Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Copy - IB Chemistry > Acids and Bases > Flashcards

Acids and Bases Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

bronsted-lowry acid

A

proton (H+​) donator

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

bronsted lowry base

A

proton (H+​) acceptor

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

conjugate acid base pairs

A

HA + B –> A- + BH+

  • conjugate acid-base pair
  • conjugate acid-base pair

differ by one proton

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

amphiprotic

A
  • substance that can act as both a proton donator and a proton acceptor
  • must have a lone pair of electrons and hydrogen that can be released as H+​
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

alkali

A

bases that dissolve in water to form the hydroxide ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

salt

A
  • ionic compound formed when the hydrogen of an acid is replaced by a metal or another positive ion
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

parent acid/base

A

e.g. NaCl derived from acid HCl and base NaOH

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

acid + metal –>

A

salt + hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

acid + carbonate –>

A
  • salt + water + carbon dioxide
  • effervescence
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

acid + base –>

A

salt + water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Neutralization

A
  • reaction that occurs when an acid and base react together to form salt and water
  • exothermic
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

enthalpy of neutralization

A

enthalpy change that occurs when an acid and a base react together to form one mole of water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

effervescence

A

gas given off so visibly produces bubbles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

acid-base indicators

A

change color reversibly according to concentration of H+ ions in the solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Why do acid-base indicators work?

A
  • indicators are weak acids or bases whose conjugates have different colors
  • color change identifies pH of substance
  • usually aqueous or absorbed on test paper
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is the sign of a good indicator?

A

gives distinct or sharp color change at equivalence point

17
Q

litmus

A
  • best known acid-base indicator
  • dye derived from lichens
  • pink in presence of acid; blue in presence of alkalis
18
Q

universal indicator

A
  • several indicators mixed together
  • changes color many times across range of acids/alkalis
  • can be used to measure [H+] on pH scale
19
Q

acid-base titration

A
  • reacting together a carefully measured volume of one of solutions, and adding the other solution gradually
  • until reach equivalence point
20
Q

equivalence point

A

where an acid and base exactly neutralize each other

21
Q

What is the pH equation?

What is the [H+] equation?

A
  • pH = -log10[H+]
  • [H+] = 10-pH
22
Q

What are some of the features of the pH scale?

A
  • pH numbers usually positive
  • have no units
  • pH inversely related to [H+]
  • change of one pH unit represents a 10-fold change in [H+]
23
Q

What are the values of pH?

A
24
Q

pH meter

A
  • probe that directly reads [H+] through an electrode
  • have accuracy to several decimal points
  • must be calibrated before each use with buffer solution
  • must be standardized for temperature
25
Q

ionic product constant of water

A
  • Kw = [H+][OH-]
  • in pure water [H+] = [OH-​]
26
Q

Definitions of acidic, neutral, and alkali solutions by [H+]

A
  • acidic solutions [H+] > [OH-]
  • neutral solutions [H+] = [OH-]
  • alkaline solutions [H+] -]
27
Q

What is the relationship between [OH-] and [H+​]?

A

inversely proportional in aqueous solution

28
Q

strong acids/bases

A
  • ionize almost completely in solution
  • hydrochloric acid, nitric acid, sulfuric acid
  • lithium hydroxide, sodium hydroxide, potassium hydroxide, barium hydroxide
29
Q

weak acids/bases and examples

A
  • ionize only partially in solution
  • ethanoic acid, carbonic acid, phosphoric acid
  • ammonia, ethylamine
30
Q

How do you distinguish between strong acids/bases and weak acids/bases?

A
  • strong acids/bases have higher concentration of ions than weak acids/bases
  • can only compare concentrations at same temperature
31
Q

electrical conductivity of strong/weak acids/bases

A

strong acids/bases have higher conductivity than weak acids/bases as long as same concentrations compared

32
Q

rate of reaction of strong/weak acids/bases

A

strong acids/bases have greater rate of reaction

33
Q

pH of strong/weak acids/bases

A

pH can be used to directly compare strengths of acids (as long as of equal molar concentration)

Copy - IB Chemistry (23 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions