Acids and Bases

Question 1

2 ways to make a solution

Answer 1

• dissolving a solid
• diluting a stock/standard

Question 2

dilution

Answer 2

the process of reducing the concentration of a solution by adding more solvent

Question 3

dilution factor

Answer 3

the concentration of the diluted solution divided by the concentration of the concentrated solution

Question 4

qualitative analysis

Answer 4

the identification of the specific substances present

Question 5

quantitative analysis

Answer 5

the measurement of the quantity of a substance present

Question 6

qualitative chemical analysis

Answer 6

planning a double displacement reaction that forms a precipitate with a specific compound to detect the presence of an element

Question 7

acids taste

Answer 7

sour

Question 8

bases taste

Answer 8

bitter

Question 9

acid SOLUTIONS conduct electricity T/F

Answer 9

T

Question 10

acids (by themselves) conduct electricity T/F

Answer 10

F

Question 11

bases conduct electricity T/F

Answer 11

T

Question 12

bases feel

Answer 12

slippery

Question 13

acids and litmus paper

Answer 13

turns blue litmus paper RED

Question 14

bases and litmus paper

Answer 14

turns red litmus paper BLUE

Question 15

acids reaction with active metals

Answer 15

produces hydrogen gas

Question 16

bases reaction with active metals

Answer 16

no reaction

Question 17

acids reaction with carbonate compounds

Answer 17

produces carbon dioxide

Question 18

bases reaction with carbonate compounds

Answer 18

no reaction

Question 19

3 types of acid-base theory

Answer 19

• arrhenius theory
• brosnted-lowry theory
• lewis theory

Question 20

arhenius

Answer 20

• describes acitivies of acids and bases dissolved in water
• acids ionize/dissociate in aqueous solution to increase H+ ion concentration
• bases ionize/dissociate in aqueous solution to increase OH- concentration

Question 21

limitations of arrhenius theory

Answer 21

• occurs in aquous solution, but water is often left out, but water is a polar molecule and must interact with the ions in some way
• ammonia produces a basic solution but does not contain OH- ions, ammonia also neutralizes acids
• limited to reactions in water
• cannot explain why salts that concain arbonate ions also have basic properties

Question 22

H+ DO NOT exist is water solution but are snatched up by water molecules ro form hydronium ions

Question 23

hydrogen ion H30+ aka hydrogen ion

Question 24

amphiprotic/amphoteric

Answer 24

compounds that can act as either an acid or a base depending on the chemical reaction

Question 25

conjugate pairs

Answer 25

two molecules or ions that differe because of the transfer of a proton

Question 26

conjugate base (of the acid)

Answer 26

the particle that remains when a proton is removed from the acid

Question 27

conjugate acid (of the base)

Answer 27

the particle formed when the base receives the proton of the acid

Question 28

ionization

Answer 28

the formation of ions from uncharged molecules

Question 29

dissociation

Answer 29

the seperation of individual ions from an ionic compounds as it dissolves inw water (started charged)

Question 30

Bronsted-Lowry Theory

Answer 30

* includes all arrhenius acids + bases* acids = a substance from which a proton (H+ ion) can be removed bases = a substance that can remove a proton (H+ ion) from an acid

Question 31

monoprotic acid

Answer 31

an acid which can supply one *one* proton

Question 32

diprotic acid

Answer 32

acid which can supply up to *two* protons

Question 33

triprotic acid

Answer 33

acid which can supply up to *three* protons

Question 34

polyprotic acid

Answer 34

acid which can supply more than one proton

Question 35

How is acid strength determined?

Answer 35

determined by the concentration of H+ ions in solution

Question 36

strong acids

Answer 36

ionize > 99% upon dissolving in water

Question 37

What are the strong acids?

Answer 37

- HCl - HBr - HClO4 -H2SO4 - HNO3 - HI are all vey good electrolytes because of all the ions in solution

Question 38

weak acids

Answer 38

dissociate less than 5% in water very poor electrolytes because of the low concentration of ions in solution

Question 39

How is base strength determined?

Answer 39

by the concentration of OH- ions is solution the more OH- ions the stronger the base

Question 40

strong bases

Answer 40

dissociate 100% upon disssolving in water.

Question 41

strong base examples

Answer 41

oxides and hydroxides of group 1 metals and all group 2 metals below berllium bery good electrolytes because of alll the ions in the solution

Question 42

Weak Bases

Answer 42

dissociate much less than 100% upon dissolving in water, poor electrolytes

Question 43

strong and weak refer to the % of ionization of dissociation of particles in water, concetrated and dilute refer to the amount of solute in a solvent

Question 44

titration

Answer 44

an analytical procedure used in chemistry to determine the concentration of an unknown acid or base, uses a neutralization reaction and stoichiometry to calculate the concentration of the unknown solution

Question 45

burette

Answer 45

a calibrated (has accurate volume markings) tube used to deliver variable known volumes of a solution during a titration

Question 46

titrant

Answer 46

the solution in the burette during the titration (most often the solution of known concentration)

Question 47

analyte

Answer 47

the solution in the Erlenmeyer flask during the titration most often the solution of unknown concentration

Question 48

equivalence point

Answer 48

the point in a titration when the quantity of acid has exactly neutralized the quantity of base

Question 49

endpoint

Answer 49

the point during a titration in which an observable change (usually colour change) caused by a significant change in pH has occured, signifying that the equivalence point has been reached