Ch. 7 Acid-Base

Question 1

What are the three different types of acids?

Answer 1

Arrhenius acids (acids dissociate to form H+ ions, and bases dissociate to form 0H-)

Brownstein-Lowry (Acids are a proton donor, and bases are a proton accceptor)

Lewis acid (acids are an electron acceptor, bases are an electron donor)

Question 2

What is Kw?

Answer 2

Water auto-ionization equilibrium constant.
It is the reaction of water with it’s self to form ions.
(H3O & OH-)

Question 3

How is water auto-ionization calculated?

Answer 3

products/reactants (H2O is not included)

Question 4

(T/F) Kw is temperature dependant.

Answer 4

True.

Water has a higher ionization at a higher temp.

Question 5

How does Ka differ? (High vs Low)

Answer 5

High Ka = acids dissolve easily

Low Ka = Acid Does not dissolve easily

Question 6

How does a high Kb effect the value?

Answer 6

High Kb means a base dissolves into large products

water reacts with base to form conjugate acid

Question 7

How are Ka and pH values reflected in a strong acid?

Answer 7

They have large Ka values (products increase, and reactants decrease)
Strong acids also produce solutions with low pH

Question 8

How are Kb and pH values reflected in a strong base?

Answer 8

They have large Kb values
Strong bases fully react with water to gain a proton
Strong bases increase pH level

Question 9

How do weak bases and acids differ from Strong ones?

Answer 9

The have a small Ka/Kb value

They also favor reactants over products

Question 10

Which compounds are the strong Acids?

Answer 10

HI, HBr, HCl (Halogen acids)
HNO3, H2SO4
HClO3, HClO4

Question 11

Which compounds are strong bases?

Answer 11

Hydroxides of alkali or alkali earth metals (NaOH, KOH, Ca(OH)2)
NH2-, H-, CH3O-, CH3CH2O-, C2H5ONa

Question 12

What does p mean?

Answer 12

negative logarithum

Question 13

How do you calculate pH?

Answer 13

-log [H3O]

Question 14

Ho do you calculate pOH-?

Answer 14

-log [OH-]

Question 15

How do you calculate pKw?

Answer 15

-log Kw

Question 16

How do you calculate Kw?

Answer 16

[H3O+]x[OH-]

pKw = pH + pOH (@25C)

Question 17

Since pKa/pKb values have a -log, this means they have a _____ relationship to Ka/Kb.

Answer 17

inverse

increase Ka = decreased pKa

Question 18

IN relation to a strong Acid/Base what would the Ka value be?

Answer 18

high Ka/Kb

Question 19

In relation to a weak acid/base, what would the pKa/pKb value be?

Answer 19

High pKa/pKb

Question 20

For nomenclature, how do you name organic acids (compounds that contin Carbon-hydrogen bonds)

Answer 20

-oic

carboxylic acid

Question 21

For nomenclature, how do you name inorganic acids (compounds w/o oxygen or carbon)?

Answer 21

Combine root of parent name with -ic acid as suffix.

Hydroiodic acid

Question 22

For nomenclature, how do you name an oxyacid (inorganic acids that have an oxygen but no carbon)?

Answer 22

The name depends on how many oxygen atoms are present.
The suffix - ic (for compounds that are normally -ate)
the suffix -ous (for compounds that are normally -ite)