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Chemistry 2 > Final > Flashcards

Final Flashcards

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1
Q

Acids

A

Can dissolve metals and neutralize bases

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2
Q

Base

A

Neutralize acids

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3
Q

Strong acids

A

Dissociates completely in water( no equilibrium)

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4
Q

What are the 6 strong acids and the extra one

A

HCl, H2SO4, HNO3, HBr, HI, HCLO4,!
(H3O+ is also a strong acid)

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5
Q

Strong base definition

A

Dissociates completely in water( no equilibrium)

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6
Q

What are the strong bases

A

NaOH, KOH, LiOH, RbOH, Ba(OH)2

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7
Q

What group is strong bases

A

Group 1 and 2 metals and hydroxide

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8
Q

Arrhenius (acids)

A

Substances that, when dissolve in water increases [H+]

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9
Q

Arrhenius( bases)

A

Substances that dissolve completely in water,[OH-]

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10
Q

Bronsted -Lowry (Acid)

A

Proton donor and must have a removable(acidic) proton (H+) that can separate H in front

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11
Q

Bronsted-Lowry (bases)

A

Proton acceptor and must have a pair of no binding electrons

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12
Q

Definition Amphoteric species

A

Can act as an acid or base

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13
Q

Example of amphoteric species

A

Water

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14
Q

Conjugate acid

A

Has a base

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15
Q

Conjugate base

A

Acid

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16
Q

Conjugate is on which side

A

Product side

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17
Q

H3O+ will never be a base or acid

A

Base

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18
Q

OH- will never be a acid or base

A

Acid

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19
Q

Polyprotic acid

A

Acid that has more than one H+ to donate

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20
Q

Examples of polyprotic acid is

A

H2SO4, H3BO3, H3PO4

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21
Q

What is the [H+] of a 0.25 M of a HCL solution

A

0.25 ( because it’s a strong)

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22
Q

What is the [OH-] of a 1.3 Msolution of NaOH

A

1.3 M

23
Q

Ka

A

Acid

24
Q

kB

A

Bases

25
Q

List acids by increasing strength

A

Larger Ka

26
Q

Auto ionization

A

When water acts as an acid or base with itself

27
Q

Equilibrium expression (calculate OH- if [H+] is 7.5x10^-5

A

KW=(H+)(OH-)
=KW/[H+]=OH-

28
Q

The solution is basic if

A

[OH] is greater

29
Q

The solution is acidic if

A

(H+) is greater

30
Q

The solution is neutral if

A

They are the same

31
Q

pH<7 it’s

A

Acidic

32
Q

pH>7

A

Is basic

33
Q

To find it it’s acidic basic or just rap you look at the..

A

pH

34
Q

Weak base is

A

A anion that is a conjugate base of a weak acid

35
Q

A strong acid or neutral idk how to put this

A

An anion that is the conjugate base of a strong acid is neutral

36
Q

Solution is an acid when

A

H+ is bigger

37
Q

Solution is basic when

A

OH is bigger

38
Q

Buffer system

A

Aqueous solution that contains a weak acid or base and it’s conjugate

39
Q

What does a buffer system do?

A

It resist a large changes in pH by neutralizing strong acid or base pair. The weka acid neutralizes an incoming strong base and the weka base neutralize an incoming strong acid

40
Q

Buffer is written

A

Weak Acid and conjugate base( don’t worry about the cation)

41
Q

Effective buffer (3)

A

-Most resistant to pH changes
- high concentration of acid and conjugate base)
-close to an equal amount of acid and conjugate base

42
Q

Titration

A

Determining a concentration of an unknown

43
Q

PH meter

A

Device that measures voltage and converts H+ into solution

44
Q

To find pH

A

Use the sigmoidal curve to find at the equivalence point

45
Q

Equivalence point

A

MolesA= molesB

46
Q

Equivalence point of a strong acid/strong base will be at

A

7

47
Q

Indicator

A

A substance usually a weak acid that undergoes a color change at a specific pH range

48
Q

Endpoint

A

Just after the equivalence point and a great estimator for equivalence point

49
Q

Neutralization

A

Base react with a acid to make water

50
Q

If acid is strong pH is

A

Ph at equivalence point will be below 7

51
Q

If base is strong ph at equivalence point Is

A

Above 7

52
Q

What is a soluable compound

A

When a compound can be slightly soluable

53
Q

Solubility in rice tables is

A

X

Chemistry 2 (3 decks)

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