Acids/bases And Salts, Ph And Buffers

Front 1

Acid, bases, and salts are the principal families of ?

Back 1

ionic compounds

Front 2

Acids, bases, and salts undergo what in aqueous solutions?

Back 2

ionization

Front 3

Definition of ionization

Back 3

process in which ions form from neutral particles

Front 4

Ionization of water, formula

Back 4

2H20 --- H3O + OH

Front 5

Ionization of water, what reaction is not favored at 25 C?

Back 5

Forward reaction, produces a pure water or a neutral solution, pH=7.0

Front 6

Acidic solution: H3O is ____ than OH?

Back 6

>

Front 7

Basic solution: H30 is ____ than OH?

Back 7

<

Front 8

Acid-base neutralization

Back 8

acids and bases can combine, in the appropriate molar concentrations to produces a neutral solution

Front 9

Example of acid-base neutralization

Back 9

HCl + NaOH -- NaCl + H2O
acid + base ---- salt + water

Front 10

What is formed by the neutralization reaction?

Back 10

A salt

Front 11

Definition of a salt

Back 11

an ionic compound consisting of any positive ion except H3O and any negative ion except OH or O2

Front 12

All salts are __________ at room temperature

Back 12

crystalline solids

Front 13

Bronsted definition of an acid

Back 13

an acid is a substance that donates H+ to solution
-the H+ is a naked proton and is strongly attracted to electrons
-H+ is always held by an electron-pair bond to something, eg, as H3O+

Front 14

What terms are used interchangeably to descibe a proton?

Back 14

proton, hydrogen ion, and hydronium ion, in other words H+ is understood to be H3O+.

Front 15

Bronsted definition of a base

Back 15

a base is a substance that accepts and binds H+
-the base has an electron pair available to bind H+

Front 16

Strength of an acid in aqueous solution

Back 16

refers to the extent to which the acid ionizes to yield H+

Front 17

strong acid

Back 17

essentially 100% ionized in water

Front 18

Monoprotic acids

Back 18

ratio of H+ to anion is 1:1(donate a single proton)

Front 19

What are 4 common strong monoprotic acids

Back 19

HCl, HBr, HI, HNO3

Front 20

Describe diprotic acids, name 1 strong diprotic acid.

Back 20

donate two H+, H2SO4

Front 21

Weak acid & name 1 monoprotic weak acid and 1 diprotic weak acid

Back 21

only a small percentage of acid molecules ionize
eg, monoprotic: acetic acid, diprotic:carbonic acid

Front 22

Carbonic acid exists where?

Back 22

only where CO2 is dissolved in water

Front 23

Ionization constant

Back 23

Ka and pKa

Front 24

Ka values are used to ?

Back 24

compare the strengths of weak acids, the weaker the acid the smaller the Ka

Front 25

pKa =

Back 25

-log Ka

Front 26

What is used more frequently pKa or Ka to compare strengths of weak acids?

Back 26

pKa

Front 27

The larger the pKa value, the ______ the acid.

Back 27

weaker

Front 28

A base is a proton acceptor, in water the strongest proton acceptor is.....? and why?

Back 28

-OH, available electrons to accept the proton

Front 29

Name one strong base

Back 29

NaOH

Front 30

A strong base is an ionic hydroxide that undergoes ...?

Back 30

essentially 100% ionization to yield -OH

Front 31

A weak base is a _____ ______ ionic hydroxide or a substance that reacts slightly with water to yield -OH

Back 31

poorly soluble

Front 32

Examples of weak bases

Back 32

Mg(OH)2, Ammonia NH3, Bicarbonate ion HCO3

Front 33

Molecular equation

Back 33

conventional equation for a reaction, shows molecular formulas of substances

Front 34

Ionic equation

Back 34

Expansion of a molecular equation, shows all dissolved species

Front 35

What are spectator species?

Back 35

nothing happens to them so they cancel out of the equation

Front 36

What is a net ionic equation then?and what must it have?

Back 36

It is the equation without the spectator species, must have material and electrical balance

Front 37

If you add -OH to a weak acid what can happen?

Back 37

the acid may completely ionize

Front 38

If you add -OH to a strong acid what happens?

Back 38

no change, already ionized 100%

Front 39

If you add -OH to water-insoluble metal hydroxides what happens?

Back 39

all the metal hydroxide may dissolve

Front 40

All metal bicarbonates react with strong acids to yield?

Back 40

CO2, water and a salt

Front 41

Why is reactions of metal bicarbonate ions with acids important in the human body?

Back 41

removes H+ from the extracellular fluid

Front 42

What is one means of excreting H+ in the urine? From what reaction?

Back 42

combination of NH3 and H+
-reaction of NH3 with aqueous acids

Front 43

Reactions of metals with acids, products are usually? and what type of reaction is this?

Back 43

hydrogen gas and a salt, redox reaction

Front 44

Activity series of metal reactivity with acids

Back 44

1. Metals above hydrogen in the series react with acids; metals below hydrogen in the series do not react with acids
2. Group 1A metals can remove H+ from pure water; no acid needs to be present

Front 45

How are ion concentrations in solution expressed?

Back 45

as equivalents (or mEq) per L

Front 46

Defintion of an equivalent

Back 46

one eq of an ion is the amount of the ion (in grams) that carries Avogadro's number (one mole) of electrical charge (positive or negative)

Front 47

One eq of a univalent ion is the same as the?

Back 47

molar mass of the ion
Na+ 23g/mole 1eq of Na=23.0g

Front 48

The eq of a polyvalent ion is what?

Back 48

its molar mass divided by the absolute value of its valence
eg, one eq of Ca+2 is 20.1g (40.2 g divided by 2;0.5 mole of Ca+2)

Front 49

Biological fluids are usually expressed in?

Back 49

meq per liter

Front 50

Solutions of ions are electrically?

Back 50

neutral, eq of positive charge=eq of negative charge

Front 51

Defintion of anion gap

Back 51

meq Na+/L- (meq Cl/L + meq HCO3/L)

Front 52

What does the anion gap account for?

Back 52

difficult to measure anions in plasma (eg, negative charges on plasma proteins, organic acids); bicarbonate and chloride are easily measured

Front 53

What is a normal anion gap?

Back 53

5-11meq/L

Front 54

Electrolytes disturbances may do what to the anion gap?

Back 54

widen the gap because organic anions increase in concentration

Front 55

Anion gap is useful for the differential diagnosis of ?

Back 55

metabolic acidosis
-poorly controlled diabetes-DKA
-severe exercise- lactate accumulates

Front 56

Simple salt

Back 56

made of only two kinds of ions
eg, NaCl, CuSO4

Front 57

Mixed salt

Back 57

has three or more different ions

Front 58

Formation of a salt, 3 options

Back 58

1. Acid+metal hydroxide--salt +water
2. acid+metal bicarbonate ---salt + water + carbon dioxide
3. acid + metal -- salt + hydrogen gas

Front 59

defintion of pH

Back 59

-log[H]

Front 60

[H+] is the?

Back 60

molar concentration

Front 61

pH of pure water?

Back 61

at 25C, [H+]= 1.0 x 10 (-7)
pH = -log (10-7) = 7.00

Front 62

pH of 7.00 corresponds to a?

Back 62

neutral solution

Front 63

pH of acidic solution?

Back 63

ph < 7.00

Front 64

When [H+] > 1M, the pH concept?

Back 64

is not used

Front 65

pH of basic solution?

Back 65

ph >7.00

Front 66

A change of one pH unit represents a?

Back 66

10-fold change in [H+], logarithmic scale

Front 67

In some cases, donated ions other than H+ or -OH can alter the pH of a solution, what happens?

Back 67

one of the ions of a salt reacts with water (hydrolysis of the ion) to yield H+ or -OH

Front 68

Anions of ________ hydrolyze in water and tend to make a solution ______. Example of a ______?

Back 68

weak acids, basic
-Sodium bicarbonate

Front 69

When anions of weak acids hydrolyze in water and tend to make a solution basic, what reaction is not favored?

Back 69

a forward reaction, but does occur to a small extent, generating hydroxide ions and forming a basic solution

Front 70

Ammonium ion hydrolyzes to make a solution?

Back 70

acidic

Front 71

pH of 0.10M ammonium chloride solution is?

Back 71

5.1

Front 72

Buffers

Back 72

solutions whose components resist large changes in pH when strong acids or bases are added to the solution

Front 73

What do the two components of a buffer system do?

Back 73

one component can act to neutralize hydrogen ions, the other component can act to neutralize hydroxide ion

Front 74

What type of solution act as buffers?

Back 74

solutions containing a weak acid and a salt (congugate base) of the weak acid

Front 75

What does the Henderson-Hasselbach equation predict?

Back 75

the pH of a buffer solution

Front 76

What are two buffers in the body?

Back 76

CO2/ bicarbonate system
Phosphate buffer

Front 77

What is the principal extracellular buffer?

Back 77

CO2/bicarbonate

Front 78

What is the principal intracellular buffer?

Back 78

Phosphate buffer