Unit 8 - Acids and Bases

Question 1

What is the balanced chemical equation of autoionization of water?

Answer 1

2H2O H3O+ + OH-

Question 2

What is the equilibrium constant of pure water at 25 degrees Celsius?

Answer 2

1 * 10^-14

Question 3

Kw is equivalent to…

Answer 3

[H3O+][OH-]

Question 4

The “p” in pH means…

Answer 4

to take the -LOG of the measurements that follow

Question 5

In acidic solutions, ….

Answer 5

[H3O+] > [OH-]

Question 6

In basic solutions, ….

Answer 6

[H3O+] < [OH-]

Question 7

In neutral solutions, ….

Answer 7

[H3O+] = [OH-]

Question 8

The pH scale measures …

Answer 8

the relative concentrations of H3O+ and OH-

Question 9

As the concentration of H3O+ increases, the pH

Answer 9

decreases

Question 10

What is the chemical formula for hydroxide ion?

Answer 10

OH-

Question 11

What is the chemical formula for hydronium ion?

Answer 11

H3O+

Question 12

In a pH of 7.345, the “7” represents …

Answer 12

the magnitude

Question 13

In a pH of 7.345, the “345” represents ….

Answer 13

the measurement

Question 14

From [H3O+] to pH …

Answer 14

[H3O+] = 10 ^ -pH

Question 15

From pH to [H3O+] …

Answer 15

pH = -log [H3O+]

Question 16

From [OH-] to pOH …

Answer 16

[OH-] = 10^-pOH

Question 17

From pOH to [OH-] …

Answer 17

pOH = -log [OH-]

Question 18

At 25 degrees Celsius, 14 is equivalent to…

Answer 18

pH + pOH

Question 19

At 25 degrees Celsius, 1 * 10^-14 is equivalent to

Answer 19

[H3O+][OH-]

Question 20

Pkw at 25 degrees Celsius is …

Answer 20

14

Question 21

If [H3O+] has a coefficient of 1, then the pH is …

Answer 21

absolute value of the exponent.

Question 22

If [H3O+] has a coefficient other than 1, then the pH is…

Answer 22

absolute value of the exponent minus one

Question 23

The autoionization of water is an _________ process.

Answer 23

ENDOTHERMIC

Question 24

As the temperature increases, the equilibrium constant will ….

Answer 24

Increase as well.

Question 25

Kw increases with temperature because ...

Answer 25

reaction shifts to form products and consume reactants | Products = [H3O+][OH-}

Question 26

In pure water how does the concentration of OH- and H3O+ compare?

Answer 26

In PURE WATER [OH-} is EQUAL to {H3O+]

Question 27

Kw is equal to....

Answer 27

10 ^ -pKW

Question 28

pKw is equal to ...

Answer 28

-log [Kw]

Question 29

As temperature increase , the pH of pure water ...

Answer 29

Decreases

Question 30

How do we determine whether a solution is acidic, basic, or neutral at temperatures other than 25 degrees Celcius?

Answer 30

By comparing the concentrations of hydroxide to hydronium ion

Question 31

Strong acids are assumed to ....

Answer 31

dissociate completely unless otherwise stated

Question 32

Strong acids examples

Answer 32

``` HCl HBr HI HClO4 HClO3 HNO3 first H in H2SO4 ```

Question 33

Strong acid dissociation

Answer 33

HCl + H2O --> Cl- + H3O+

Question 34

In pure water at 25 degrees Celsius, the concentration of OH- and H3O+ is equivalent to...

Answer 34

1.0 * 10 ^ -7 M

Question 35

Strong bases are assumed to ...

Answer 35

dissociate completely unless otherwise stated

Question 36

Strong acids dissociate in water to produce ...

Answer 36

H3O+ ions

Question 37

Strong bases to dissociate in water to produce ...

Answer 37

OH- ions

Question 38

The net ionic equation for the mixing a strong acid and strong base is ....

Answer 38

OH- + H+ --> H2O

Question 39

The neutralization reaction for mixing a strong acid and strong base is ...

Answer 39

Strong acid + Strong Bases ---> Water + Salt

Question 40

Group 1 hydroxides include ...

Answer 40

Oh

Question 41

Group 2 hydroxides include ...

Answer 41

Oh

Question 42

When acids dissociate, only one ...

Answer 42

"H' is dissociate at a time.

Question 43

[H3O+] is also known as ...

Answer 43

H+

Question 44

pH < pKa

Answer 44

acid has a higher concentration in the original solution

Question 45

pH > pKa

Answer 45

conjugate acid has a higher concentration in the original solution

Question 46

acid-base indicator

Answer 46

any substances that exhibit different properties in protonated/ deprotonated states RESPOND to pH

Question 47

Equivalence point

Answer 47

of moles of titrant added is EXACTLY sufficient to react completely with # of moles of titrated species

Question 48

End point

Answer 48

point in titration at which indicator undergoes its color change

Question 49

At the equivalence point pKa can be determined by...

Answer 49

taking the -log of Ka

Question 50

At the equivalence point pKb can be determined by...

Answer 50

taking the -log of Kb

Question 51

A titration graph of a weak acid titrated with a strong base looks like ....

Answer 51

forward "S"

Question 52

A titration graph of a weak base titrated with a strong acid looks like...

Answer 52

backward "S"

Question 53

Molecular structure of stronger acids

Answer 53

weak H-X bond where X is another element

Question 54

Molecular structure of weaker acids

Answer 54

strong H-X bond where X is another element

Question 55

Oxoacids/ Oxyacids

Answer 55

Contain an atom bonded to one or more oxygen atoms

Question 56

inductive effect

Answer 56

Attraction of electrons in adjacent bonds by more electronegative atoms

Question 57

Strong acids experience an inductive effect due to ...

Answer 57

highly ELECTRONEGATIVE oxygen atoms

Question 58

Polarity in strong acids draw electrons ....

Answer 58

AWAY from H- atom causing an EASIER IONIZATION

Question 59

Weak acids do not experience a

Answer 59

STRONG induced dipole force

Question 60

Polarity in weak acids are ....

Answer 60

less than in strong acids -> stronger bond between H+ and oxygen atom -> LESS IONIZABLE

Question 61

If conjugate bases are less stable then...

Answer 61

a stronger base will result

Question 62

Stronger acids results in ...

Answer 62

Weaker bases