Vocabulary

Question 1

Arrhenius Acid

Answer 1

Hydrogen ions H +

Question 2

Arrhenius Base

Answer 2

Hydroxide ions OH-

Question 3

Bronsted Acid

Answer 3

Hydrogen Containing substance donates a proton(H+)

Question 4

Bronsted Base

Answer 4

Capable of accepting a proton time

Question 5

Conjugate Base

Answer 5

Species remaining when a Bronsted donates a proton

Question 6

Conjugate acid-Base Pair

Answer 6

Bronsted acid(HNO2) and it’s conjugate base (NO2-)

Question 7

Self ionization of water

Answer 7

Contains H2O molecules and small but equal amounts of H3O+ and OH- ions

Question 8

Water

Answer 8

Behaves as an acid and a base self in auto ionization. 1.0x10-7 concentration in 1 liter.

Question 9

Acidic solution

Answer 9

Concentration of H30+ is greater than the concentration of OH-
ph less than 7

Question 10

Basic or alkaline solution

Answer 10

Concentration of OH- is greater than the concentration of H3O+
ph is greater than 7

Question 11

ph Formula

Answer 11

-log[H+] or [H+]=1x10-ph

Question 12

Cation

Answer 12

Positively charged ion

Question 13

Anion

Answer 13

Negatively charged ion

Question 14

Salts

Answer 14

Compounds I have at least one ionic bond

Question 15

Strong acid and strong bases

Answer 15

Acids and bases that dissociates(ionize) completely when dissolved to form a solution

Question 16

Weak(Moderately weak) Acids and bases

Answer 16

Acids and bases that dissociate (ionize) less than completely when dissolved to form a solution.

Question 17

Buffers

Answer 17

Solutions that resist changes in pH

Mixture of an acid and a salt of an acid.

Question 18

Buffer Capacity

Answer 18

The amount of acid(H+) or base(OH-) that can be absorbed by a buffer without causing a significant change in pH.

Question 19

Molarity

Answer 19

The number of moles of solute per liter of solvent

Question 20

Molarity formula

Answer 20

M= moles of solute

Liters of solution

Question 21

Osmole

Answer 21

Unit of measurement that describes the number of moles of a compound that contribute to the osmotic pressure of a chemical solution

Question 22

Osmolarity

Answer 22

Osmoles of solute per liter of solvent

Question 23

Tonicity

Answer 23

Compare osmolarity of two solutions separated by a semi permeable membrane

Question 24

Isotonic

Answer 24

Solution has the same osmolarity compare to the solution on the other side of the membrane

Question 25

Hypertonic

Answer 25

Solution has a higher osmolarity compared the solution on the other side of the membrane

Question 26

Hypotonic

Answer 26

Solution has a lower osmolarity compared to the solution on the other side of the membrane

Question 27

Neutral

Answer 27

A term used to describe any water solution in which the concentrations of H3O+ and OH− are equal. Also, a water solution with pH = 7.

Question 28

ion-product-of-water

Answer 28

The equilibrium constant for the dissociation of pure water into H3O+ and OH−.

Question 29

ph

Answer 29

The negative logarithm of the molar concentration of H+ (H3O+) in a solution.

Question 30

salt

Answer 30

A solid crystalline ionic compound at room temperature that contains the cation of a base and the anion of an acid.

Question 31

hydrate

Answer 31

A salt that contains specific numbers of water molecules as part of the solid crystalline structure.

Question 32

water-of-hydration

Answer 32

Water retained as part of the solid crystalline structure of some salts.

Question 33

equivalent-of-salt

Answer 33

The amount that will produce 1 mol of positive (or negative) electrical charges when dissolved and dissociated.

Question 34

pka

Answer 34

The negative logarithm of Ka.

Question 35

henderson–hasselbalch-equation

Answer 35

A relationship between the pH of a buffer, pKa, and the concentrations of acid and salt in the buffer.