Definitions

Question 1

What is a Bronsted acid?

Answer 1

proton donor

Question 2

What is a Bronsted base

Answer 2

proton acceptor

Question 3

expression of ph

Answer 3

Ph = -log[H3O+]

Question 4

calculate Ph concentration

Answer 4

10^-pH

Question 5

Define conjugate base?

Answer 5

It is the species left behind after a bronsted acid has transeferred a proton

Question 6

Define a conjugate acid

Answer 6

It is the species formed after a base accepts a proton

Question 7

What do you call a species that can both donate or accept protons?

Answer 7

Amphiprotic

Question 8

What do you call a species that can donate more than one proton?

Answer 8

polyprotic

Question 9

Define monoprotic acid

Answer 9

It is an acid which can donate ONLY one H+ (proton) to water eg. HCl

Question 10

Define diprotic acid

Answer 10

It can donate up to two protons (H+) to water eg. H2SO4

Question 11

define triprotic acid

Answer 11

It can donate up to three protons to water eg. H3PO4

Question 12

What is Ka?

Answer 12

Acid disscociation constant / or acid ionization constant

Question 13

What is the expression for Ka?

Answer 13

Ka = [A-] *[ H3O+]/ [HA]

Question 14

What is the expression for pKa?

Answer 14

pKa = -log (Ka)

Question 15

What factors are the strength of an acid dependent on?

Answer 15

charge of A
electronegativity of A
the strength of an HA bond
the extentof the delocalisation of of the negative charge on the anion A-

Question 16

What is the autoprotolysis constant of water defined by?

Answer 16

Kw = [H3O+] [OH-]

water reacting by itself

Question 17

In pure water is [H3O+] = [OH-] ?

Answer 17

yes; Kw = square root of Kw

Question 18

What does the Henderson Hasslebach equation state?

Answer 18

pH = pKa + log 10 (A- aq/HA aq)

Question 19

What is a titration?

Answer 19

A method of volumetric analysis used for determining the concentration of an uknown solution by letting it react with another

Question 20

What is the equivalence point?

Answer 20

It is the volume at which the reaction is just completed. In an acid base titration, the pH changes most rapidly at the equivalence point

Question 21

In a titration C1V2 = C2V2 at equivalence point

Answer 21

…

Question 22

Where is the buffer region in a titration involving a weak acid and a strong base

Answer 22

around half way to the equivalence point; at this point ph= pka

Question 23

In a titration involving a weak acid a strong base, what is the pH at equivalence point dependent on?

Answer 23

the pka of the acid and the concentration

Question 24

What is an indicator?

Answer 24

A substance that has different colors in the acid and basic solution

Question 25

What is the indicator usually? is it a weak acid?

Answer 25

yes

Question 26

Where does an indicator change color most rapidly

Answer 26

When pH = Pkln

Question 27

What is Kln?

Answer 27

the acid dissociation constant of that indicator

Question 28

What is the best choice for an indicator?

Answer 28

an indicator whose color changes occurs at the pH of the equivalence point of the titration

Question 29

What is a buffer solution?

Answer 29

a solution whose pH changes much less than that of pure water as we add either acid or base

Question 30

What does a buffer solution typically contain?

Answer 30

approximately equal concentrations of a weak acid and its conjugate base, and its pH is the pKa of the acid

Question 31

How does a zwitterion result?

Answer 31

is the result of an internal proton transfer, such as +NH3CH2CO2-

Question 32

What is the isoelectric point?

Answer 32

the pH at which the majority of the species is the a zwitterion

Question 33

What is electrophoresis?

Answer 33

is the separation of mixtures of amino acids based on their different isoelectric points

Question 34

Acid rain? How does it arise?

Answer 34

arises when gases like SO2, SO3, NO2, etc... are dissolved in rainwater

Question 35

What does it mean by the levelling effect of the solvent?

Answer 35

H3O+ is the strongest acid, and OH- is the strongest base, that can exist when water is the solvent

Question 36

What is a superacid?

Answer 36

It is an acid stronger than pure sulfuric acid

Question 37

What is a superbase?

Answer 37

is a very strong base

Question 38

What happens to the conjugate base of an acid?

Answer 38

it loses an H+ and gains a one more negative charge?

Question 39

What happens to the conjugate acid of a base?

Answer 39

It gains a proton and gains one more positive charge