Accelerated Chemistry Chapter 14 Notes

Accelerated Chemistry

Chapter 14

Accelerated Chemistry Chapter 14 Notes

Writing Names for Acids –

-2 types

-______

- ______(sometimes called _____)

binary - H and one other type of atom

name them hydro ______ic acid

Ex1 HCl

Ex2 HBr

Ex3 H3P

Writing formulas from names for Acids -

Ex4 Hydronitric Acid

Ex5 Hydrosulfuric Acid

ternary (oxy) – acids that have H with a polyatomic ion

Do not start with Hydro-

Change the –ate ending to –ic

Change the – ite ending to –ous

Ex6 H2SO4

Ex7 H2SO3

Ex8 HClO4

Ex9 HClO

When writing formulas from names-

Ex10 Nitric Acid

Ex11 Phosphorous Acid

Some common acids:

______– used for fertilizer, petroleum, production of metal, paper, paint

____ – stomach acid, food processing, iron, steel

______– vinegar, fungicide, produced by fermentation

______– explosives, rubber, plastics, dyes, drugs

______– beverage flavoring, animal feed, detergents

Properties of Acids:

Acid comes from Latin meaning acidus, or ______.

Affect the colors of ______. An indicator is a chemical that shows one color in an acid and another in a ______. Acids turn blue litmus ______.

Acids react with bases to produce ______. This is called ______.

HCl(aq) + NaOH(aq) ® NaCl(aq) + HOH(l)

3 H2SO4(aq) + 2 Al(OH)3(aq) ® Al2(SO4)3(aq) + 6 HOH(aq)

Acids ______in water. So, they ______electricity (______).

Acids react with active metals to produce ______and ______.

Mg(s) + 2 HCl(aq) ® MgCl2(aq) + H2(g)

Cu(s) + HCl(aq) ® NR

Definitions of Acids

1. Arrhenius Acids – a substance that produces _____ ions when mixed with water

HCl + H2O ®

Since that time it is found that

H+1 + H2O ®

so it is really…

HCl + H2O ®

2. Bronsted-Lowery Acids – proton donors

HCl + H2O ® H3O+1(aq) + Cl-1(aq)

HCl + NH3 ® NH4+1(aq) + Cl-1(aq) (*not Cl2!!)

Types of Acids

Strong - HI, HBr, HCl, HNO3, H2SO4, HClO4 (one way arrows always!)

Weak – HF, H2PO4, H2CO3, H2PO4 (double arrows always!)

Molecular, Total Ionic, and Net Ionic Equations for acids:

Molecular Equation:

Zn(s) + 2 HCl(aq) ®

But, since it’s aqueous, it is really…..

Total Ionic Equation:

Net Ionic Equation:

Some acids donate more than 1 proton….

Monoprotic (HF) - an acid that donates ______(one hydrogen)

Ex1: Write the reaction(s) showing the complete ionization of HF.

Diprotic (H2SO4) - an acid that donates ______(two hydrogens)

Ex2: Write the reaction(s) showing the complete ionization of H2SO4.

*Note: When you lose a H+1, you gain a negative.Triprotic Acid: an acid that donates ______(three hydrogens).

Ex3: Write the reaction(s) showing the complete ionization of H3PO4.

Diprotic and Triprotic can also be referred to as polyprotic.

2nd and 3rd ionizations are always weak (so, «).

When an acid ionizes, the reactions are written:

Ex1:

HCl(g) + H2O(l) ® H3O+1(aq) + Cl-1(aq)

______from the HCl is donated to the water.

HCl is a ______electrolyte (use a ______arrow).

H3O+1(aq) is called a ______ion.

Ex2:

HC2H3O2(l) + H2O(l) « H3O+1(aq) + C2H3O2-1(aq)

HC2H3O2 is a ______electrolyte (use a ______arrow).

Bases

Bases are used in cleaners (floors, drains, ovens), react with fats and oils so they become water soluble, used to neutralize stomach acid (antacids), used as laxatives

Properties of bases:

1. Bases are ______. They ______in water. NaOH and KOH are ______electrolytes because they are both highly soluble.

2. Affect the colors of ______. An indicator is a chemical that shows one color in an acid and another in a ____. Bases turn red litmus _____.

3. Bases react with acids to produce ______. This is called ______.

4. Bases taste______and feel ______. ______is an example of a base.

Definitions of Bases

A substance that has _ ions. Bases dissociate in water to give __ions.

Types of Bases

1. Traditional Bases (Arrhenius) – a substance that contains ______ions and dissociates to give ______ions in water.

NaOH(s) + H2O à Na+(aq) + OH-(aq)

Mg(OH)2(s) + H2O à Mg+2(aq) + 2OH-(aq)

2. Bronsted- Lowry bases –

NH3(g) + H2O(l) « NH4+1(aq) + OH-1(aq)

Water is ______. It can act as an ______or ______.

List of strong bases:

NaOH, KOH, CsOH, Ca(OH)2

List of weak bases:

many organic compounds with N…NH3, C6H5NH2, C2H3O2-

Neutralization reactions – hydronium + hydroxide yields water

It is a type of ______replacement reaction.

Note: H2O = ______

Acid + Base →

General Formula: HX + MOH ® MX + H2O

Example: hydrochloric acid + barium hydroxide ( molecular, total ionic, net ionic)

Relative Strengths of Acids and Bases

Some acids and bases are ______than others.

Bronsted (Danish) and Lowry (English) independently discovered that acids are

proton ______and bases are proton ______. A proton is a ______ion.

Strong Acid Example:

HCl(g) + H2O(l) ® H3O+1(aq) + Cl-1(aq)

Weak Base Example:

NH3(g) + H2O(l) « NH4+1(aq) + OH-1(aq)

Conjugate Acid-Base Pairs

Conjugate Acid: the substance that was the base and now acts as an ______.

Conjugate Base: the substance that was the acid and now acts as a ______.

HCl(g) + H2O(l) ® H3O+1(aq) + Cl-1(aq)

NH3(g) + H2O(l) « NH4+1(aq) + OH-1(aq)

HF(l) + H2O(l) « H3O+1(aq) + F-1(aq)

H2CO3(aq) + H2O(l) « H3O+1(aq) + HCO3-1(aq)

)

The stronger the acid, the weaker the ______.

Proton transfer reactions favor the production ______

______

Complete the equation and label acid base pairs

HSO4-1(aq) + HCO3-1(aq) «

Write an equation showing how NH2-1 is a stronger base than HSO4-1

Which one is correct?

HSO4-1(aq) + H3O+1(aq) « H2SO4(aq) + H2O(l)

(Base) (Acid) (Conjugate Acid) (Conjugate Base)

HSO4-1(aq) + OH-1(aq) « SO4-2(aq) + H2O(l)

(Acid) (Base) (Conjugate Base) (Conjugate Acid)

Strengths of Acids and Bases

Stuff to know:

2nd and 3rd ionizations are always weak. This means a double yield sign (______).

3. Memorize these strong acids. Strong means a single yield sign (______).

HI, HBr, HCl, HNO3, H2SO4, HClO4

4. All other acids get ______yield signs.

5. Strong bases include metals from column #1 and column #2 (below magnesium).

Proton reactions favor the formation of the ______acid and base.

General Reactions of Acids and Bases:

1. Neutralization (double replacement):

Acid + Base ®

HX + MOH ® MX + H2O

Ex1:

HCl(aq) + NaOH(aq) ®

2. Acid + Metal (single replacement):

Metal + Acid ®

Ex2:

Mg(s) + 2 HCl(aq) ®

3. Acid in water:

Acid + Water à

Ex3:

HCl(g) + H2O(l) ®

4. Traditional Base (ends with OH) in water (dissociation):

Base + Water à

Ex4:

Fe(OH)3(s) + H2O(l) «

5. Formation of acids and bases from anhydrides - synthesis (anhydride “without water”):

Nonmetal oxide + water ® acid

Ex5a:

CO2(g) + H2O(l) ® H2CO3(aq)

Ex5b:

SO3(g) + H2O(l) ® H2SO4(aq)

Note: just add the nonmetal oxide to the water to determine the product.

Metal oxide + water ®

Ex5c:

Na2O(s) + H2O(l) ®

Ex5d:

MgO(s) + H2O(l) ®

6. Acid and metal oxide (really just an acid and a base):

Acid + Metal Oxide à

Ex6:

H2SO4(aq) + CuO(s) ®

Turn CuO into Cu(OH)2

H2SO4(aq) + Cu(OH)2 (aq) ®

Now, re-write the original reactants, new products, and balance.

7. Base and nonmetal oxide (really just an acid and a base):

Base + Nonmetal Oxide à Salt + Water

Ex7a:

CO2(g) + NaOH(aq) ®

This is a little confusing. So these reactions will be done like:

CO2(g) + NaOH(aq) ®

Turn CO2 into H2CO3

Now, re-write the original reactants, new products, and balance.

Ex7b:

2 CO2(g) + Ca(OH)2(aq) ® Ca(HCO3)2(aq)

CO2(g) + Ca(OH)2(aq) ®

Turn CO2 into H2CO3

H2CO3(aq) + Ca(OH)2(aq) ® CaCO3(aq) + HOH(l)

Now, re-write the original reactants, new products, and balance.

CO2(g) + Ca(OH)2(aq) ® CaCO3(aq) + H2O(l)

8. Metal oxide and nonmetal oxide

It is like an acid base reaction they yield salt. However, it does not produce water

since no hydrogen is involved.

Ex8a:

MgO(s) + CO2(g) ® MgCO3(s)

Note: just add the nonmetal oxide to the metal oxide to determine the product.

Ex8b:

CuO(s) + SO3(g) ® CuSO4(s)

14_Notes_S.doc Page 1 of 13

Accelerated Chemistry Chapter 14 Notes