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MEHC U2 > Acids And Bases > Flashcards

Acids And Bases Flashcards

1
Q

What is an acid? (Arrhenius definition)

A

An acid is a substance that produces hydrogen ions in solution

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2
Q

Give an example of an acidic reaction for the Arrhenius definition of an acid

A

HCl –(H2O)–> H+ + Cl-

HCl dissolves (ionises) in water to H+ + Cl-

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3
Q

What is a base? (Arrhenius definition)

A

a base is a substance that produces hydroxide ions in solution

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4
Q

Give an example of a basic reaction (Arrhenius definition)

A

NaOH dissociates in water to form aqueous solution of Na+ ions and OH-

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5
Q

What is the Bronsted-Lowry model of acids and bases describe?

A

An acid reacting to form its conjugate base and a base reacting to form its conjugate acid

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6
Q

What is an acid? Bronsted-Lowry definition

A

Acid is a proton donor

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7
Q

What is a base?

Bronstd-Lowry definition

A

A base is a proton accepter

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8
Q

Give an example of a bronsted-Lowry model of acids and bases and also give an explanation to why it helps.

A

H-Cl + H2O ➡️ Cl- + H3O
(Acid) + (Base) ➡️ (Conjugate base of acid HCl) + (conjugate acid of H2O)

This model of acids and bases helps to explain why some substances are basic even though hydroxide ions are not produced in solution

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9
Q

What is an amphoteric?

A

A substance that can accept or donate a proton

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10
Q

What is an amphoteric substance?

A

Water is considered to be amphoteric as it can donate a proton to form an hydroxide ions or accept a proton to form the hydronic ion (H3O+)

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11
Q

What do acids taste like?

A

Sour

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12
Q

What do bases taste like?

A

Bitter

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13
Q

What colour does acids turn litmus?

A

Red

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14
Q

What colour do bases turn litmus?

A

Blue

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15
Q

What pH do acids have?

A

pH below 7 at 25C

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16
Q

What pH do bases have?

A

pH above 7 at 25C

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17
Q

Are acids sticky or slippery?

A

may feel sticky

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18
Q

Are bases sticky or slippery?

A

may feel slippery

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19
Q

Do acids and bases both conduct electricity when in solution?

A

YAS

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20
Q

Are both acids and bases corrosive?

A

YAS

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21
Q

What do acids react with?

A

React with metals, metal oxides, metal hydroxides, metal carbonates and metal hydrogen carbonates.

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22
Q

What do bases react with?

A

Reacts with acids, oils and fats

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23
Q

What are the 8 type of acid/base reactions?

A 
Acid and metal
Acid and metal hydroxide
Acid and metal oxide
Acid and carbonate
Acid and hydrogen carbonate 
Acid and metal sulfite
Base and ammonium salt
Base and non-metal oxide
24
Q

Acid and Metal —> ?

A

Acid and Metal —> Salt and H2 (gas)

eg. 2HCl(aq) + Ni(s)—> NiCl2(aq) + H2(g)

25
Acid and Metal Hydroxide ---> ?
Acid and Metal Hydroxide ---> Salt + H2O | eg. 2HNO3(aq) +Ca(OH)2(s) ---> Ca(NO3)2 (aq) + 2H2O (l)
26
Acid and Metal Oxide ---> ?
Acid and Metal Oxide ---> Salt + H2O | eg. H2SO4 + CuO ---> CuSO4 + H2O
27
Acid and Carbonate ---> ?
Acid and Carbonate ---> Salt + H2O + CO2
28
Acid and Hydrogen carbonate ---> ?
Acid and Hydrogen carbonate ---> Salt + H2O +CO2
29
Acid and Metal Sulfite ---> ?
Acid and Metal Sulfite ---> Salt + H2O + SO2 | eg. 2HCl(aq) + Na2SO3(s) ---> 2NaCl(aq) + H2O(l) + SO2(g)
30
Base and Ammonium salt ---> ?
Base and Ammonium salt ---> Salt + H2O +NH3(g) | eg. KOH(aq) + NH4Cl (aq) ---> KCl(aq) + H2O(l) + NH3(g)
31
Base + Non-Metal oxide (acid) ---> ?
Base + Non-Metal oxide (acid) ---> Salt + H2O eg. 2KOH(aq) + SO2(g) ---> K2SO3(aq) + H2O(l) 2NaOh(aq) + CO2(g) ---> H2O(l) + NaCO3
32
What is an indicator?
a substance that changes colour depending on the | concentration of hydronium (hydrogen) ions present.
33
What is pH?
pH is a measure of the hydronium (hydrogen) ion concentration in a solution and is calculated using the formula: pH = - log [H3O+]
34
What is the H3O+ concentration for ph 1, 2, 3
pH 1 = 1.Ox10^-1 pH 2 = 1.Ox10^-2 pH 1 = 1.Ox10^-3 The change of one pH unit is equivalent to a ten-fold change in the hydronium ion concentration
35
Give an example of when the concentration of hydronium ions is equal to the concentration of hydroxide ions
For pure water at 25C the concentration of hydronium ions is equal to the concentration of hydroxide ions and the pH is exactly 7. At 25C a pH of 7 is called neutral (neither acidic or basic).
36
What are some strong acids (6)
``` HCl H2SO4 HNO3 HI HBr HClO4 ```
37
What are some weak acids? (7)
``` H2SO3 H3PO4 HF CH3COOH H2CO3 Ammonium salts (NH4Cl, NH4NO3) ```
38
What are some strong bases? (4 types)
oxides of group 1 metals - Li2O - K2O - Na2O oxides of group 2 metals - MgO - CaO - BaO Hydroxides of group 1 metals - LiOH - NaOH - KOH Hydroxides of group 2 metals - Mg(OH)2 - Ba(OH)2
39
What are some weak bases? (4 types)
Metal Phosphates - Na3PO4 - K3PO4 Metal carbonates - Na2CO3 - K2CO3 metal hydrogen-carbonates - NaHCO3 - KHCO3 - Ca(HCO3)2 AMMONIA - NH3 - NH3OH
40
Are non-metal oxides are acidic? and also describe a reaction of non-metal oxides with water.
many non-metal oxides are acidic, though it is not immediately apparent from Arrhenius theory. Non-metal oxides like CO2 and SO3 combine with water to form acids then acids ionise to form H+ and acidic solution
41
Give an example of a reaction of non-metal oxides with water
When added to water, SO2 initially dissolves to form H2SO3 which then partially ionises forming hydrogen ions, this lowers the solutions pH. SO2 + H2O ↔️ H2SO3 then H2SO3 + H2O ↔️ H3O+ + HSO3- overall SO2 + 2H2O ↔️ H3O+ + HSO3-
42
Are metallic oxides basic or amphoteric like Na2O or CaO basic? and also describe a reaction of metallic oxides?
they are basic or amphoteric in nature and are not immediately obvious from Arrhenius theory. - Dissociation releases positive metal ions and O2- (aq) - - then rapidly combines with H2O to produce OH-(aq) - - when dissolve in H2O a metal oxide converts into a basic solution of corresponding metal hydroxide
43
Give a example of a reaction of a metallic oxides with water
Na2O dissolves.... Na2O(s) ---> 2Na+(aq) + O2- (aq) Oxides ion reacts with water.... O2-(aq) + H2O(l) ---> 2OH-(aq) Overall..... Na2O(s) + H2O (l) ----> 2Na+(aq) + 2OH- (aq)
44
What happens when the metallic oxide is insoluble?
CaO and MgO will absorb water to produce an hydroxide eg. CaO(s) + H2O ----> Ca(OH)2 (s) MgO(s) + H2O ----> Mg(OH)2 (s)
45
What is a polyprotic acid?
A polyprotic acid is one that has more than one acidic hydrogen atom eg. H2SO4 HSCO3 H3PO4
46
What is are strong electrolytes?
Strong acids and all ionic compounds
47
What are weak electrolytes?
Weak acids or bases
48
What is dissociation?
When an ionic solid dissolves in water
49
What is ionisation?
When a covalent molecular substance dissolves in water to form ions.
50
Why do partially ionised/dissociated reactions occur?
as a weak electrolyte or non-electrolyte is used
51
What are non-electrolytes?
most covalent molecular substances, as they don't conduct electricity when molten or in aqueous solution
52
What happens when an acid and ammonia react?
H attaches to the NH3 (not H2O) to produce NH4+ eg. HCl(aq) + NH3(aq) —-> NH4Cl(aq)
53
What happens when ammonia reacts with water?
Ammonia is considered a weak base due to the production of OH- ions when it reacts with water, NH3(g) + H2O(l) —> NH4+ + OH-
54
What happens when ammonium salt reacts with a base?
ammonium ion is considered to be a weak acid. Meaning it will react with a base to produce a salt and water, however ammonia gas will also be produced in the reaction NaOH + NH4Cl —> NaCl(aq) + NH3(g) +H2O
55
Name 6 acidic ions
``` NH4+ Al3+ Fe3+ HCO3- H2PO4- HSO4- ```
56
Name 3 basic ions. And a one weakly base.
SO4^2- CO3^2- HCO3- PO4^3-

MEHC U2 (8 decks)

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