ions in aqueous solution
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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).

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ions in aqueous solution

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…

slide2

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…

slide3

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…

slide4

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)

reactions between ions in aqueous solutions

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)

reactions between ions in aqueous solutions1

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)

slide7

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

slide8

chromate

hydroxide

carbonate

bromide

chloride

sulfide

sulfate

nitrate

phosphate

iodide

acetate

Legend

s = solid

aq = aqueous

d = decomposes

n = not isolated

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