Solutions & Solubility: Net Ionic...

Solutions & Solubility: Net Ionic Equations

(9.1 in MHR Chemistry 11)

Friday, April 5, 2013

Solubility vs. Temperature

Solubility TableSOLUBILITYTable 8.3page 363 in MHR

SOLUBILITYTable 8.3page 363 in MHR

AnionsAnionsAnionsAnionsAnionsAnionsAnionsSOLUBILITYTable 8.3page 363 in MHR

SOLUBILITYTable 8.3page 363 in MHR Cl-, Br-, I- S2- OH- SO4

2- CO32-,

PO43-,

C2H3O2- NO3

High solubility

(aq)≥ 0.1 mol/L

at SATP

MostGroup 1,

Group 2

Group 1, NH4

+, Sr2+,

Ba2+, Tl+Most Group 1,

NH4+ Most AllHigh

solubility (aq)

≥ 0.1 mol/L at SATP All Group 1 compounds, including acids, and all ammonium compounds

are assumed to have high solubility in water.All Group 1 compounds, including acids, and all ammonium compounds

are assumed to have high solubility in water.

Low solubility

(s)< 0.1 mol/L

at SATP

Ag+, Pb2+, Tl+, Hg2

2+, (Hg+), Cu+

Most MostAg+, Pb2+, Ca2+, Ba2+, Sr2+, Ra2+

Most Ag+ None

ns ?Friday, April 5, 2013

Solubility Table Create soluble and insoluble compounds using OH-

2- CO32-,

PO43-,

C2H3O2- NO3

High solubility

(aq)≥ 0.1 mol/L

at SATP

MostGroup 1,

Group 2

Group 1, NH4

+, Sr2+,

NH4+ Most AllHigh

solubility (aq)

Low solubility

(s)< 0.1 mol/L

at SATP

Ag+, Pb2+, Tl+, Hg2

2+, (Hg+), Cu+

Most Ag+ None

1. Write the overall balanced chemical equation.

2. Write the total ionic equation. Break all aqueous compounds into constituent

ions using solubility information (page 363). Leave solids, liquids and gases alone.

3. Write the net ionic equation. Identify and cancel spectator ions in the total

ionic equation. Reduce coefficients if necessary.

Writing Net Ionic Equation

Sample Problem 1 - Net Ionic Equation

Write the net ionic equation for the reaction between aqueous silver nitrate and aqueous sodium chloride.

Step 1 - Overall balanced chemical equation

AgNO3 (aq) + NaCl (aq)

AgCl (?) + NaNO3 (?)

2. Write the total ionic equation. Break all aqueous compounds into

constituent ions using solubility information (page 363).

Leave solids, liquids and gases alone.

AgCl (?) + NaNO3 (?)

Check solubility information (page 363)

SOLUBILITYTable 5, page 324

AnionsAnionsAnionsAnionsAnionsAnionsAnionsSOLUBILITYTable 5, page 324

SOLUBILITYTable 5, page 324 Cl-, Br-, I- S2- OH- SO4

2- CO32-,

PO43-,

C2H3O2- NO3

High solubility

(aq)≥ 0.1 mol/L

at SATP

MostGroup 1,

Group 2

Group 1, NH4

+, Sr2+,

NH4+ Most AllHigh

solubility (aq)

Low solubility

(s)< 0.1 mol/L

at SATP

Ag+, Pb2+, Tl+, Hg2

2+, (Hg+), Cu+

Most Ag+ None

AgCl ( ? ) AgCl ( s )

Check solubility information (p. 363)

SOLUBILITYTable 5, page 324

AnionsAnionsAnionsAnionsAnionsAnionsAnionsSOLUBILITYTable 5, page 324

SOLUBILITYTable 5, page 324 Cl-, Br-, I- S2- OH- SO4

2- CO32-,

PO43-,

C2H3O2- NO3

High solubility

(aq)≥ 0.1 mol/L

at SATP

MostGroup 1,

Group 2

Group 1, NH4

+, Sr2+,

NH4+ Most AllHigh

solubility (aq)

Low solubility

(s)< 0.1 mol/L

at SATP

Ag+, Pb2+, Tl+, Hg2

2+, (Hg+), Cu+

Most Ag+ None

NaNO3 ( ? ) NaNO3 ( aq )

AgCl (s) + NaNO3 (aq)

Ag+ (aq) + NO3

- (aq) + Na+ (aq) + Cl- (aq)

AgCl (s) + Na+(aq) + NO3

- (aq)

Writing Net Ionic Equations Step 2 - Total ionic equation

AgNO3 (aq) NaCl (aq)

NaNO3 (aq)Do not dissociate into

ionsFriday, April 5, 2013

Ag+ (aq) + NO3

- (aq) + Na+ (aq) + Cl- (aq)

AgCl (s) + Na+(aq) + NO3

- (aq)

2. Write the total ionic equation. Break all aqueous compounds into constituent

ions using solubility information (p. 363). Leave solids, liquids and gases alone.

3. Write the net ionic equation. Identify and cancel spectator ions in the total

ionic equation. Reduce coefficients if necessary.

Writing Net Ionic Equations Step 3 - Net ionic equation

Ag+(aq) + Cl- (aq) AgCl (s)

Spectator ions: NO3- (aq) , Na+

Complete Solution Write the net ionic equation for the reaction between aqueous silver nitrate and aqueous sodium chloride.

Step 1. Complete Balanced Chemical EquationAgNO3(aq) + NaCl (aq) AgCl (s) + NaNO3 (aq)

Step 2. Total Ionic EquationAg+

(aq) + NO3- (aq) + Na+

(aq) + Cl- (aq) AgCl (s) + NO3-

(aq) + Na+

Step 3. Net Ionic Equation Ag+

(aq) + Cl- (aq) AgCl (s) Spectator ions: NO3

- (aq) , Na+ (aq)

Sample Problem 2 - Net Ionic Equation

Write the net ionic equation for the reaction between aqueous lithium carbonate & aqueous calcium acetate

Write the net ionic equation for the reaction between aqueous lithium carbonate and aqueous calcium acetate.

Li2CO3 (aq) + Ca(C2H3O2)2 (aq)

2 LiC2H3O2 (?) + CaCO3 (?)

Check solubility information (p. 363)

LiC2H3O2 ( ? ) LiC2H3O2 ( aq )SOLUBILITYTable 8.3page 363 in MHR

2- CO32-,

PO43-,

C2H3O2- NO3

High solubility

(aq)≥ 0.1 mol/L

at SATP

MostGroup 1,

Group 2

Group 1, NH4

+, Sr2+,

NH4+ Most AllHigh

solubility (aq)

Low solubility

(s)< 0.1 mol/L

at SATP

Ag+, Pb2+, Tl+, Hg2

2+, (Hg+), Cu+

Most Ag+ None

CaCO3 ( ? ) CaCO3 ( s )SOLUBILITYTable 8.3page 363 in MHR

2- CO32-,

PO43-,

C2H3O2- NO3

High solubility

(aq)≥ 0.1 mol/L

at SATP

MostGroup 1,

Group 2

Group 1, NH4

+, Sr2+,

NH4+ Most AllHigh

solubility (aq)

Low solubility

(s)< 0.1 mol/L

at SATP

Ag+, Pb2+, Tl+, Hg2

2+, (Hg+), Cu+

Most Ag+ None

nsCheck solubility information (p. 363)

Li2CO3 (aq) + Ca(C2H3O2)2 (aq)

2 LiC2H3O2 (aq) + CaCO3 (s)

2 Li+(aq) + CO32- (aq) + Ca2+

(aq) +2 C2H3O2-(aq)

2 Li+(aq) +2 C2H3O2-(aq) + CaCO3 (s)

Writing Net Ionic Equations Step 3 - Net ionic equation

Ca2+(aq) +CO3

2-(aq) CaCO3 (s)

Spectator ions: C2H3O2- (aq) , Li+

Complete SolutionWrite the net ionic equation for the reaction between aqueous lithum carbonate and aqueous calcium acetate.

Step 1. Complete Balanced Chemical EquationLi2CO3(aq) + Ca(C2H3O2)2 (aq) 2 LiC2H3O2 (aq) + CaCO3 (s)

Step 2. Total Ionic Equation2 Li+(aq)+CO3

2-(aq) + Ca2+

(aq)+ 2 C2H3O2- (aq) 2 Li+(aq)+ 2 C2H3O2

- (aq) + CaCO3 (s)

Step 3. Net Ionic Equation Ca2+

(aq) + CO3- (aq) CaCO3 (s)

Spectator ions: C2H3O2

- (aq) , Li+ (aq)

Try it!

z p. 410 # 2,4,6,8,10

Solutions & Solubility: Net Ionic...

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