Chem Acids/ Bases

Front 1

Bronsted Acid

Back 1

Proton Donor

Front 2

Bronsted Base

Back 2

Proton Acceptor

Front 3

Lewis Acid

Back 3

Electron pair acceptor

Front 4

Lewis base

Back 4

electron base donor

Front 5

Autoionization

Back 5

self ionizing; means that water reacts with itself

Front 6

Kw (Autoionization constant)

Back 6

[H3O][OH]=1 x 10^-14 @ 25 degrees

than means each one is 1 x 7^-14

Front 7

pH

Back 7

-log[H+]

Front 8

Estimating pH

Back 8

if its 1 x 10^-4, pH is 4. You take the negative of the exponent.

However, if its a number bigger than one, something like 5 x 10^-6, you have to take the negative of the exponent and just subtract one.

Front 9

Any dilution on the mcat of an acid or a base:

Back 9

the solution always moves toward the neutral pH of 7 and will not move more than 1 pH unit. That will be your answer

Front 10

Strong Acid

Back 10

Completely dissociates

Front 11

6 Strong acids

Back 11

HCl

HI

Hbr

H2SO4:Sulfuric Acid

HNO3:Nitric Acid

HClO4: Perchloric Acid

Front 12

Strong Bases

Back 12

1.) All Group 1 oxides and hydroxides

Examples: NaOH or Li2O

2.) some group 2 hydroxides (strontium, calcium, barium)

2.) Some metal amides (NaNH2)

Front 13

Weak acid

Back 13

does not completely dissociate

Front 14

Ka

Back 14

[H+][A-] / HA

basic means more acidic

Front 15

Kb

Back 15

[OH-][HB] / B

bigger means more basic

Front 16

(Ka x Kb)=

Back 16

10 ^-14 For acid base pairs (conjugate pairs)

Front 17

pKa + pKb=

Back 17

14 for acid base pairs (conjugate pairs)

Front 18

Conjugate pair

Back 18

The acid and its conjugate base after removal of a proton

Front 19

Conjugate Rules

Back 19

1.) The conjugate of any strong acid or base is pH neutral; the conjugate base of a strong acid has no basic properties; vice versa

2.) The conjugate of any WEAK acid or base is a weak base or acid; the stronger the weak acid or base, the weaker its conjugate

Front 20

For a strong acid or base, what is the H+ or OH- concentration always equal to?

Back 20

the solution concentration; pH can easily be found from the concentration

Front 21

Quick way to find pH of solution if they give concentration of a weak acid or base solution

Back 21

Ka= x^2 / [Initial concentration]

value of x will be H+ concentration which you can use to find pH

Front 22

Neutralization Reaction

Back 22

When acid and base react, they form a salt and water every time. (strength of either acid or base does not matter)

Reaction is always exothermic and always goes to completion when equal molar amounts of base and acid are used

Ex:

HCl + KOH --> KCl + H2O

Front 23

Equation for Neutralization reaction

Back 23

(a)(Volume of A)[concentration of A]=(b)(volume of B)[Concentration of B]

a= number of acid protons that can be donated

b= number of protons that can be accepted

Front 24

pH after neutralization reaction

Back 24

pH of the resulting solution is determined by the type of salt formed.

If the anion of the salt is inactive in water, the solution is pH neutral and thus it is the conjugate base of a strong acid.

If the cation is group 1 or 2 cation it will have no effect on pH

If the cation is more acidic than H2O, then it is the conjugate acid of a weak base and the pH will be acidic.

If the anion is more basic than water, then it is the conjugate base of a weak acid.

Front 25

Buffer Solution

Back 25

Resist a change in pH when a small amount of acid or base is added

To make a buffer, combine a weak acid or base and its conjugate in roughly equal amounts

Front 26

Henderson Hasselback equation (shortcut to find pH of buffer solution)

Back 26

pH= pKa + log [A-]/[HA]

poH= pKb + log [HB+]/[B]

Front 27

How to pick a buffer

Back 27

Always pick a buffer with a pKa close to the pH that you are trying to maintain

However, if a buffer solution is diluted, the pH is unchanged

Front 28

Indicator

Back 28

weak acid or base that changes color when it changes into its conjugate

Front 29

Always pick an indicator with a pKa close to the pH you want to indicate

Back 29

YUH

Front 30

Titration

Back 30

used to determine an unknown acid or base by determining its pKa or pKb

Front 31

Procedure for titration

Back 31

Add a titrant (strong acid or base of known concentration) to the unknown in a dropwise fashion

Record the pH changes and plot the results

Graph looks like a muthfuckin S nigga

Front 32

Titration Curve

Back 32

Front 33

Equivalence point

Back 33

Concentration of [H+] is equal to concentration of [OH-]

all acid is neutralized

Front 34

Half Equivalence point

Back 34

Half of acid is neutralized; [HA] = [A-]

pH = pKa of unknown

Uknown is found using this point

Front 35

What determines the pH of the equivalence point?

Back 35

the salt formed

Front 36

Buffering domain

Back 36

Part of titration curve where pH changes very slowly