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Yr 11 Chemistry > U2- Acids + Bases > Flashcards

U2- Acids + Bases Flashcards

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1
Q

Bronsted-Lowry acid

A

a species that donates a proton, H+, during an acid-base reaction

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2
Q

general properties of acids

A

change colour of some indicators (exception eg is phenolphthalein indicator)
tend to be corrosive
sour
react w bases
pH<7
solutions can conduct electric current (bc covalent molecules can ionise and ions are free to move and carry e charge)

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3
Q

Bronsted-Lowry base

A

a species that accepts a proton, H+, during an acid-base reaction

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4
Q

alkali

A

soluble base that dissociates (splits up) hydroxide ions

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5
Q

general properties of bases

A 
red litmus -> blue
slippery
bitter
caustic (react w living tissue)
react w acids
pH>7 (alkali only)
solutions can conduct electric current (alkali only)
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6
Q

ionisation

A

process by which a chemical species gains or loses an electric charge

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7
Q

dissociation

A

process by which a molecule separates into smaller particles

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8
Q

acid + alkali

A

[BAWS] salt (aq) + water (l)

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9
Q

acid + metal

A

[MASH] salt (aq) + hydrogen gas (g)

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10
Q

acid + carbonate

A

[CAWCS] salt (aq) + carbon dioxide (g) + water (l)

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11
Q

conjugate acid-base pairs: NH3 (aq) + H2O (l)

A

NH3 (aq) + H2O (l) –> NH4+(aq) + OH-(aq)

base. acid. conj acid. conj base.

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12
Q

amphiprotic substances

A

can either donate or accept a proton, H+

eg H2O, HSO4-

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13
Q

monoprotic, diprotic, triprotic and polyprotic

A

species that donates one/two/three/multiple protons, H+, during ionisation

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14
Q

strength of acid and bases

A

how readily an acid or base donates or accepts a proton, H+

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15
Q

strong acids + egs

A 
undergo almost complete ionisation when added to water. Almost all acid molecules in solution will donate proton to form aqueous H+ ions
good conductors
eg sulfuric acid
hydrochloric acid
nitric acid
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16
Q

weak acids + eg

A 
does not readily donate a proton, H+, in a solution. More reactant acid molecules present I'm solution that product of H+ ions hence <-->
poor conductors
eg ammonium
ethanoic acid
carbonic acid
17
Q

strong bases

A 
readily accepts a proton, H+ and dissociates to form OH- ions and a basic solution in an acid-base reaction
eg O2-
OH-
HPO4 2-
H-
S2-
18
Q

weak bases + eg

A

doesn’t readily accept H+ ions. More reactant base molecules present in solution than product of OH- ions hence <–>
eg ammonia
sulphate
ethanoate

19
Q

strength vs concentration

A

strength of an acid/base relates to what proportion of its molecules will donate/accept a proton, H+
w/a
acid/base concentration depends on how many of those acid/base molecules were in the solution to begin with

20
Q

pH and pH scale

A

measure of the concentration of H3O+ ions in solution
values of pH arranged on a logarithmic scale

[OH-][H3O+] = 10^-14 M^2

21
Q

alkali

A

a soluble base

22
Q

pH formulas

A

(dilute a solution by factor of 10 to increase/decrease pH by 1)
pH = -log [H3O+]
pH = 14 + log [OH-]

23
Q

concentration from pH formulas

A

[H3O+] = 10 ^-pH
[OH-] = 10 ^pH-14
or
C1V1 = C2V2

24
Q

ionic product of water

A

Kw = [H3O+] x [OH-] = 1 x 10^-14

constant value tf as [H3O+] increases, [OH-] must decrease to maintain constant and vice versa

25
Q

acid dissociation constant, Ka

A

used to distinguish strong acids from weak acids (higher=stronger)
Ka = [H3O+][A-]
—————-
[HA]

26
Q

hydrolysis

A

chemical reaction where water is used to break the bonds of a substance

27
Q

acid-base reactions

A

chemical reaction where a proton, H+, is transferred between two chemical species

28
Q

ionic equation

A

simplified equations not including spectator ions

29
Q

spectator ions

A

aqueous ions which do not react and remain dissolved in a solution throughout a reaction

30
Q

conjugate acid/base

A

chemical species formed from a base/acid that has accepted/donated a proton, H+

31
Q

concentration

A

amount of chemical substance in a unit of volume

32
Q

concentrated vs dilute solution

A

relatively high vs relatively low amount of solute compared to the volume of solution

Yr 11 Chemistry (12 decks)

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