Acids, bases, salts and ionization

Question 1

• A water molecule is able to self-ionize.
• In pure water, a very small amount of water molecules ionize into hydrogen (proton) and hydroxide.
  
  • There are always equal parts of H+ and OH- in pure water.
• Therefore the pH of water is neutral (7).

Answer 1

Hydrogen and Hydroxide ions

Question 2

The measurement of H+ in a solution.

• Equal amounts of H+ and OH- is a neutral solution and has a pH of 7.
• pH of less than 7 are acidic, more H+ than OH-
• Less H+ than OH- is a basic solution, pH is greater than 7

Answer 2

pH

Question 3

The amount of H+ in a solution is calculated as a molar concentration.
- 1 mole = 6.023 X 10 to the 23rd.

Answer 3

Determining the pH

Question 4

Compounds that release H+ in a solution.
- Adding this to water will lower the pH.
- Dissociates in water :
HA => A- + H+

Answer 4

Acids

Question 5

Compounds that release OH- in a solution.
- Adding this to water will increase the pH.
- Dissociate in water
- React with water to produce OH-
- General formula:
XOH => X+ + OH-

Answer 5

Bases

Question 6

• Appear as all three states of matter, but liquid is most common.
• Pure molecules are usually dry crystals and are extremely hygroscopic.
• Binary
• Ternary

Answer 6

General properties of acids

Question 7

Pull water out of the air to them.

Answer 7

Hygroscopic

Question 8

Contain H+ and one other non-metal (HCl, HF, HBr)

Answer 8

Binary acids

Question 9

Contain H+, O, and one non-metal radical.

Answer 9

Ternary acids

Question 10

• Also called alkaline compound
• Bitter taste (physical property)
• Bases can appear in all three states, but most commonly found as greasy, slippery, powder form.
• All ternary compounds because they all contain O and a metal.

Answer 10

General properties of bases

Question 11

States that acids dissociate into an aqueous solution to yield H+ and bases dissociate into an aqueous solution to yeild OH-

• The most commonly used biochemical definition for an acid and base.

Answer 11

Arrhenius theory

Question 12

Defines acids as proton donors and bases as proton acceptors.

• Conjugate acid-base pairs differ by a single proton
• Amphorteric compounds can act as either a base or an acid.

Answer 12

Bronstead- Lowery Theory

Question 13

States that an acid is any substance that accepts a pair of electrons and a base is any substance that donates a pair of electrons.

Answer 13

Lewis theory

Question 14

• Acids can be added to basic solutions to decrease the pH
• Bases an be added to acidic solutions to increase the pH
• A neutralization reaction results in a pH of 7.

Answer 14

Acid-base reactions

Question 15

A reaction with the product being a salt and water.

Answer 15

Neutralization

Question 16

Ionic compounds and are neutral in water.

Answer 16

Salts

Question 17

• 2 Ionic compounds are mixed together (acid and base)
• Ionic compounds split apart into their respective anion and cations.
• The cations will swap anions.
• A reaction occurs if, by swapping anions, a product is formed that cannot split apart into anions and cations- or what is known as an insoluble precipitate (salt) or gas.

Answer 17

Double replacement/ Neutralization

Question 18

Contains a metal and a non-metal molecule.

Answer 18

Inorganic salt

Question 19

Joining one metal and one non-metal element.

Answer 19

Binary salt

Question 20

All H+ in the acid have been replaced by a metal.

Answer 20

Normal salt

Question 21

Only some of the H+ in the acid have been replaced by a metal.

Answer 21

Acid salt

Question 22

Contain one or more replaceable -OH.

Answer 22

Basic salt

Question 23

Oxides of metals and non-metals.

Answer 23

Anhydrides

Question 24

Form acids when placed in water.

Answer 24

Acid anhydride

Question 25

Form bases when placed in water.

Answer 25

Basic anhydride

Question 26

Substances that prevent major changes in pH by absorbing excess H+ or OH-. - Maintaining the optimum pH for the organism is part of maintaining homeostasis. - Blood contains these and therefore resist major fluctuations in pH.

Answer 26

Buffers

Question 27

Contain water in their formula. Compounds that have water held in them.

Answer 27

Hydrates

Question 28

Water held within a hydrate.

Answer 28

Water of crystallization

Question 29

Have the water of crystallization removed by dehydration.

Answer 29

Anhydrous

Question 30

- Some hydrates can attract more water from the atmosphere. - hydrophilic or hygroscopic - Deliquescent - Efflorescent - Compounds in the prep room that are known to be hygroscopic or efflorescent need to be kept tightly sealed so water doesn't get in or escape.

Answer 30

Descriptions of hydrates

Question 31

If something can attract so much water from the air that they dissolve.

Answer 31

Deliquescent

Question 32

Spontaneously release water.

Answer 32

Efflorescent

Question 33

Draw moisture from tissue.

Answer 33

Hardening compounds

Question 34

Plaster of paris and gypsum are two different hydrates of this compound.

Answer 34

Calcium sulfate (CaSO4)

Question 35

For the embalmer, you are interested in counteracting this in the biological sense. - It can also occur in inorganic substances such as salts (not all salts) - The properties are the same.

Answer 35

Hydrolysis

Question 36

Double replacement reaction involving salt and water. - Similar to neutralization in that you have an acid and a base (which is neutralized into a salt and water). - Dissimilar because you make an acid and base of different strength. (strong acid and weak base, or weak acid and strong base).

Answer 36

Hydrolysis

Question 37

Allows you to determine the relative strength of an acid or base. - red and blue - The strong member of a hydrolysis solution would cause a change in the litmus paper while the weak would not.

Answer 37

Litmus reactions