Water, Acids And Bases, And Buffers

Front 1

Is a polar Molecule consisting of two hydrogen atoms and one oxygen atom

Back 1

Water

Front 2

Properties of Water

Back 2

1. Water is Polar

2. Water is an excellent solvent

3. Water has high heat capacity

4. Water has high heat of vaporization

5. Water has cohesive and Adhesive Properties

6. Water is less dense as a solid than as a liquid

Front 3

It is the universal solvent

Back 3

Water

Front 4

Why is water essential?

Back 4

1. It is the universal Lubricant

2. Water is cohesive

3. Water supports cellular structure

4. Water as a Lubricant and Cushion

Front 5

Water allows everything inside cells to have the right shape at the Molecular level.

Back 5

Water supports Cellular Structure

Front 6

Water molecules have strog cohesive forces due to their ability to form hydrogen bonds with one another

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Water is Cohesive

Front 7

Because water is polar, with slight positive and negative charges, ionic compounds and polar molecules can readily dissolve in it

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It is the universal solvent

Front 8

A substance or object that absorbs and dissipates heat but does not experience a corresponding increase in temperature.

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Water as a heat sink

Front 9

Water absorbs the heat generated by chemical reactions without greatly increasing in temperature

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Water as a heat sink

Front 10

For cells in the body to survive, they must be kept moist in a water based liquid called

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Solutions

Front 11

Like salts, disssociate in water into electrolytes

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Acids and Bases

Front 12

Can very much change the properties of the solutions in which they are dissolved

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Acids and Bases

Front 13

A substance that releases hydrogen ions (H+) in solution

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Acid

Front 14

Are compounds that release all of their H+ in solution: that is, they ionize completely

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Strong Acid

Front 15

Do not ionize completely; that is, some of their hydrogen ions remain bonded within a compound in solution

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Weak Acids

Front 16

Example of Weak Acid

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Vinegar, or Acetic Acid

Front 17

Is a substance that release hydroxyl ions (OH-) in solution or one that accepts H+ already present in solution

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Base

Front 18

Release most or all of their hydroxyl ions

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Strong Bases

Front 19

Release only some hydroxyl ions or absorb only a few H+

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Weak Bases

Front 20

Is any substance that in water solution taste sour, changes blue litmus paper to red

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Acid

Front 21

Is a molecule or ion able to accept hydrogen ion

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Base

Front 22

Taste Sour

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Acid

Front 23

Do not feel slippery

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Acid

Front 24

Release hydrogen ions in aqueous solution

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Acid

Front 25

Corrodes metals

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Acid

Front 26

React with metals to produce a compound and hydrogen gas

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Acids

Front 27

Turns litmus paper red/pink

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Acid

Front 28

Taste bitter

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Base

Front 29

Feel slippery

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Base

Front 30

pH higher 7

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Base

Front 31

Releases hydroxide ion's in aqueos solution

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Base

Front 32

Do not corrode metals

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Base

Front 33

Do not react with metals to produce a compound And hydrogen gas

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Base

Front 34

Turns litmus paper blue

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Base

Front 35

pH lower than 7

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Acid

Front 36

This theory was limited to substances with those "parts"; ammonia is a major exception

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Arrhenius Definition

Front 37

Acid donates a hydrogen ion in water

Base donates hydroxide ion in water

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Arrhenius Definition

Front 38

Donates Hydrogen ion in water

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Acid

Front 39

Donate hydroxide ion in water

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Base

Front 40

Donates Proton in Water

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Bronsted-Lowry Acid

Front 41

Accepts proton in water

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Bronsted-Lowry Base

Front 42

Acid donates proton in water

Base accepts proton in water

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Bronsted-Lowry Definition

Front 43

This theory is better; it explains ammonia as a base!

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Bronsted-Lowry Definition

Front 44

This is the main theory that will be used in the doscussions

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Bronsted-Lowry Definition

Front 45

Accepts an electron pair

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Acid

Front 46

Donates an electron pair

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Base

Front 47

Acid accepts an electron pair

Base donates an electron pair

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Lewis definition

Front 48

This theory explains all traditional acids and bases plus a host of coordination compounds and is used widely in organic chemistry.

Back 48

Lewis Definition

Front 49

Uses coordinate covalent bonds.

Back 49

Lewis Definition

Front 50

The product that accepted Proton

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Conjugate Acid

Front 51

The product that Donated proton

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Conjugate base

Front 52

A species that has the potential to act both as an acid and s a base

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Amphiprotic Character

Front 53

Water is an ___________ substance that can act either as an acid or a base

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Amphiprotic

Front 54

The reaction of an acid and a base, which forms water and a salt

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Neutralization

Front 55

When acids and bases react they form _____ and ____

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Water and Salt

Front 56

Most ionic compounds can actually be considered ____

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Salts

Front 57

Are typically crystalline, ionic material

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Salts

Front 58

Is a chemical reaction where a compound breaks into two or more components

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Dissociation

Front 59

When NaCl is dissolved in water. It breaks up into Na+ and Cl- ion.

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Ionization

Front 60

Is the process by which atoms or molecules get positive or negative charge

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Ionization

Front 61

Formations of ion

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Ionization

Front 62

Occurs when an atom or a molecule gains or loses an electron

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Ionization

Front 63

Always formed ions in the end

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Ionization

Front 64

The breakdown of substance into smaller particles such as atoms, ions and molecules

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Dissociation

Front 65

Formation of small constitutes from larger compounds

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Dissociation

Front 66

Occurs with the addition of solvent and the addition of energy in the form of heat

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Dissociation

Front 67

Forms atoms, ions or molecules that are smaller than the starring material

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Dissociation

Front 68

Quantitative measure of the acidity or basicity of aqueous or other liquid solutions

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pH

Front 69

Is a solution that can resist pH change upon the addition of acidic or basic components

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Buffers

Front 70

Is a solution of a weak acid and its conjugate base

Back 70

Buffer

Front 71

Can neutralize small amounts of acids and bases in our body

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Buffer

Front 72

If a decrease below 7.35 in the pH of bodily fluid, the buffer in the fluid will act as

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A weak base

Front 73

If an increase above 7.45 in the pH of bodily fluid, the buffer in the fluid will act as

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Weak acid

Front 74

H2CO3

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Carbonic Acid

Front 75

HCO3

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Bicarbonate ion system

Front 76

A component of buffering system of blood. Hydronium ions are removed preventing the pH of Blood becoming acidic

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Carbonic Acid

Front 77

When any substance enter the bloodstream, the bicarbonate ions neutralize the hydronium ion forming ---------- ---- and -----

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Carbonic acid and Water

Front 78

When a basic substance enters the blood stream, carbonic acid reacts with hydroxide ions producing ----------- ---- and -----

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Bicarbonate ions and water

Front 79

The pH human blood normally ranges from

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7.4

Front 80

Can reduce the acidity resulting from the carbon dioxide constantly released into the bloodstream by the trillions of cells in the body

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Blood

Front 81

Acids called ketones are produced as a form of body fuel. These can build up in the blood, causing serious conditions called

Back 81

Diabetic Ketoacidosis

Front 82

A condition in which the blood and other body fluids are too alkaline (basic)

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Alkalosis