HonorsCh11(12-13).pptx

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1) Write a word equation for the reaction.

Write a balanced equation for the reaction between chlorine gas and aqueous sodium bromide to produce liquid bromine

and aqueous sodium chloride.

2) Write the correct formulas for all reactants and products.

3) Determine the coefficients that make the equation balance.

chlorine + sodium bromide  bromine + sodium chloride

Cl₂ _(g) + NaBr _(aq)  Br_{2 (l)} + NaCl _(aq)

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1) Write a word equation for the reaction.

2) Write the correct formulas for all reactants and products.

3) Determine the coefficients that make the equation balance.

aluminum sulfate + calcium chloride  calcium sulfate

Al₂(SO₄)₃ _(aq)+ CaCl_{2 (aq)}  CaSO_{4 (s)} + AlCl_{3 (aq)}

Write the balanced equation for the reaction

between aqueous aluminum sulfate and aqueous calcium chloride to form solid calcium sulfate and aqueous aluminum chloride.

Al₂(SO₄)_3(aq) + 3 CaCl_2(aq)  3 CaSO_4(s) + 2 AlCl_{3 (aq)}

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Many reactions involve substances dissolved in

water!

 Solute – substance that is dissolved.

 Solvent – the most plentiful substance

in the solution.

 Aqueous solution – a solution with

water as the solvent.

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11.3 Reactions in Aqueous

Solutions

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11.3 Reactions in Aqueous

Solutions

When ionic substances (and molecular acids) dissolve in water, they dissociate into individual ions and are more

accurately expressed as the products in the following equation.

HCl_(aq) H+

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11.3 Reactions in Aqueous

Solutions

When substances are put in

water and dissolved, calling

them aqueous is easy, but

it’s not an accurate depiction

of how the particles exist!

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Cl -(aq)

11.3 Reactions in Aqueous

Solutions

What is a more accurate way to write each aqueous

substance?

NaOH_(aq) 

MgCl_2(aq) 

Na+

(aq) + OH-(aq)

Mg2+

(aq) + 2Cl-(aq)

Mg2+ (aq)

Cl -(aq)

Na+

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11.3 Reactions in Aqueous

Solutions

How do you know if the compound dissolves in

water?

Use the solubility table!

From this point forward, please make sure you

include states of matter for all reactants and products.

Find states:

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11.3 Solubility

Substance State in water Dissociation reaction

AgCl

Pb(NO₃)₂

KI

Al₂(CO₃)₃

AgCl_(s) AgCl _(s)  NR

Pb(NO₃)_2(aq) Pb(NO3)2 (aq)  Pb2+ (aq) + 2NO3-(aq)

KI_(aq₎ KI _(aq)  K+

(aq) + I- (aq)

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11.3 Net Ionic Equations

Not all single replacement reactions occur – does this apply to double

replacement reactions too?

YES!

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11.3 Net Ionic Equations

When aqueous solutions that contain

ions are mixed, the ions may react in a

double-replacement reaction.

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11.3 Net Ionic Equations

 An example of a double-replacement

reaction that produces a precipitate

occurs when aqueous solutions of sodium chloride and silver nitrate are mixed to

form a precipitate of solid silver chloride.

 Use solubility chart to determine which

one is the solid.

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11.3 Net Ionic Equations



To show all of the particles in solution

as they really exist, a

complete ionic

equation

can be written.

Na+

(aq) + Cl

-(aq) + Ag

+

(aq) + NO3

-(aq) Na

+

(aq) + NO3

-(aq) + AgCl (s)

 Complete ionic equation – an ionic equation

that shows all of the particles as they really

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11.3 Net Ionic Equations

Na+

(aq) + Cl- (aq) + Ag+ (aq) + NO3- (aq)  Na+ (aq) + NO3- (aq) + AgCl (s)

Notice the sodium and nitrate ions are on both sides of the

equation.

Do they really do anything in the reaction?

No, they are spectator ions!

Na+

(aq) and NO3- (aq)

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11.3 Net Ionic Equations

If you eliminate the spectator ions, you are left with

the net ionic equation.

This is an ionic equation including only the particles

that participate in the reaction!

Na+

(aq) + Cl- (aq) + Ag+ (aq) + NO3- (aq)  Na+ (aq) + NO3- (aq) + AgCl (s)

Ag+

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Finding the Net Ionic

Equation

1. Predict products of the double

replacement reaction.

2. Balance

3. Find states of matter:

Insoluble (s), soluble (aq), and H₂O (l)

4. Write ionic equations (separate aqueous

into ions)

5. Write net ionic equation by canceling

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Pb(NO

₃

)

_{2 (aq)}

+ H

₂

SO

_{4 (aq)} 

Pb(NO₃)_{2 (aq)} + H₂SO_{4 (aq)}  PbSO₄ + HNO₃

Pb(NO₃)_{2 (aq)} + H₂SO_{4 (aq)}  PbSO₄ + 2HNO₃

Pb(NO₃)_{2 (aq)} + H₂SO_{4 (aq)}  PbSO_{4 (s)} + 2HNO_{3 (aq)}

Pb2+

(aq) + 2NO3- (aq) + 2H+(aq) + SO42- (aq)  PbSO4 (s) + 2H+ (aq) +

2NO₃- (aq)

Pb2+

(aq) + SO42- (aq)  PbSO4 (s)

1: Predict Products

2: Balance

3: Find States

4: Write ionic equations (separate into ions)

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Zn(NO

₃

)

_{2 (aq)}

+ Ba(OH)

_{2 (aq)} 

Zn(NO₃)_{2 (aq)} + Ba(OH)_{2 (aq)}  Zn(OH)₂ + Ba(NO₃)₂

Zn(NO₃)_{2 (aq)} + Ba(OH)_{2 (aq)}  Zn(OH)_{2 (s)} + Ba(NO₃)₂

(aq)

Zn2+

(aq) + 2NO3-(aq) + Ba2+(aq)+2OH1-(aq)  Zn(OH)2 (s) + Ba2+(aq)

+ 2NO₃ -(aq)

Zn2+

(aq) + 2 OH1-(aq)  Zn(OH)2 (s)

2: Balance

3: Find States

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Cu(OH)_{2 (aq)} + H₂SO_{4 (aq)}  CuSO₄ + H₂O

Cu(OH)_{2 (aq)} + H₂SO_{4 (aq)} CuSO₄ + 2 H₂O

Cu(OH)_{2 (aq)} + H₂SO_{4 (aq)}  CuSO_{4 (aq)} + 2 H₂O _(l)

Cu2+

(aq) + 2OH-(aq) + 2H+(aq) + SO42- (aq)  Cu2+ (aq) + SO42- (aq)

+ 2 H₂O _(l)

2 H+

(aq) + 2 OH1-(aq)  2H2O(l)

2: Balance

3: Find States

5: Write net ionic equation by canceling spectator ions (can be NR)

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CuCl

_2(aq)

+ NaNO

_3(aq) 

CuCl_{2 (aq)} + NaNO_{3 (aq)}  Cu(NO₃)₂ + NaCl

CuCl_{2 (aq)} + 2NaNO_{3 (aq)}  Cu(NO₃)₂ + 2NaCl

CuCl_{2 (aq)} + 2NaNO_{3 (aq)}  Cu(NO₃)_{2 (aq)} + 2NaCl _(aq)

Cu2+

(aq)+ 2Cl-(aq)+ 2Na1+(aq)+2NO31-(aq)Cu2+(aq)+2NO31-(aq)+ Na1+ (aq) 2Cl-(aq)

Cu2+

(aq)+ 2Cl-(aq)+ 2Na1+(aq)+2NO31-(aq)  NR 1: Predict Products

2: Balance

3: Find States