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Summary of Acid-Base Reactions

1) Neutralization:

acid + base salt + water

e.g. HCl (aq) + NaOH (aq) NaCl (aq) + H2O(l)

net ionic = H+

(aq) + OH

(aq) 2 H2O(l)

[ or H3O+(aq) + OH(aq) 2 H2O(l) ]

2) Bronsted- Lowry Acid-Base Reaction:

a) Acid + base salt

HCl(aq) + NH3(aq) NH4+

(aq) + Cl

(aq)

net ionic = H+(aq) + NH3 (aq) NH4+

(aq)

*Note: the presence of water as a solvent is not always required:HCl(g) + NH3 (g) NH4Cl (s)

b) Proton transfer reaction:

acid + base conjugate acid + conjugate base

CH3COOH + H2O (l) H3O+

(aq) + CH3COO

(aq)

H2O (l) + CO32-

(aq) HCO3-(aq) + OH

(aq)

Reminder: Water is amphoteric so can behave as either an acid or a base.

3) Lewis Acid-Base Reaction:

* Hint: For common examples, look for compounds of boron tri_______, combined with

a substance that has at least one lone electron pair, or look for formation of a

complex ion.

e.g. BF3 + F

(aq) BF4-(aq)

e.g. BCl3 + NH3 ClBNH3

acid + base salt

e.g. Ag+

(aq) + 2 NH3 Ag(NH3)2+

e.g. Reaction of a metal cation with water:

Fe3+

+ 6 H2O Fe(H2O)63+

Fe(H2O)5(OH)2+

+ H+

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4) Basic Oxides: (basic anhydrides) * basic oxides have metal cations

* Metal oxide + water metal hydroxide (base)

e.g. Na2O(s) + H2O(l) 2 NaOH(aq)net = Na2O(s) + H2O(l) 2 Na

+(aq) + 2 OH

-(aq)

e.g. BaO(s) + H2O(l) Ba(OH)2 (aq)

net = BaO(s) + H2O(l) Ba2+(aq) + 2 OH-(aq)

5) Acidic Oxides: (acid anhydrides)

* nonmetal oxide + water oxyacid

(1) CO2 (g) + H2O (l) H2CO3 (aq)(2) SO2(g) + H2O (l) H2SO3(3) SO3(g) + H2O (l) H2SO4*Note: These acids may further dissociate, especially if a strong acid:

SO3(g) + H2O HSO4- + H+

6) Reactions of Metals with Acids:

* nonoxidizing acids (HCl, dilute H2SO4) result in a single replacement reactions

Metal + acid salt + H2(g)

e.g. Zn + H2SO4 ZnSO4(aq) + H2(g)

net = Zn(s) + 2 H+

(aq) Zn2+

(aq) + H2(g)

* oxidizing acids (hot concentrated H2SO4, HNO3) form additional products besides

the salt + water.

w/ dilute HNO3 NO

conc. HNO3 NO2conc. H2SO4 H2S or SO2

eg. Zn(s) + H2SO4(conc.) ZnSO4 + H2S + H2OOR Zn

2++ SO2(g) + H2O(l)

(*I have found conflicting results on the above reaction in different textbooks)

HNO3 (dilute) + Cu(s) Cu(NO3)2 + NO(g) + H2O(l) (not balanced)

HNO3 (conc.) + Cu(s) Cu(NO3)2 + NO2(g) + H2O(l) (not balanced)

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7) Reactions of Acids with Metal Oxides:

Metal oxide + acid salt + water

CuO(s) + H2SO4 (dilute) CuSO4 + H2O(l)

net = CuO(s) + 2 H+

(aq) Cu2+

(aq) + H2O(l)

8) Reactions of Acids with Carbonates:

* note- almost all reactions that involve carbonates will result in the production of CO 2

Carbonate + acid salt + water + CO2(g)

e.g. CaCO3 (s) + 2 HCl (aq) CaCl2 (aq) + H2O + CO2(g)

net = CaCO3 (s) + 2 H+

(aq) Ca2+

(aq) + H2O(l) + CO2(g)

e.g. Na2CO3 (aq) + H2SO4 (aq) Na2SO4 (aq) + H2O + CO2(g)

net = CO32-

(aq) + 2 H+

(aq) H2O(l) + CO2(g)

e.g. 2 CH3COOH (aq) + CaCO3 (s) Ca(CH3COO)2 (aq) + H2O + CO2(g)

9) Reactions of Bases with Nonmetal Oxides:

* nonmetal oxide + hydroxide salt- or -

* nonmetal oxide + excess hydroxide salt + water

CO2(g) + NaOH (aq) NaHCO3 (aq)

CO2(g) + excess NaOH(aq) Na2CO3 (aq) + H2O (l)

10) Reactions of Metal oxides with nonmetal oxides (heated together no water involved)

Metal oxide + nonmetal oxide salt (containing oxygen in the anion)

e.g. MgO(s) + CO2 (g) MgCO3 (s)

6 CaO (s) + P4O10 (s) 2 Ca3(PO4)2 (s)

CaO (s) + SO3 (g) CaSO4 (s)

* Since these are all solids or

gases, not dissolved, these are the

net ionic equation also.

* Products are dependent on

relative concentrations of eachreactant

For net ionic

equations, do not

show the sodium