-(aq) 3 PbCl2(s) + 2 Fe3+(aq) + 6 NO31-(aq) Pb2+(aq) + 2 Cl1-(aq) PbCl2(s) Key Print Copy of Lab Reactions Between Ions in Aqueous Solutions spectator ions 2. Co2+(aq) + 2 NO31-(aq) + 2 K1+(aq) + 2 OH1-(aq) Co(OH)2(s) + 2 K1+(aq) + 2 NO31-(aq)

  6. Key Reactions Between Ions in Aqueous Solutions 15. Cu2+(aq) + 2 NO31-(aq) + 2 K1+(aq) + 2OH1-(aq) Cu(OH)2(s) + 2 K1+(aq) + 2 NO31-(aq) Cu2+(aq) + 2 OH1-(aq) Cu(OH)2(s) 16. Cu2+(aq) + 2 NO31-(aq) + 2 Na1+(aq) + 2OH1-(aq) Cu(OH)2(s) + 2 Na1+(aq) + 2 NO31-(aq) Cu2+(aq) + 2 OH1-(aq) Cu(OH)2(s) 20. Fe3+(aq) + 3 Cl1-(aq) + 3 K1+(aq) + 3 OH1-(aq) Fe(OH)3(s) + 3 K1+(aq) + 3 Cl1-(aq) Fe3+(aq) + 3 OH1-(aq) Fe(OH)3(s) 21. Fe3+(aq) + 3 Cl1-(aq) + 3 Na1+(aq) + 3 OH1-(aq) Fe(OH)3(s) + 3 Na1+(aq) + 3 Cl1-(aq) Fe3+(aq) + 3 OH1-(aq) Fe(OH)3(s) 24. Co2+(aq) + 2 Cl1-(aq) + 2 K1+(aq) + 2 OH1-(aq) Co(OH)2(s) + 2 K1+(aq) + 2 Cl1-(aq) Co2+(aq) + 2 OH1-(aq) Co(OH)2(s) 25. Co2+(aq) + 2 Cl1-(aq) + 2 Na1+(aq) + 2 OH1-(aq) Co(OH)2(s) + 2 Na1+(aq) + 2 Cl1-(aq) Co2+(aq) + 2 OH1-(aq) Co(OH)2(s)

  7. chromate hydroxide carbonate bromide chloride sulfide sulfate nitrate phosphate iodide acetate Legend SOLID SOLID AQUEOUS i = insoluble ss = slightly soluble s = soluble d = decomposes n = not isolated

  8. chromate hydroxide carbonate bromide chloride sulfide sulfate nitrate phosphate iodide acetate Legend s = solid aq = aqueous d = decomposes n = not isolated

More Related