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Chemistry > Acids and Bases > Flashcards

Acids and Bases Flashcards

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1
Q

2 ways to make a solution

A
  • dissolving a solid
  • diluting a stock/standard
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2
Q

dilution

A

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

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3
Q

dilution factor

A

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

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4
Q

qualitative analysis

A

the identification of the specific substances present

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5
Q

quantitative analysis

A

the measurement of the quantity of a substance present

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6
Q

qualitative chemical analysis

A

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

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7
Q

acids taste

A

sour

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8
Q

bases taste

A

bitter

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9
Q

acid SOLUTIONS conduct electricity T/F

A

T

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10
Q

acids (by themselves) conduct electricity T/F

A

F

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11
Q

bases conduct electricity T/F

A

T

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12
Q

bases feel

A

slippery

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13
Q

acids and litmus paper

A

turns blue litmus paper RED

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14
Q

bases and litmus paper

A

turns red litmus paper BLUE

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15
Q

acids reaction with active metals

A

produces hydrogen gas

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16
Q

bases reaction with active metals

A

no reaction

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17
Q

acids reaction with carbonate compounds

A

produces carbon dioxide

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18
Q

bases reaction with carbonate compounds

A

no reaction

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19
Q

3 types of acid-base theory

A
  • arrhenius theory
  • brosnted-lowry theory
  • lewis theory
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20
Q

arhenius

A
  • 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
21
Q

limitations of arrhenius theory

A
  • 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
22
Q

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

A
23
Q

hydrogen ion H30+ aka hydrogen ion

A
24
Q

amphiprotic/amphoteric

A

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

25
Q

conjugate pairs

A

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

26
Q

conjugate base (of the acid)

A

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

27
Q

conjugate acid (of the base)

A

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

28
Q

ionization

A

the formation of ions from uncharged molecules

29
Q

dissociation

A

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

30
Q

Bronsted-Lowry Theory

A
  • 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

31
Q

monoprotic acid

A

an acid which can supply one one proton

32
Q

diprotic acid

A

acid which can supply up to two protons

33
Q

triprotic acid

A

acid which can supply up to three protons

34
Q

polyprotic acid

A

acid which can supply more than one proton

35
Q

How is acid strength determined?

A

determined by the concentration of H+ ions in solution

36
Q

strong acids

A

ionize > 99% upon dissolving in water

37
Q

What are the strong acids?

A
  • HCl
  • HBr
  • HClO4
    -H2SO4
  • HNO3
  • HI

are all vey good electrolytes because of all the ions in solution

38
Q

weak acids

A

dissociate less than 5% in water

very poor electrolytes because of the low concentration of ions in solution

39
Q

How is base strength determined?

A

by the concentration of OH- ions is solution

the more OH- ions the stronger the base

40
Q

strong bases

A

dissociate 100% upon disssolving in water.

41
Q

strong base examples

A

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

42
Q

Weak Bases

A

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

43
Q

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

A
44
Q

titration

A

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

45
Q

burette

A

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

46
Q

titrant

A

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

47
Q

analyte

A

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

48
Q

equivalence point

A

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

49
Q

endpoint

A

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

Chemistry (21 decks)

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